Thermodynamics

1. The term “thermodynamics” comes from Greek words “therme” and “dynamis” which means _______. 

A. Heat power



B. Heat transfer



C. Heat energy



D. Heat motion

2. The term “thermodynamics” was first used in 1849 in the publication of a 

A. Rudolph Clausius



B. William Rankine



C. Lord Kelvin



D. Thomas Savery

3. What law asserts that energy is a thermodynamic property? 

A. First law of Thermodynamics



B. Second law of Thermodynamics



C. Third law of Thermodynamics



D. Zeroth law of Thermodynamics

4. What law asserts that energy has quality as well as quantity? 

A. First law of Thermodynamics



B. Second law of Thermodynamics



C. Third law of Thermodynamics



D. Zeroth law of Thermodynamics

5. The macroscopic approach to the study of thermodynamics does not require a knowledge of the behavior of individual particles is called _____. 

A. Dynamic thermodynamics



B. Static thermodynamics



C. Statistical thermodynamics



D. Classical thermodynamics

6. What is the more elaborate approach to the study of thermodynamics and based on the average behavior of large groups of individual particles? 

A. Dynamic thermodynamics



B. Static thermodynamics



C. Statistical thermodynamics



D. Classical thermodynamics

7. What is defined a region in space chosen for study? 

A. Surroundings



B. System



C. Boundary



D. Volume

8. The first law of thermodynamics is based on which of the following principles? 

A. Conservation of mass



B. Conservation of energy



C. Action and reaction



D. The entropy-temperature relationship

9. What is the mass or region outside the system called? 

A. Surroundings



B. Boundary



C. Volume



D. Environment

10. What is the real or imaginary surface that separates the system from its surroundings? 

A. Division



B. Wall



C. Boundary



D. Interface

11. A system which consists of fixed amount of mass and no mass can cross its boundary called _____. 

A. Equilibrium system



B. Thermal equilibrium system



C. Open system



D. Closed system

12. A system in which even energy is not allowed to cross the boundary is called ____. 

A. Closed system



B. Exclusive system



C. Isolated system



D. Special system

13. A system in which there is a flow of mass is known as _____. 

A. Equilibrium system



B. Isolated system



C. Open system



D. Closed system

14. Open system usually encloses which of the following devices? 

A. Compressor



B. Turbine



C. Nozzle



D. All of the above

15. The boundaries of a control volume, which may either real or imaginary is called _____. 

A. Control boundary



B. Control system



C. Interface



D. Control surface

16. Any characteristic of a thermodynamics system is called a _____. 

A. Property



B. Process



C. Phase



D. Cycle

17. How are thermodynamic properties classified? 

A. Physical and chemical



B. Intensive and extensive



C. Real and imaginary



D. Homogeneous and heterogeneous

18. The thermodynamic properties that are independent on the size of the system is called _____. 

A. Extensive property



B. Intensive property



C. Open property



D. Closed property

19. The thermodynamic properties that are dependent on the size or extent of the system is called _____. 

A. Extensive property



B. Intensive property



C. Open property



D. Closed property

20. Which is NOT an intensive property of thermodynamics? 

A. Temperature



B. Mass



C. Pressure



D. Density

21. Which is NOT an extensive property of thermodynamics? 

A. Density



B. Mass



C. Volume



D. Energy

22. Extensive properties per unit mass are called _____. 

A. Specific properties



B. Relative properties



C. Unit properties



D. Phase properties

23. A system is in ______ equilibrium if the temperature is the same throughout the entire system. 

A. Static



B. Thermal



C. Mechanical



D. Phase

24. A system is in ______ equilibrium if there is no change in pressure at any point of the system with time.



A. Pressure



B. Thermal



C. Mechanical



D. Phase

25. If a system involves two phases, it is in ______ equilibrium when the mass of each phase reaches an equilibrium level and stays there. 

A. Chemical



B. Thermal



C. Mechanical



D. Phase

26. A system is in ______ equilibrium of its chemical composition does not change with time, i.e., no chemical reaction occurs. 

A. Chemical



B. Thermal



C. Mechanical



D. Phase

27. “The state of a simple compressible system is completely specified by two independent, intensive properties”. This is known as ______. 

A. Equilibrium postulate



B. State postulate



C. Environment postulate



D. Compressible system postulate

28. What is the unit of the total energy of the system? 

A. Kj



B. Kj/Kg



C. Kg



D. g

29. Without electrical, mechanical, gravitational, surface tension and motion effects, a system is called _____ system.



A. Simple



B. Simple compressible



C. Compressible



D. Independent

30. What refers to any change that a system undergoes from one equilibrium state to another equilibrium state? 

A. Process



B. Path



C. Phase



D. Cycle

31. What refers to the series of state through which a system passes during a process? 

A. Path



B. Phase



C. Cycle



D. Direction

32. How many independent properties are required to completely fix the equilibrium state of a pure gaseous compound? 

A. 4



B. 3



C. 2



D. 1

33. What is a process in which the system remains infinitesimally closed to an equilibrium state at all times? 

A. Path equilibrium process



B. Cycle equilibrium process



C. Phase equilibrium process



D. Quasi-state or quasi- equilibrium process

34. A closed system may refer to ______. 

A. Control mass



B. Control volume



C. Control energy



D. Control temperature

35. An open system may refer to ______. 

A. Control mass



B. Control volume



C. Control energy



D. Control temperature

36. A system is said to be in thermodynamic equilibrium if it maintains ______ equilibrium. 

A. Mechanical and phase



B. Thermal and chemical



C. Thermal, mechanical and chemical



D. Thermal, phase, mechanical and chemical

37. What is a process with identical end states called? 

A. Cycle



B. Path



C. Phase



D. Either path or phase

38. What is a process during which the temperature remains constant? 

A. Isobaric process



B. Isothermal process



C. Isochoric process



D. Isometric process

39. What is a process during which the pressure remains constant? 

A. Isobaric process



B. Isothermal process



C. Isochoric process



D. Isometric process

40. What is a process during which the specific volume remains constant? 

A. Isobaric process



B. Isothermal process



C. Isochoric or isometric process



D. Isovolumetric process

41. The prefix “iso” used to designate a process means ______. 

A. Cannot be interchanged



B. Remains constant



C. Approximately equal



D. Slight difference

42. What does the term “steady” implies? 

A. No change with volume



B. No change with time



C. No change with location



D. No change with mass

43. What does the tem “uniform” implies? 

A. No change with volume



B. No change with time



C. No change with location



D. No change with mass

44. What is defined as a process during which a fluid flows through a control volume steadily? 

A. Transient-flow process



B. Steady and uniform process



C. Uniform-flow process



D. Steady-flow process

45. The sum of all the microscopic form of energy is called _____. 

A. Total energy



B. Internal energy



C. System energy



D. Phase energy

46. What type of system energy is related to the molecular structure of a system? 

A. Macroscopic form of energy



B. Microscopic form of energy



C. Internal energy



D. External energy

47. What form of energy refers to those a system possesses as a whole with respect to some outside reference frame, such as potential and kinetic energies? 

A. Macroscopic form of energy



B. Microscopic form of energy



C. Internal energy



D. External energy

48. Who coined the word “energy” in 1807? 

A. William Rankine



B. Rudolph Clausius



C. Lord Kelvin



D. Thomas Young

49. The molecules of a gas moving through space with some velocity possesses what kind of energy? 

A. Translational energy



B. Spin energy



C. Rotational kinetic energy



D. Sensible energy

50. The electrons in an atom which rotate about the nucleus possess what kind of energy? 

A. Translational energy



B. Spin energy



C. Rotational kinetic energy



D. Sensible energy

51. The electrons which spins about its axis will possess what kind of energy? 

A. Translational energy



B. Spin energy



C. Rotational kinetic energy



D. Sensible energy

52. What refers to the portion of the internal energy of a system associated with the kinetic energies of the molecules? 

A. Translational energy



B. Spin energy



C. Rotational kinetic energy



D. Sensible energy

53. What is the internal energy associated with the phase of a system called? 

A. Chemical energy



B. Latent energy



C. Phase energy



D. Thermal energy

54. What is the internal energy associated with the atomic bonds in a molecule called? 

A. Chemical energy



B. Latent energy



C. Phase energy



D. State energy

55. What is the extremely large amount of energy associated with the strong bonds within the nucleus of the atom itself called? 

A. Chemical energy



B. Latent energy



C. Phase energy



D. Nuclear energy

56. What are the only two forms of energy interactions associated with a closed system? 

A. Kinetic energy and heat



B. Heat transfer and work



C. Thermal energy and chemical energy



D. Latent energy and thermal energy

57. What states that if two bodies are in thermal equilibrium with a third body, they are also in equilibrium with each other? 

A. Zeroth law of thermodynamics



B. First law of thermodynamics



C. Second law of thermodynamics



D. Third law of thermodynamics

58. Who formulated the zeroth law of thermodynamics in 1931? 

A. A. Celsuis



B. A. Einstein



C. R.H. Fowler



D. G. Fahrenheit

59. What is the thermodynamic temperature scale in the SI system? 

A. Kelvin scale



B. Celsius scale



C. Fahrenheit scale



D. Rankine scale

60. What is the thermodynamic temperature scale in the English system? 

A. Kelvin scale



B. Celsius scale



C. Fahrenheit scale



D. Rankine scale

61. What temperature scale is identical to the Kelvin scale? 

A. Ideal gas temperature scale



B. Ideal temperature scale



C. Absolute gas temperature scale



D. Triple point temperature scale

62. The temperatures of the ideal gas temperature scale are measured by using a ______. 

A. Constant-volume gas thermometer



B. Constant-mass gas thermometer



C. Constant-temperature gas thermometer



D. Constant-pressure gas thermometer

63. What refers to the strong repulsion between the positively charged nuclei which makes fusion reaction difficult to attain? 

A. Atomic repulsion



B. Nuclear repulsion



C. Coulomb repulsion



D. Charge repulsion

64. What gas thermometer is based on the principle that at low pressure, the temperature of a gas is proportional to its pressure at constant volume? 

A. Constant-pressure gas thermometer



B. Isobaric gas thermometer



C. Isometric gas thermometer



D. Constant-volume gas thermometer

65. What is the state at which all three phases of water coexist in equilibrium? 

A. Tripoint of water



B. Triple point of water



C. Triple phase point of water



D. Phase point of water

66. What is defined as the force per unit area? 

A. Pressure



B. Energy



C. Work



D. Power

67. The unit “pascal” is equivalent to ______. 

A. N/m^2



B. N/m



C. N-m



D. N-m^2

68. Which of the following is NOT a value of the standard atmospheric pressure? 

A. 1 bar



B. 1 atm



C. 1 kgf/cm^2



D. 14.223 psi

69. What is the SI unit of pressure? 

A. Atm



B. Bar



C. Pa



D. Psi

70. 1 bar is equivalent to how many pascals? 

A. 10^3



B. 10^4



C. 10^5



D. 10^6

71. 1 atm is equivalent to how many pascals? 

A. 101,325



B. 101,689



C. 101,102



D. 101,812

72. What is considered as the actual pressure at a given position and is measured relative to absolute vacuum? 

A. Gage pressure



B. Absolute pressure



C. Atmospheric pressure



D. Vacuum pressure

73. What is the pressure below atmospheric pressure called? 

A. Gage pressure



B. Absolute pressure



C. Atmospheric pressure



D. Vacuum pressure

74. The difference between the absolute pressure and the atmospheric pressure is called the _____ pressure. 

A. Gage



B. Normal



C. Standard



D. Vacuum

75. Which of the following is NOT an instrument used to measure pressure? 

A. Bourdon tube



B. Pitot tube



C. Aneroid



D. Manometer

76. What instrument is used to measure atmospheric pressure? 

A. Pitot tube



B. Wind vane



C. Barometer



D. Manometer

77. Another unit used to measure atmospheric pressure is the “torr”. This is named after the Italian physicist, Evangelista Torrecelli. An average atmospheric pressure is how many torr? 

A. 740



B. 750



C. 760



D. 770

78. What states that for a confined fluid, the pressure at a point has the same magnitude in all directions? 

A. Avogadro’s Law



B. Amagat Law



C. Pascal’s Law



D. Bernoulli’s Theorem

79. What pressure measuring device consists of a coiled hollow tube that tends to straighten out when the tube is subjected to an internal pressure? 

A. Aneroid



B. Manometer



C. Bourdon pressure gage



D. Barometer

80. What is an energy that can be transferred from one object to another causing a change in temperature of each object? 

A. Power



B. Heat transfer



C. Heat



D. Work

81. What is the SI unit of energy?



A. Newton



B. Btu



C. Calorie



D. Joule

82. One joule is equivalent to one _____. 

A. Kg ∙ m/ s^2



B. Kg ∙ m^2/s^2



C. Kg ∙ m^2/s



D. Kg ∙ m/s

83. One calorie is equivalent to how many joules? 

A. 4.448



B. 4.184



C. 4.418



D. 4.814

84. One erg is equivalent to how many joules? 

A. 10^-8



B. 10^-7



C. 10^-6



D. 10^-5

85. The first law of thermodynamics is the: 

A. Law of conservation of momentum



B. Law of conservation of mass



C. Law of conservation of power



D. Law of conservation of energy

86. What is the study of energy and its transformations?



A. Thermostatics



B. Thermophysics



C. Thermochemistry



D. Thermodynamics

87. What is considered as the heat content of a system? 

A. Enthalpy



B. Entropy



C. Internal heat



D. Molar heat

88. What refers to the amount of heat needed to raise the temperature of an object by one degree Celsius or 1K? 

A. Heat capacity



B. Specific heat



C. Latent heat



D. Molar heat

89. What is the heat capacity of one mole of substance? 

A. Molecular heat



B. Specific heat



C. Latent heat



D. Molar heat

90. What is the heat capacity of one gram of a substance? 

A. Molecular heat



B. Specific heat



C. Latent heat



D. Molar heat

91. “The enthalpy change for any chemical reaction is independent of the intermediate stages, provided the initial and final conditions are the same for each route.” This statement is known as:



A. Dulong’s Law



B. Dalton’s Law



C. Hess’s Law



D. Petit Law

92. What refers to the measure of the disorder present in a given substance or system? 

A. Enthalpy



B. Entropy



C. Heat capacity



D. Molar heat

93. Entropy is measured in ______. 

A. Joule/Kelvin



B. Joule-Meter/Kelvin



C. Meter/Kelvin



D. Newton/Kelvin

94. What is the energy absorbed during chemical reaction under constant volume conditions? 

A. Entropy



B. Ion exchange



C. Enthalpy



D. Enthalpy of reaction

95. When water exists in the liquid phase and is not about to vaporize, it is considered as _____liquid. 

A. Saturated



B. Compressed or subcooled



C. Superheated



D. Unsaturated

96. A liquid that is about to vaporize is called ______ liquid. 

A. Saturated



B. Compressed or subcooled



C. Superheated



D. Unsaturated

97. A vapor that is about to condense is called ______ vapor. 

A. Saturated



B. Compressed or subcooled



C. Superheated



D. Unsaturated

98. A vapor that is not about to condense is called _____ vapor. 

A. Saturated



B. Compressed or subcooled



C. Superheated



D. Unsaturated

99. A substance that has a fixed chemical composition is known as ______ substance. 

A. Monoatomic



B. Heterogeneous



C. Homogeneous



D. Pure

100. What refers to the temperature at which a pure substance changes phase at a given pressure? 

A. Equilibrium temperature



B. Saturation temperature



C. Superheated temperature



D. Subcooled temperature

101. What refers to the pressure at which a pure substance changes phase at a given temperature? 

A. Equilibrium pressure



B. Saturation pressure



C. Superheated pressure



D. Subcooled pressure

102. What is the amount of heat needed to turn 1 kg of the substance at its melting point from the solid to liquid state? 

A. Heat of fusion



B. Heat of vaporation



C. Heat of condensation



D. Heat of fission

103. What is the amount of heat needed to turn 1kg of the substance at its boiling point from the liquid to the gaseous state? 

A. Heat of fusion



B. Heat of vaporation



C. Heat of condensation



D. Heat of fission

104. What refers to the amount of energy absorbed or released during a phase-change process? 

A. Molar heat



B. Latent heat



C. Vaporization heat



D. Condensation heat

105. What is the latent heat of fusion of water at 1 atm?



A. 331.1 kJ/kg



B. 332.6 kJ/kg



C. 333.7 kJ/kg



D. 330.7 kJ/kg

106. What is the latent heat of vaporization of water at 1 atm? 

A. 2314.8 kJ/kg



B. 2257.1 kJ/kg



C. 2511.7 kJ/kg



D. 2429.8 kJ/kg

107. What refers to the point at which the saturated liquid and saturated vapor states are the same or identical? 

A. Triple point



B. Inflection point



C. Maximum point



D. Critical point

108. What is defined as the direct conversion of a substance from the solid to the vapor state or vice versa without passing the liquid state? 

A. Condensation



B. Vaporization



C. Sublimation



D. Cryogenation

109. The amount of heat required to raise the temperature of 1kg of water through 1 °C is called ______. 

A. Calorie



B. Joule



C. BTU



D. Kilocalorie

110. The amount of heat required to raise the temperature of 1 pound of water by 1°F is called ______. 

A. Calorie



B. Joule



C. BTU



D. Kilocalorie

111. 1 British thermal unit (BTU) is equivalent to how many joules? 

A. 1016



B. 1043



C. 1023



D. 1054

112. The term “enthalpy” comes from Greek “enthalpen” which means ______. 

A. Warm



B. Hot



C. Heat



D. Cold

113. The ratio of the mass of vapor to the total mass of the mixture is called ______. 

A. Vapor ratio



B. Vapor content



C. Vapor index



D. Quality

114. The “equation of state” refers to any equation that relates the ______ of the substance. 

A. Pressure and temperature



B. Pressure, temperature and specific weight



C. Temperature and specific weight



D. Pressure, temperature and specific volume

115. In the equation Pv = RT, the constant of proportionality R is known as ______. 

A. Universal gas constant



B. Gas constant



C. Ideal gas factor



D. Gas index

116. The gas constant of a certain gas is the ratio of: 

A. Universal gas constant to molar mass



B. Universal gas constant to atomic weight



C. Universal gas constant to atomic number



D. Universal gas constant to number of moles

117. What is the value of the universal gas constant in kJ/kmol ∙ K? 

A. 10.73



B. 1.986



C. 8.314



D. 1545

118. The mass of one mole of a substance in grams is known as ______. 

A. Molar weight



B. Molar mass



C. Molar volume



D. Molar constant

119. What is defined as the energy required to raise the temperature of a unit mass of a substance by one degree?



A. Latent heat of fusion



B. Molar heat



C. Specific heat capacity



D. Specific heat

120. The ______ of a substance is the amount of heat that must be added or removed from a unit mass of the substance to change its temperature by one degree. 

A. Latent heat of fusion



B. Molar heat



C. Specific heat capacity



D. Specific heat

121. What is the specific heat capacity of water in J/kg ∙°C? 

A. 4581



B. 4185



C. 4518



D. 4815

122. What is the SI unit of specific heat capacity? 

A. J/kg



B. J/kg∙ °F



C. J/kg∙ °C



D. J/°C

123. What is constant for a substance that is considered “incompressible”? 

A. Specific volume of density



B. Pressure



C. Temperature



D. All of the above

124. If there is no heat transferred during the process, it is called a ______ process. 

A. Static



B. Isobaric



C. Polytropic



D. Adiabatic

125. The term “adiabatic” comes from Greek “adiabatos” which means ______. 

A. No heat



B. No transfer



C. Not to be passed



D. No transformation

126. How is heat transferred? 

A. By conduction



B. By convection



C. By radiation



D. All of the above

127. What refers to the transfer of energy due to the emission of electromagnetic waves or photons? 

A. Conduction



B. Convection



C. Radiation



D. Electrification

128. What refers to the transfer of energy between a solid surface and the adjacent fluid that is in motion? 

A. Conduction



B. Convection



C. Radiation



D. Electrification

129. What refers to the transfer of energy from the more energetic particles of a substance to the adjacent less energetic ones as a result of interaction between particles? 

A. Conduction



B. Convection



C. Radiation



D. Electrification

130. What states that the net mass transfer to or from a system during a process is equal to the net change in the total mass of the system during that process? 

A. Third law of thermodynamics



B. Conservation of energy principle



C. Second law of thermodynamic



D. Conservation of mass principle

131. Which of the following statements is TRUE for an ideal gas, but not for a real gas? 

A. PV = nRT



B. An increase in temperature causes an increase in the kinetic energy of the gas



C. The total volume of molecules on a gas is nearly the same as the volume of the gas as a whole



D. No attractive forces exists between the molecule of a gas

132. How does an adiabatic process compare to an isentropic process? 

A. Adiabatic heat transfer is not equal to zero; isentropic heat transfer is zero



B. Both heat transfer = 0; isentropic: reversible



C. Adiabatic heat transfer = 0; isentropic: heat transfer is not equal to zero



D. Both heat transfer is not equal to zero; isentropic: irreversible

133. Which of the following is the Ideal gas law (equation)? 

A. V/T = K



B. V= k*(1/P)



C. P1/T1 = P2/T2



D. PV = nRT

134. What is a measure of the ability of a material to conduct heat? 

A. Specific heat capacity



B. Coefficient of thermal expansion



C. Coefficient of thermal conductivity



D. Thermal conductivity

135. What refers to the heating of the earth’s atmosphere not caused by direct sunlight but by infrared light radiated by the surface and absorbed mainly by atmospheric carbon dioxide? 

A. Greenhouse effect



B. Global warming



C. Thermal rise effect



D. Ozone effect

136. What is a form of mechanical work which is related with the expansion and compression of substances? 

A. Boundary work



B. Thermodynamic work



C. Phase work



D. System work

137. Thermal radiation is an electromagnetic radiation with wavelengths in _____ range.



A. 1 to 100 µm



B. 0.1 to 100 µm



C. 0.1 to 10 µm



D. 10 to 100 µm

138. What refers to the rate of thermal radiation emitter per unit area of a body? 

A. Thermal conductivity



B. Absorptivity



C. Emissivity



D. Emissive power

139. What states that for any two bodies in thermal equilibrium, the ratios of emissive power to the absorptivity are equal? 

A. Kirchhoff’s radiation law



B. Newton’s law of cooling



C. Stefan-Boltzmann law



D. Hess’s law

140. What is considered as a perfect absorber as well as a perfect emitter? 

A. Gray body



B. Black body



C. Real body



D. White body

141. What is a body that emits a constant emissivity regardless of the wavelength? 

A. Gray body



B. Black body



C. Real body



D. White body

142. At same temperatures, the radiation emitted by all real surfaces is ______ the radiation emitted by a black body. 

A. Less than



B. Greater than



C. Equal to



D. Either less than or greater than

143. Which is NOT a characteristic of emissivity? 

A. It is high with most nonmetals



B. It is directly proportional to temperature



C. It is independent with the surface condition of the material



D. It is low with highly polished metals

144. What is the emissivity of a black body? 

A. 0



B. 1



C. 0.5



D. 0.25

145. What is the absorptivity of a black body? 

A. 0



B. 1



C. 0.5



D. 0.25

146. What is sometimes known as the “Fourth-power law”? 

A. Kirchhoff’s radiation law



B. Newton’s law of cooling



C. Stefan-Boltzmann law



D. Hess’s law

147. What states that the net change in the total energy of the system during a process is equal to the difference between the total energy entering and the total energy leaving the system during that process? 

A. Third law of thermodynamics



B. Conservation of energy principle



C. Second law of thermodynamics



D. Conservation of mass principle

148. The equation Ein – Eout = ∆Esystem is known as ______. 

A. Energy conservation



B. Energy equation



C. Energy balance



D. Energy conversion equation

149. What remains constant during a steady-flow process? 

A. Mass



B. Energy content of the control volume



C. Temperature



D. Mass and energy content of the control volume

150. Thermal efficiency is the ratio of: 

A. Network input to total heat input



B. Network output to total heat output



C. Network output to total heat input



D. Network input to total heat output

151. What law states that it is impossible to operate an engine operating in a cycle that will have no other effect than to extract heat from a reservoir and turn it into an equivalent amount of work?



A. Zeroth law of thermodynamics



B. First law of thermodynamics



C. Second law of thermodynamics



D. Third law of thermodynamics

152. Which statement of the second law of thermodynamics states that no heat engine can have a thermal efficiency of 100 percent? 

A. Kelvin-Planck statement



B. Clausius statement



C. Kevin statement



D. Rankine statement

153. What is the ratio of the useful heat extracted to heating value? 

A. Combustion efficiency



B. Phase efficiency



C. Heat efficiency



D. Work efficiency

154. What is defined as the ratio of the net electrical power output to the rate of fuel energy input? 

A. Combustion efficiency



B. Thermal efficiency



C. Overall efficiency



D. Furnace efficiency

155. What refers to the amount of heat removed from the cooled space in BTS’s for 1 watt-hour of electricity consumed? 

A. Cost efficiency rating



B. Energy efficiency rating



C. Coefficient of performance



D. Cost of performance

156. What law states that it is impossible to build a device that operates in a cycle and produces no effect other than the transfer of heat from a lowertemperature body to a higher-temperature body? 

A. Zeroth law of thermodynamics



B. First law of thermodynamics



C. Second law of thermodynamics



D. Third law of thermodynamics

157. What statement of the second law of thermodynamics states that it is impossible to build a device that operates in a cycle and produces no effect other than the transfer of heat from a lower-temperature body to a highertemperature body? 

A. Kelvin-Planck statement



B. Clausius statement



C. Kelvin statement



D. Rankine statement

158. A device that violates either the first law of thermodynamics or the second law of thermodynamics is known as _____. 

A. Ambiguous machine



B. Universal machine



C. Perpetual-motion machine



D. Unique machine

159. A device that violates the first law of thermodynamics is called a _____. 

A. Perpetual-motion machine of the first kind



B. Universal machine of the first kind



C. Ambiguous machine of the first kind



D. Unique machine of the first kind

160. A device that violates the second law of thermodynamics is called a ______. 

A. Perpetual motion machine of the second kind



B. Universal machine of the second kind



C. Ambiguous machine of the second kind



D. Unique machine of the second kind

161. Carnot cycle is the best known reversible cycle which was first proposed in what year? 

A. 1842



B. 1824



C. 1832



D. 1834

162. Who proposed the Carnot cycle? 

A. Sammy Carnot



B. Sonny Carnot



C. Sadi Carnot



D. Suri Carnot

163. The Carnot cycle is composed of how many reversible processes? 

A. 2



B. 3



C. 4



D. 5

164. The Carnot cycle is composed of ______ processes. 

A. One isothermal and one adiabatic



B. One isothermal and two adiabatic



C. Two isothermal and one adiabatic



D. Two isothermal and two adiabatic

165. What is the highest efficiency of heat engine operating between the two thermal energy reservoirs at temperature limits?



A. Ericson efficiency



B. Otto efficiency



C. Carnot efficiency



D. Stirling efficiency

166. What is a heat engine that operates on the reversible Carnot cycle called? 

A. Carnot heat engine



B. Ideal heat engine



C. Most efficient heat engine



D. Best heat engine

167. What states that thermal efficiencies of all reversible heat engines operating between the same two reservoirs are the same and that no heat engine is more efficient than a reversible one operating between the same two reservoirs? 

A. Ericson principle



B. Carnot principle



C. Otto principle



D. Stirling principle

168. Who discovered the thermodynamic property “Entropy” in 1865? 

A. Zeroth law of thermodynamics



B. First law of thermodynamics



C. Second law of thermodynamics



D. Third law of thermodynamics

169. A process during which entropy remains constant is called ______ process 

A. Isometric



B. Isochoric



C. Isobaric



D. Isentropic

170. “A reversible adiabatic process is necessarily isentropic but an isentropic process is not necessarily reversible adiabatic process.” This statement is: 

A. True



B. False



C. May be true and may be false



D. Absurd

171. The term “isentropic process” used in thermodynamics implies what? 

A. Reversible adiabatic process



B. Externally reversible, adiabatic process



C. Internally reversible, adiabatic process



D. Irreversible adiabatic process

172. What states that the entropy of a pure crystalline substance at absolute zero temperature is zero? 

A. Zeroth law of thermodynamics



B. First law of thermodynamics



C. Second law of thermodynamics



D. Third law of thermodynamics

173. What law provides an absolute reference point for the determination of entropy? 

A. Zeroth law of thermodynamics



B. First law of thermodynamics



C. Second law of thermodynamics



D. Third law of thermodynamics

174. “The entropy change of a system during a process is equal to the net entropy transfer through the system boundary and the entropy generated within the system”. This statement is known as: 

A. Entropy generation



B. Entropy change of a system



C. Entropy balance relation



D. Third law of thermodynamics

175. What law states that entropy can be created but it cannot be destroyed? 

A. Zeroth law of thermodynamics



B. First law of thermodynamics



C. Second law of thermodynamics



D. Third law of thermodynamics

176. Entropy is transferred by ______. 

A. Work



B. Heat



C. Energy



D. Work and heat

177. During adiabatic, internally reversible process, what is true about the change in entropy? 

A. It is temperature-dependent



B. It is always greater than zero



C. It is always zero



D. It is always less than zero

178. Water boils when: 

A. Its saturated vapor pressure equals to the atmospheric pressure



B. Its vapor pressure equals 76cm of mercury



C. Its temperature reaches 212 degree Celsius



D. Its vapor pressure is 1 gram per sq. cm

179. Which of the following is standard temperature and pressure (STP)? 

A. 0 degree Celsius and one atmosphere



B. 32 degree Fahrenheit and zero pressure



C. 0 degree Kelvin and one atmosphere



D. 0 degree Fahrenheit and zero pressure

180. What is the value of the work done for a closed, reversible isometric system? 

A. Zero



B. Positive



C. Negative



D. Positive or negative

181. “At constant pressure, the volume of a gas is inversely proportional to the pressure”. This is known as ______. 

A. Boyle’s Law



B. Charles’s Law



C. Gay-Lussac Law



D. Ideal gas law

182. Which of the following is the mathematical representation of the Charles’s law? 

A. V1/V2= P2/P1



B. V1/T1=V2/T2



C. V1/T2=V2/T1



D. V1/V2=√P2/√P1

183. Which of the following is the formula for thermal resistance?



A. Thickness of material/ thermal conductivity of material



B. 2(thickness of material)/thermal conductivity of material



C. Thickness of material/ 2(thermal conductivity of material)



D. Thickness of material x thermal conductivity of material

184. In the process of radiation, energy is carried by electromagnetic waves. What is the speed of electromagnetic waves? 

A. 182,000 miles/second



B. 184,000 miles/second



C. 186,000 miles/second



D. 188,000 miles/second

185. For heat engine operating between two temperatures (T1>T2), what is the maximum efficiency attainable? 

A. Eff = 1 – (T2/T1)



B. Eff = 1 - (T1/T2)



C. Eff = T1 - T2



D. Eff = 1 - (T2/T1)^2

186. Which one is the correct relation between energy efficiency ratio (EER) and coefficient of performance (COP)? 

A. EER = 2.34 COP



B. EER = 3.24 COP



C. EER = 3.42 COP



D. EER = 4.23 COP

187. The coefficient of performance (COP) is the ratio between the: 

A. Power consumption in watts and heat absorbed per hour



B. Heat absorbed per hour and the power consumption in watts



C. Work required and the absorbed heat



D. Absorbed heat and work required

188. What predicts the approximate molar specific heat at high temperatures from the atomic weight? 

A. Third law of thermodynamics



B. Law of Dulong and Petit



C. Mollier diagram



D. Pressure-enthalpy diagram

189. Considering one mole of any gas, the equation of state of ideal gases is simply the ______ law. 

A. Gay-Lussac law



B. Dulong and Petit



C. Avogadro’s



D. Henry’s

190. An ideal gas whose specific heats are constant is called _____. 

A. Perfect gas



B. Natural gas



C. Artificial gas



D. Refined gas

191. What are the assumptions of the kinetic gas theory? 

A. Gas molecules do not attract each other



B. The volume of the gas molecules is negligible compared to the volume of the gas



C. The molecules behave like hard spheres



D. All of the above

192. “The total volume of a mixture of non-reacting gases is equal to the sum of the partial volumes.” This statement is known as ______. 

A. Law of Dulong and Petit



B. Maxwell-Boltzmann law



C. Amagat’s law



D. Avogadro’s law

193. An adiabatic process in which there is no change in system enthalpy but for which there is a significant decrease in pressure is called _____. 

A. Isochoric process



B. Isobaric process



C. Throttling process



D. Quasistatic process

194. What is defined as the ratio of the change in temperature to the change in pressure when a real gas is throttled? 

A. Rankine coefficient



B. Kelvin coefficient



C. Maxwell-Boltzmann coefficient



D. Joule-Thomson coefficient

195. The low temperature reservoir of the heat reservoirs is known as ______. 

A. Source reservoir



B. Heel reservoir



C. Toe reservoir



D. Sink reservoir

196. A ______ is a flow in which the gas flow is adiabatic and frictionless and entropy change is zero. 

A. Isentropic flow



B. Isobaric flow



C. Steady flow



D. Uniform flow

197. What refers to the minimum temperature at which combustion can be sustained?



A. Burn temperature



B. Kindle temperature



C. Spark temperature



D. Ignition temperature

198. What law predicts the dew point of moisture in the fuel gas? 

A. Dalton’s law



B. Law of Dulong and Petit



C. Ringelman law



D. Amagat’s law

199. What law states that one energy from can be converted without loss into another form? 

A. Amagat’s law



B. Joule’s law



C. Lussac’s law



D. Henry’s law

200. Which is NOT a correct statement? 

A. A superheated vapor will not condense when small amount of heat re removed



B. An ideal gas is a gas that is not a superheated vapor



C. A saturated liquid can absorb as much heat as it can without vaporizing



D. Water at 1 atm and room temperature is subcooled

201. Thermodynamics is the study of heat and its transformation which stems from Greek words meaning _________. 

a. transformation of heat



b. transformation of energy



c. movement of heat



d. movement of matter

202. What is the Si unit for temperature? 

a. Kelvin



b. Celsius



c. Fahrenheit



d. Rankine

203. The energy that flows from higher temperature object to a lower temperature object because of the difference in temperature is called 

a. heat



b. temperature



c. thermodynamics cycle



d. energy flow

204. The amount of heat energy per kilogram that must be added or removed when a substance changes from one phase to another. 

a. specific heat



b. heat of expansion



c. latent heat



d. useful heat

205. The change in physical size of a substance when its temperature changes. 

a. intensive property



b. extensive property



c. volume expansion



d. thermal expansion

206. A stress which develops within an object when it attempts to expand or contract in response to a temperature changes, but cannot, due to being held rigidly in place. 

a. elongation



b. thermal stress



c. expansion contraction



d. thermal expansion

207. The energy associated with individual molecules in a gas, liquid or solid. 

a. Specific Energy



b. Molecular Energy



c. Internal Energy



d. Phase Energy

208. The heat Q per unit mass per degree change in temperature that must be supplied or removed to change the temperature of a substance. 

a. Specific Heat Capacity



b. Latent Heat



c. Heat of Transformation



d. Internal Heat

209. The pressure of the vapor phase of a substance that is in equilibrium with the liquid or solid phase. 

a. Phase Pressure



b. Equilibrium Vapor Pressure



c. Specific Pressure



d. Equilibrium Phase Pressure

210. Vapor pressure depends only on _________. 

a. pressure



b. force



c. volume



d. temperature

211. A plot of pressure vs. temperature for a given substance showing the various phases possible for that particular substance. 

a. Phase diagram



b. P-T diagram



c. Wein Diagram



d. Histogram

212. _________ is the grand total of all energies inside a substance. 

a. Internal Energy



b. Grand Energy



c. Atomic Energy



d. Elemental Energy

213. The _________ is defined as the amount of heat required to change the temperature of 1 gram of water by 1 Celsius degree. 

a. specific heat



b. latent heat



c. Joule



d. calorie

214. _________ is a measure of the average kinetic energy per molecule in a substance. 

a. movement



b. temperature



c. heat



d. mass

215. _________ the very small KE still present in molecules at absolute zero temperature. 

a. internal KE



b. Atomic kinetic energy



c. Zero-Point Energy



d. Subliminal Energy

216. Convert the change of temperature from 20˚C to 30˚C to Kelvin scale. 

a. 10 K



b. 293 K



c. 303 K



d. 273 K

217. _________ is a thermodynamic potential which measures the “useful” work obtainable from a closed thermodynamic system at a constant temperature and volume. 

a. useful work



b. energy consumed



c. Helmholtz free energy



d. Kinetic Energy

218. How much will the length of a 1.0 km section of concrete highway change if the temperature varies from -15˚C in winter to 41˚C in summer? 

a. 0.67 m



b. 2.2 m



c. 3.1 m



d. 0.47 m

219. Two 12 ft. sections of aluminum siding are placed end to end on the outside wall of house. How large a gap should be left between the pieces to prevent buckling if the temperature can change by 55˚C? 

a. 0.21 m



b. 0.18 m



c. 0.31 in



d. 0.18 in

220. What is the amount of radiant energy received each second over each square meter that is at right angles to the sun’s rays at the top of the atmosphere? 

a. 1400 J



b. 6000 J



c. 10000 J



d. 800 J

221. _________ is a thermodynamic potential that measures the “useful” or process-initiating work obtainable from an isothermal, isobaric thermodynamic system. 

a. Du-Pont Potential



b. Gibbs free energy



c. Rabz-Eccles Energy



d. Claussius Energy

222. All the energy we consume ultimately becomes _________. 

a. heat



b. depleted



c. exhausted



d. work

223. _________is the partial pressure of water vapor at the existing temperature divided by the equilibrium vapor pressure of water at the existing temperature. 

a. vacuum pressure



b. relative humidity



c. absolute pressure



d. vapor pressure

224. _________ is the transition of a given substance from the solid to the gas phase with no intermediate liquid stage. 

a. Convection



b. Conduction



c. Radiation



d. Sublimation

225. A process in which heat energy is transferred by the flow of fluid. 

a. Convection



b. Conduction



c. Radiation



d. Sublimation

226. In order to use a substance to make a thermometer the substance must _________ with a temperature change. 

a. expand



b. contract



c. change



d. increase

227. For most solids, the coefficient of volume expansion is _________ the coefficient of linear expansion. 

a. unrelated to



b. proportional to



c. twice



d. three times

228. The volume of a given amount of water _________ as the temperature decreases from 4˚C to 0˚C. 

a. decreases



b. increases



c. remains constant



d. none of the above

229. The gas in a constant gas thermometer cooled to absolute zero would have _________. 

a. no volume



b. no pressure



c. zero temperature at all scales



d. none of the above

230. On a day when the partial pressure of water vapor remains constant, what happens as the temperature rises? 

a. the relative humidity increases



b. the relative humidity decreases



c. the relative humidity remains constant



d. the air would eventually become saturated

231. The flow of a fluid when heat is transferred by convection. 

a. placidity



b. mass flow



c. convection current



d. heat transfer

232. An idealized perfect absorber and perfect emitter of radiation. 

a. elastic material



b. transponder material



c. Teflon



d. blackbody

233. A process by which heat is transferred through a material without a bulk movement of the material.



a. Convection



b. Conduction



c. Radiation



d. Emission

234. Is the amount of a substance that contains Avogadro’s number of atoms/molecules. 

a. mass



b. matter



c. gram-mole



d. volume

235. The distribution of particle speeds in an ideal gas at a given temperature. 

a. velocity of propagation



b. escape velocity



c. Maxwell speed Distribution



d. terminal velocity

236. A convection process in which an external device, such as a fan, is used to produce the fluid flow. 

a. Forced Convection



b. External Convection



c. Placid Convection



d. Thermionic Convection

237. A _________ is a quantity whose value at any state is independent of the path or process used to reach that state. 

a. cycle



b. path function



c. point function



d. process

238. A _________ is a quantity whose value depends on the path followed during a particular change in state. 

a. path function



b. point function



c. process



d. cycle

239. The contact surface shared by both the system and the surroundings is called _________. 

a. wall



b. boundary



c. interface



d. intersection

240. A closed system is also known as _________. 

a. isolated system



b. closed container



c. control mass



d. control volume

241. Open system is also known as _________. 

a. isolated system



b. closed container



c. control mass



d. control volume

242. Liquid hydrogen boils at 17 K. What is the temperature in degrees Celsius? 

a. 290



b. 63



c. -120



d. -256

243. When a solid melts, 

a. the temperature of the substance increases.



b. the temperature of the substance decreases.



c. heat leaves the substance.



d. heat enters the substance.

244. How many kilocalories of heat are required to heat 750 g of water from 35˚C to 55˚C. 

a. 15



b. 1500



c. 1.5 x 10^4



d. 6.3 x 10^4

245. Which of the following does not determine the amount of internal energy an object has? 

a. temperature



b. amount of material



c. type of material



d. shape of the object

246. Which of the following have the highest thermal conductivities? 

a. liquids



b. gases



c. metals



d. solids other than metals

247. Identical objects of four different materials are heated to the same high temperature. Which of the following would least likely burn your hand if touched? 

a. aluminium



b. brass



c. glass



d. concrete

248. As we heat a gas at constant pressure, its volume 

a. increases



b. decreases



c. stays the same



d. none of the above

249. The volume of an ideal gas is directly proportional to its 

a. pressure



b. Celsius temperature



c. Kelvin temperature



d. Fahrenheit temperature

250. An ideal gas is maintained at constant temperature. If the pressure on the gas is doubled, the volume is 

a. increased fourfold



b. doubled



c. reduced by half



d. decreased by a quarter

251. If the Kelvin temperature of an ideal gas is doubled, what happens to the rms speed of the molecules in the gas? 

a. it increases by a factor of square root of 2



b. it increases by a factor of 2



c. it increases by factor of 4



d. none of the above

252. A function of state that is associated with disorder in the system and environment. 

a. enthalpy



b. entropy



c. law of diminishing return



d. Lenz’ Law

253. No volume changes occur during this type of process 

a. Isobaric process



b. Isomillimetric process



c. Isocaloric process



d. Isochoric process

254. The boiling of water into steam in an open container is an example of a/an _________ process. 

a. adiabatic



b. isochoric



c. isobaric



d. zero work

255. When liquid water is converted to steam at 100˚C, the entropy of water 

a. increases



b. decreases



c. remains the same



d. none of the above

256. Only energy can cross the boundaries.



a. Closed system



b. Open system



c. Isolated system



d. Isoenergetic system

257. The temperature at which the vapor pressure exactly equals one atm is called _________. 

a. boiling temperature



b. normal boiling point



c. triple point



d. point of infliction

258. Mixture of liquid and steam of the same substance in which both are at saturation temperature. 

a. dry steam



b. current steam



c. wet steam



d. aerosol

259. The term _________ is traditionally used to describe steam issuing from condensate receiver vents and open-ended condensate discharge lines from steam traps. 

a. dry steam



b. wet steam



c. phase steam



d. flash steam

260. Defined as the ratio of weight of dry steam to the weight of stuff. 

a. dryness fraction



b. Vaporization



c. fusion



d. super heated steam

261. What device measures infrared radiation below? 

a. thermocouple



b. thermopile



c. thermodynamic device



d. thermos

262. When an object undergoes thermal expansion, 

a. any holes in the object expand as well



b. any holes in the object remain the same



c. mass increases



d. molecular activities would cease

263. _________ is the quantity of heat required to raise the temperature of one pound of water 1 F˚ from 63 ˚F to 64 ˚F. 

a. one Joule



b. one calorie



c. one watt



d. one BTU

264. Boiling temperature of a material is dependent on its _________. 

a. volume



b. power



c. heat



d. pressure

265. Thermos was invented by _________. 

a. Sir Arthur Conan Doyle



b. Sir Fredrich the Great



c. Thomas Edison



d. Sir James Dewar

266. Most cooking activities involve _________ process. 

a. Isochoric



b. Isothermal



c. Isobaric



d. Isovolumic

267. Adiabatic heating and Adiabatic cooling really means _________ and _________ respectively. 

a. raising the temp and lowering the temp



b. maintaining the pressure and changing the temperature



c. decreasing the volume and increasing the pressure



d. lowering the temp and raising the temp

268. The statement “heat cannot by itself flow from one body into a hotter body” is governed by _________. 

a. the first law of thermodynamics



b. the second law of thermodynamics



c. the third law of thermodynamics



d. the zeroth law of thermodynamics

269. It is impossible for any process to have as its sole result the transfer of heat from a cooler to a hotter body 

a. Carnot’s statement



b. Clausius statement



c. Rankine statement



d. Gauss statement

270. _________ is the average distance a molecule moves before colliding with another molecule.



a. mean free path



b. path allowance



c. compacting factor



d. molecular space

271. Find the pressure due to a column of mercury 74.0 cm high. 

a. 91.80 x 10^3 N/m^2



b. 73.56 x 10^2 N/m^2



c. 9.86 x 10^4 N/m^2



d. 87.2 x 10^4 N/m^2

272. Roughly what is the total weight of air in the entire earth? 

a. 1 x 10^5 tons



b. 2 x 10^6 tons



c. 6 x 10^15 tons



d. 8 x 10^10 tons

273. _________ is defined as that equivalent to the pressure due to a column of mercury 76cm long. 

a. surface pressure



b. gage pressure



c. standard atmospheric pressure



d. isobaric pressure

274. If any external pressure is applied to a confined fluid, the pressure will be increased at every point in the fluid by the amount of the external pressure is known as _________. 

a. Torricelli’s law



b. Barometric law



c. Newton’s Second law



d. Pascal’s law

275. What type of pressure cannot be used for Boyle’s Law? 

a. Atmospheric Pressure



b. Gauge Pressure



c. Surface Pressure



d. Isobaric Pressure

276. To displace a cubic foot of fresh water, you need _________ force. 

a. 62.4 lb



b. 9.81 lb



c. 76 lb



d. 760 lb

277. The force per unit length across such a line in the surface is called _________. 

a. force per length



b. surface tension



c. Pressure



d. Density

278. The speed at which a liquid escapes from a vessel through an orifice is given by _________. 

a. Archimedes Principle



b. Evangelista’s Law



c. Torricelli’s Theorem



d. Bernoulli’s Equation

279. The process of one substance mixing with another because of molecular motion is called _________. 

a. diffusion



b. viscosity



c. streamline flow



d. solution

280. When was the Ninth General Conference on Weights and Measures decided to abandon centigrade and used Celsius Instead? 

a. 1950



b. 1936



c. 1957



d. 1948

281. _________ is the temperature to which the air must be cooled, at constant pressure, to produce saturation. 

a. relative humidity



b. triple point temperature



c. dew point



d. critical point

282. _________ is a succession of changes that ends with the return of the body or system to its initial state. 

a. process



b. system



c. equilibrium



d. cycle

283. Intensive properties of a system are called _________. 

a. Bulk Properties



b. Innate Properties



c. Natural Properties



d. Inside Properties

284. In thermodynamics, a throttling process, also called a _________, is a type of isenthalpic process where a liquid or gas is cooled as it passes from a higher pressure state to a lower pressure state. 

a. Rankine Process



b. Carnot Cycle



c. Joule-Thomson process



d. Refrigeration process

285. Gasoline and Diesel Engines are best described by the _________. 

a. Otto Cycle



b. Burnign Cycle



c. Shikki Cycle



d. Shapa R’ Elli Cycle

286. Twenty grams of ice at 0˚C melts to water at 0˚C. How much does the entropy of the 20g change in this process? 

a. 30.5 J/K



b. 24.6 J/K



c. 21.3 J/K



d. 15.7 J/K

287. The first law of thermodynamics is based on which of the following principles? 

a. conservation of mass



b. the enthalpy-entropy relationship



c. action – reaction



d. conservation of energy

288. If a system absorbs 500 cal of heat at the same time does 400J of work, find the change in internal energy of the system. 

a. 1400 J



b. 1700 J



c. 1900 J



d. 1500 J

289. A gas is enclosed in a cylinder with a weighted piston as the top boundary. The gas is heated and expands from a volume of 0.04 m3 to 0.10 m3 at a constant pressure of 200 kPa. Find the work done on the system. 

a. 5 kJ



b. 15 kJ



c. 10 kJ



d. 12 kJ

290. A simple steam engine receives steam from the boiler at 180˚C and exhausts directly into the air at 100˚C. What is the upper limit of its efficiency? 

a. 11.28 %



b. 36.77 %



c. 20.36 %



d. 17.66 %

291. Heat which causes a change in temperature of a substance. 

a. Latent heat



b. Sensible heat



c. Specific heat



d. Heat of Fusion

292. Who coined the term latent heat? 

a. John Thompson



b. Studey Baker



c. Joe di Maggio



d. Joseph Black

293. Which of the following cannot be measured by a thermometer?



a. Latent Heat



b. Sensible Heat



c. Specific Heat



d. Heat of Fusion

294. It is generally accepted as a law of nature that although one may closely approach 0 Kelvin it is impossible actually to reach it. 

a. First Law of thermodynamics



b. Second Law of thermodynamics



c. Third Law of thermodynamics



d. Zeroth Law of thermodynamics

295. One calorie is equal to _________. 

a. 1/180 W.h



b. 1/860 W.h



c. 1/360 W.h



d. 1/250 W.h

296. A _________ is a reversible process in which there is transfer of heat and takes place according to the relation pVn = C where n is any constant. 

a. Polytropic process



b. Entropy



c. Ideal Gas Law



d. Carnot Cycle

297. The flow through an open system is _________ if all properties at each point within the system remain constant with respect to time. 

a. streamline flow



b. steady flow



c. constant flow



d. algebraic flow

298. The most efficient cycle that can operate between two constant temperature reservoir is the _________. 

a. Otto Cycle



b. Lazare Cycle



c. Isothermal Cycle



d. Carnot Cycle

299. The flow energy of 150 L of a fluid passing a boundary to a system is 110 kJ. Determine the pressure at this point 

a. 733.33 kPa



b. 833.33 kPa



c. 933.33 kPa



d. 633.33 kPa

300. Who is the father of thermodynamics? 

a. Lazare Carnot



b. Sadi Carnot



c. William Thompson



d. Rudolf Classius

301. If air is at pressure, p, of 3200 lbf/ft2, and at a temperature, T, of 800 ˚R, what is the specific volume, v? (R=5303 ft-lbf/lbm-˚R, and air can be modeled as an ideal gas.) 

A.9.8 ft^3/lbm



B.11.2 ft^3/lbm



C.13.33 ft^3/lbm



D.14.2 ft^3/lbm

Formula: pv = RT v = RT / p

302. Steam at 1000 lbf/ft^2 pressure and 300˚R has specific volume of 6.5 ft^3/lbm and a specific enthalpy of 9800 lbf-ft/lbm. Find the internal energy per pound mass of steam. 

A.2500 lbf-ft/lbm



B.3300 lbf-ft/lbm



C.5400 lbf-ft/lbm



D.6900 lbf-ft/lbm

Formula: h= u+ pV u= h– pV 303. 3.0 lbm of air are contained at 25 psia and 100 ˚F. Given that Rair = 53.35 ft-lbf/lbm- ˚F, what is the volume of the container? 

A.10.7 ft^3



B.14.7 ft^3



C.15 ft^3



D.24.9 ft^3

Formula: use the ideal gas law pV = mRT T = (100 +460) ˚R V = mRT/p 304. The compressibility factor, x, is used for predicting the behavior of nonideal gases. How is the compressibility ty factor defined relative to an ideal gas? (subscript “c”refers to critical value) 

A. z = P / Pc



B. z = pV/ RT



C. z = T /Tc



D. z = RT / pV

Hint: for an real gases the compressibility factor, x, is an dimensionless constant given by pV= zRT. Therefore z = pV / RT 305. From the steam table, determine the average constant pressure specific heat (c) of steam at 10 kPa and45.8 ˚C 

A.1.79 kJ/ kg-˚C



B.10.28 kJ/ kg-˚C



C.30.57 kJ/ kg-˚C



D. 100.1 kJ/ kg-˚C

Formula: ∆h = c∆T From the steam table At 47.7 ˚C h= 2588.1 kJ/ kg At 43.8 ˚C h= 2581.1 kJ/ kg 306. A 10m^3 vessel initially contains 5 m^3 of liquid water and 5 m^3 of saturated water vapor at 100 kPa. Calculate the internal energy of the system using the steam table. 

A. 5 x10^5 kJ



B. 8x10^5 kJ



C. 1 x10^6 kJ



D. 2 x10^6 kJ

Formula: fromthe steamtable vƒ = 0.001043 m^3 / kg vg = 1.6940 m^3 / kg u ƒ= 417.3 kJ/kg ug= 2506kJ/kg formula: Mvap = V vap/vg

M liq = Vliq/ vƒ u =uƒM liq + ug M vap 307. A vessel with a volume of cubic meter contains liquid water and water vapor ion equilibrium at 600 kPa. The liquid water has mass of1kg. Using the steam table, calculate the mass of the water vapor. 

A. 0.99kg



B. 1.57 kg



C. 2.54 kg



D. 3.16 kg

Formula: from the steam table at 600kPa vƒ = 0.001101 m^3 / kg vg = 0.3157 m^3 / kg Vtot = mƒ vƒ + mg vg mg = (tot-mƒ vƒ) / vg 308. Calculate the entropy of steam at 60psiawith a quality of 0.8 

A. 0.4274 BTU/lbm-˚R



B. 0.7303 BTU/lbm-˚R



C. 1.1577 BTU/lbm-˚R



D. 1.2172 BTU/lbm-˚R

Formula: fromthe steamtable at 60 psia: sƒ = 0.4274 BTU/lbm-˚R sƒg = 1.2172 BTU/lbm-˚R) s = sƒ + x sƒg where x = is the quality

309. Find the change in internal energy of 5 lb. of oxygen gas when the temperature changes from 100 ˚F to 120 ˚F. CV = 0.157 BTU/lbm-˚R 

A.14.7 BTU



B.15.7 BTU



C. 16.8 BTU



D. 15.9 BTU

Formula: ∆U= mcv∆T 310. Water (specific heat cv= 4.2 kJ/ kg ∙ K ) is being heated by a 1500 W h eater. What is the rate of change in temperature of 1kg of the water? 

A. 0.043 K/s



B. 0.179 K/s



C. 0.357 K/s



D. 1.50 K/s

Formula: Q = mcv (∆T) 311. A system weighing 2kN. Determine the force that accelerate if to 12 m/s^2. a. vertically upward when g = 9.7 m/s^2 

A. 4474.23 N



B.5484.23 N



C.4495.23 N



D.5488.23 N

Formula: F = m/k (a +g) 312. Refer to problem # 11. Determine the force that accelerates if to 12 m/s^2. horizontally along frictionless plane. 

A. 2474.23 N



B. 2574.23 N



C. 3474.23 N



D. 2374.23 N

Formula : M = wk / g F = ma /k 313. A problem Drum ( 3 ft. diameter ; 6 ft. height ) is field with a fluid whose density is 50 lb/ft^3. Determine the total volume of the fluid. 

A. 42.41 ft^3



B.44.35 ft^3



C.45.63 ft^3



D.41.23 ft^3

Formula: Vf = (pi d^2 h) / 4 314. What is the resulting pressure when one pound of air at 15 psia and 200 ˚F is heated at constant volume to 800 ˚F? 

A.15 psia



B. 28.6 psia



C. 36.4 psia.



D. 52.1 psia

Formula : T1/p1 = T2/p2 p2= p1T2 / T1 315. What horse power is required to isothermally compress 800 ft^3 of Air per minute from 14.7 psia to 120 psia? 

A. 28 hp



B.108 hp



C.256 hp



D.13900 hp

Formula: W= p1V1 ln (p1/p2) Power = dW / dt 316. What is the equation for the work done by a constant temperature system? 

A. W = mRTln(V2-V1)



B. W = mR( T2-T1 ) ln( V2/V1)



C. W = mRTln (V2/V1)



D. W = RT ln (V2/V1)

Formula : W=∫ pdV lim1,2 р = mRT / V 317. Twenty grams of oxygen gas are compressed at a constant temperature of 30 ˚C to 5%of their original volume. What work is done on the system. 

A.824 cal



B.924 cal



C.944 cal



D.1124 cal

Formula: W = -mRTln (V2/V1) Where R = (1.98 cal/gmole·K) (32 g/gmole) 318. Helium ( R= 0.4698 BTU/lbm-˚R ) is compressed isothermally from 14.7 psia and 68 ˚F. The compression ratio is 1:4. Calculate the work done by the gas.



A. –1454 BTU/lbm



B. -364 BTU/lbm



C.-187BTU/lbm



D.46.7 BTU/lbm

Formula: W = RT ln (V2/V1) 319. Gas is enclosed in a cylinder with a weighted piston as the stop boundary. The gas is heated and expands from a volume of 0.04 m^3 to 0.10 m^3 at a constant pressure of 200kPa.Calculate the work done by the system. 

A. 8 kJ



B. 10 kJ



C.12 kJ



D.14 kJ

Formula: W = p(V2-V1) 320. refer to problem no.13. Determine the specific volume. 

A. 0.02 ft^3/lbm



B. 0.05 ft^3/lbm



C. 1.0 ft^3/lbm



D. 1.2 ft^3/lbm

Formula : Vf = ( pi d^2 h) / 4 Pf = mf / vf Specific volume= Vf /mf 321. What is the weight of a66-kgm man at standard condition? (Formula: Fg= mg / k)



a. 66 kgf



b. 66 kgm



c. 66 lbm



d. 66 gf

322. What is the specific weight of water at standard condition? (Formula: γ = ρg / k)   

a. 1000 kgm/m3 b. 9.8066 m/s2 c. 1000 kgf/m3



d. None of the above

323. 746 °R = ______ °F 

a. 254



b. 345



c. 286



d. None of the above

324. A 30-m vertical column of fluid (density 1878 kg/m3 ) is located where g= 9.65 mps2. Find the pressure at the base of the column. (Formula: pg= gρhg/k ) 

a. 543680 N/m2



b. 543.68 kPa (gauge)



c. Both a & b



d. None of the above

325. Ten cu ft. of air at 300 psia 400°F is cooled to 140°F at constant volume. What is the final pressure? (formula: p2 = p1T2/T1) 

a. 0



b. 209 psia



c. - 420 psia



d. None of the above

326. 876 °R = _____ °F 

a. 335



b. 416



c. 400



d. None of the above

327. There are 1.36 kg of gas, for which R = 377 J/kg.k and k = 1.25, that undergo a nonflow constant volume process from p1 = 551.6 kPa and t1 = 60°C to p2 = 1655 kPa. During the process the gas is internally stirred and there are also added 105.5 kJ of heat. Determine t2. (Formula: T2= T1p2/ p1) 

a. 999 K



b. 888 K



c. 456 K



d. One of the above

328. 5 atm = ____mmHg 

a. 8300



b. 3800



c. 3080



d. None of the above

329. A certain gas, with cp = 0.529Btu/lb.°R and R = 96.2 ft.lb/lb.°R, expands from 5 cu ft and 80°F to 15 cu ft while the pressure remains constant at 15.5 psia. Compute for T2. (Formula: T2= T1V2/V1) 

a. 460°R



b. 270°R



c. 1620 °R



d. None of the above

330. In the above problem, compute for the mass. (Formula: m = p1V1 / RT1) 

a. 0.2148 lb



b. 0.2134 lb



c. 0.1248 lb



d. None of the above

331. 710°R= ______ °C 

a. 214



b. 121



c. 213



d. None of the above

332. 212 °F = _____ °C 

a. 200



b. 150



c. 100



d. None of the above

333. Let a closed system execute a state change for which the heat is Q = 100 J and work is W = -25 J. Find ∆E. (Formula: ∆E = Q- W) 

a. 125 J



b. 123 J



c. 126 J



d. None of the above

334. A pressure gage registers 50 psig in a region where the barometer is 14.25 psia. Find absolute pressure in psia, Pa. (Formula; p = patm+ pg) 

a. 433 kPa



b. 443 kPa



c. 343 kPa



d. None of the above

335. A mass of 5kg is 100m above a given datum where local g = 9.75 m/s2. Find the gravitational force in newtons. (Formula: Fg= mg/k ) 

a. 48.75 N



b. 50 N



c. 45 N



d. None of the above

336. In the above problem, find the potential energy of the mass with respect to datum. (Formula: P = mgz/k ) 

a. 4875 j



b. 0.51 j



c. 0.46 j



d. None of the above

337. The combined mass of car and passengers travelling at 72 km/hr is 1500 kg. Find the kinetic energy of this combined mass. (Formula: K =mv2/ 2k ) 

a. 300 kJ



b. 200 kJ



c. 500 kJ



d. None of the above

338. 14.696 psia = _____ mmHg 

a. 760



b. 1



c. 350



d. None of the above

339. 212 °C = _____ K 

a. 485



b. 435



c. 498



d. None of the above

340. 212 °F = _____R 

a. 567



b. 672



c. 700



d. None of the above

341. An automobile tire has a gauge pressure of 200 kpa at 0°C assuming no air leaks and no change of volume of the tire, what is the gauge pressure at 35ºC. 

a. 298.645



b. 398.109



c. 291.167



d. 281.333

Pg = Pabs - Patm

342. An ideal gas at 45psig and 80ºF is heated in the close container to 130ºF. What is the final pressure? 

a. 65.10 psi



b. 65.11 psi



c. 65.23 psi



d. 61.16 psi

P1V1/T1= P2V2/T2;V = Constant 343. A wall of the firebrick has an inside temperature of 313ºF and an outside temperature of 73ºF. What is the difference in the surface temperature in Rankin? 

a. 70



b. 68



c. 72



d. 94

ºR = ºF + 460 344. What is the force required to accelerate amass of 30kg at a rate of 15m/s². 

a. 460 N



b. 380 N



c. 560 N



d. 450 N

F = ma 345. How much does an object having the mass of 100kg weight in newton. 

a. 981 N



b. 991 N



c. 981.6 N



d. 980.1N

F = ma 346. The volume of the gas held at constant pressure increases 4 cm² at 0°C to 5cm². What is the final pressure? 

a. 68.65ºC



b. 68.25ºC



c. 70.01°C



d. 79.1ºC

t2= T2–T1 347. A certain gas with cp = 0.529Btu/lb°R and R = 96.2ft/lbºR expands from 5 ft and 80ºF to 15 ft while the pressure remains constant at 15.5 psia. 

a. T2=1.620ºR, ▲H = 122.83 Btu



b. T2 = 2°R, ▲H = 122.83 Btu



c. T2 = 2.620ºR, ▲H = 122.83 Btu



d. T2 = 1°R, ▲H = 122.83 Btu

T2= V2(t2)/V1 and ▲H = mcp (T2-T1) 348. A vacuum is connected to a tank reads 3kpa at a location w/ the barametric pressure reading is 75mmhg. Determined the P absolute in the tank 

a. 70.658 kpa



b. 68 kpa



c. 58.78 kap



d. None of the above

Pabs = Patm – Pvacuum 349. Calculate:

a. Mass flow rate in lb/hr. b. The velocity at section 2 in fps 

a. 800,000lb/hr;625ft/s



b. 900,000lb/hr;625 ft/s



c. 888,000lb/hr;269 ft/s



d. 700,000lb/hr;269 ft/s

m = A1V!/V1 350. A 600kg hammer of a pile driver is lilted 2m the pilling head. What is the change of potential energy? If the hammer is realest. What will be its velocity and the instant if it sticks the pilling? 

a. 10,772 N-m and 5.26m/s



b. 13,200 N-m and 5.26m/s



c. 11,772 N-m and 6.26m/s



d. 11,77 2N-m and5.26m/s

▲PE = mgo(▲Z)/gc

351. A bayabas falls from a branch 5m above the ground with what speed in meter per second does it strike the ground assume g = 10m/s². 

a. 11m/s



b. 12m/s



c. 13m/s



d. 10m/s

▲KE = mV2/2gc 352. While swimming a depth of 13m in a fresh water lake a fish emits an air bubble of volume 2 mm² atmospheric pressure is 100kpa what is the original pressure of the bubble.



a. 217.17 kpa



b. 119 kpa



c. 326.15 kpa



d. 210 kap

Pabs = Pg + Patm 353. Oxygen at 15ºC and 10.3 Mpa gauge pressure occupies 600L. What is the occupied by the oxygen at 8.28 Mpa gauge pressure and 35ºC? 

a. 789.32 L



b. 796.32 L



c. 699 L



d. 588 L

V2= P1V1/T1P2 354. Water is flowing through a 1 foot diameter pipe at the rate of 10ft/sec. What is the volume flow rate of water in ft³/sec? 

a. 7.85



b. 6.85



c. 8.85



d. 5.85

V = Aν 355. A certain fluid is flowing in a 0.5m x 0.3 channel at the rate of 3 m/s and has a specific volume of 0.012 m³/kg. Determined the mass of water flowing in kg/s. 

a. 267 kg/s



b. 378 kg/s



c. 375 kg/s



d. 456.5 kg/s

m = Aν/V

356. A gas having a volume of100 ft³ at 27ºC is expanded to 120 ft³by heated at constant pressure to what temperature has it been heated to have this new volume? 

a. 87°C



b. 85°C



c. 76°C



d. 97°C

t2= T2–T1 357. Water flow to a terminal 3 mm diameter and has an average speed of 2 m/s. What is the rate of flow in cubic meter/mm? 

a. 0.0001m³/min



b. 0.076 m³/min



c. 0.085 m³/min



d. 0.097 m³/min

358. Water flowing at a 6m/s through a 60 mm pipe is suddenly channeled into a 30 mm pipe. What is the velocity in the small pipe? 

a. 34m/s



b. 24m/s



c. 15m/s



d. 27m/s

359. A vertical column of water will be supported to what height by standard atmospheric pressure. 

a. 33.9 ft



b. 45 ft



c. 67 ft



d. 25.46 ft

ho= Po/Yo

360. A fluid flows in a steady manner between two section in a flow line at section 1: A 1 = 1ft², V1 = 100fpm, volume1 of 4ft³/lb. at sec2: A2 = 2 ft², p= 0.20 lb/ft³ calculate the velocity at section 2. 

a. 625 fpm



b. 567 fpm



c. 356 fpm



d. None of the above

361. The weight of an object is 50lb. What is its mass at standard condition? 

a. 50 lbm



b. 60 lbm



c. 70 lbm



d. 80 lbm

formula: m = Fgk /g 362. A vertical column of water will be supported to what height by standard atmospheric pressure. If the Y w = 62.4lb/ft3 po = 14.7 psi. 

a. 44.9 ft



b. 33.9 ft



c. 22.9 ft



d. 55.9 ft

formula: ho= po/Yw 363. For a certain gas R = 320 J/kg.K and cv= 0.84kJ/kg.K. Find k? 

a. 1.36



b. 1.37



c. 1.38



d. 1.39

formula: k= R / cv+1

364. Ten cu. ft of air at 300psia and 400°F is cooled to 140°F at constant volume. What is the transferred heat? 

a.-120Btu



b. -220Btu



c.-320Btu



d. -420Btu

formula: Q= mcv(T2-T1) 365. Utilizing the answer to the previous problem, estimate the overall or average increase in temperature ( ΔT) of the concrete roof from the energy absorbed from the sun during a12hour day. Assume that all of the radiation absorbed goes into heating the roof. The specific heat of concrete is about 900 J/kg, and the density is about 2,300 kg/m3. 

a. 7.9 °C



b. 8.9°C



c. 9.9°C



d. 10.9°C

formula: ΔQ = m c ΔT 366. The concrete roof of a house is 10 m by 8 m and 10 cm thick (4"). Estimate the total heat the roof would absorb over the 12 day?    

a. 1.3 x 108 J b 2.3 x 108 J c. 3.3 x 108 J d. 4.3 x 108 J

formula: ΔQ = ΔQ/Δtx Δt 367. The value for the ΔU of a system is -120 J. If the system is known to have absorbed 420 J of heat, how much work was done? 

a. -540 J



b. -640 J



c. -740 J



d. -840 J

formula: ΔU = q +w 368. When the pressure on a 1 kg liquid is increased isothermally from 1 bar to 3000 bar the Gibbs free energy increases by 360 kJ. Estimate the density of the liquid.    

a. 0.66 kg liter-1 b. 0.77 kg liter-1 c. 0.88 kg liter-1 d. 0.99 kg liter-1

369. A car whose mass is 2 metric tons is accelerated uniformly from stand hill to 100 kmph in 5 sec. Find the driving force in Newton’s. 

a. 11,120 N



b. 11,320 N



c. 11,420 N



d. 11520 N

formula: F= ma / k 370. An ideal gas of volume 1liter and pressure 10 bar undergoes a quasistatic adiabatic expansion until the pressure drops to 1 bar. Assume γ to be 1.4 what is the final volume? 

a. 3.18 l



b. 4.18 l



c. 5.18 l



d. 6.18 l

371. Two masses, one of the 10kg and the other unknown, are placed on a scale in a region where g = 9.67 m/sec2. The combined weight of these two masses is 174.06 N. Find the unknown mass in kg. 

a. 20 kg



b. 19 kg



c. 18 kg



d. 17 kg

formula: m=Fg k / g 372. The flow energy of 5 ft3 of a fluid passing a boundary to a system is 80,000 ft-lb. Determine the pressure at this point. 

a. 222 psi



b. 333 psi



c. 444 psi



d. 111 psi

formula: Ef= pV 373. Find и for steam at 100 psia and 600°F.If h = 1329.6 and v = 6.216 

a. 1214 Btu / lb



b. 1234 Btu /lb



c. 1342 Btu / lb



d. 1324 Btu /lb

formula: и = h– pv/ J 374. What mass of nitrogen is contained in a10 ft3 vessel at a pressure of 840atm and 820°R? Make a computation by using ideal gas equation. 

a. 194lb



b. 214lb



c. 394 lb



d. 413lb

formula: m=pV /RT 375. A rotary compressor receives 6m3/ min of a gas(R=410J/ kgK, cp=1.03kJ /kgK,k= 1.67) at 105 k/Paa, 27°C and delivers it at 630kPaa: ΔP = 0, ΔK= 0. Find the work if the process is isentropic? 

a. –1664 kJ/min



b. –1774 kJ/min



c. –1884 kJ/min



d. –1994 kJ/min

formula: WSF = Q- ΔH m=p1V1/RT1 T2= T1(p2/p1)(k-1)/k 376. A carnot power cycle operates on 2 lb of air between the limits of 71 °F and 500°F. The pressure at the beginning of isothermal expansion is 400 psia and at the end of isothermal expansion is 185psig. Determine the volume at the end of isothermal compression.    

a. 7.849 ft3 b. 7.850 ft3 c. 7.851 ft3 d. 7852 ft3

formula: V= mRT/ P P3= P2[T3/ T2] 377. During a polytropic process,10lb of an ideal gas, whose R= 40ft.lb/lb.R and cp = 0.25Btu/lb.R, changes state from 20 psia and 40°F to 120psia and 340°F. Determine n? 

a. 1.234



b. 1.345



c. 1.456



d. 1.356

formula: [ p2/p1]n-1 / n = T2/T1 378. A perfect gas has a value of R= 319.2 J/ kf.K and k= 1.26. If 120 kJ are added to 2.27 kf\g of this gas at constant pressure when the initial temp is 32.2°C? Find T2. 

a. 339.4 K



b. 449.4 K



c. 559.4K



d. 669.4K

formula: cp = kR/ k-1 Q= mcp(T2-T1) 379. A certain gas, with cp = 0.529Btu/ lb. °Rand R = 96.2ft.lb/lb. °R, expands from 5 cu ft and 80°F to 15 cu ft while the pressure remains constant at 15.5psia. Compute for T2.



a.1520°R



b. 1620°R



c. 1720°R



d. 1820°R

formula: T2= T1V2/V1 380. A System has a temperature of 250°F. Convert this Value to °R? 

a. 740°R



b.730°R



c. 720°R



d. 710°R

formula: °R= °F + 460 381. Steam with a specific volume of 0.09596 m³/kg undergoes a constant pressure process at 1.70 MPa until the specific volume becomes 0.13796 m³/kg. What are (a) the final temperature, (b) ∆u, (c) W, (d)∆s, and (e) Q? 

a) 265.4°C, 430.7kJ/kg, 71.4kJ/kg, 1.0327kJ/(kg)(K),502.1 kJ/kg



b) 204.2°C, -703.2 kJ/kg, -84.15 kJ/kg, -1.7505 kJ/(kg)(K), -787.4 kJ/kg



c) 304.2°C, -803.2 kJ/kg, -89.15 kJ/kg, -2.7505 kJ/(kg)(K), -987.4 kJ/kg



d) 279.4°C, 439.7kJ/kg, 79.4kJ/kg, 3.0327kJ/(kg)(K),602.1 kJ/kg

382. Steam with an enthalpy of 2843.5 kJ/kg undergoes a constant pressure process at 0.9 MPa until the enthalpy becomes 2056.1 kJ/kg. What are (a) the initial temperature or quality, (b) ∆u, (c)W, (d) ∆s, and(e) Q? 

a) 265.4°C, 430.7kJ/kg, 71.4kJ/kg, 1.0327kJ/(kg)(K),502.1 kJ/kg



b) 204.2°C, -703.2 kJ/kg, -84.15 kJ/kg, -1.7505 kJ/(kg)(K),-787.4 kJ/kg



c) 304.2°C, -803.2 kJ/kg, -89.15 kJ/kg, -2.7505 kJ/(kg)(K), -987.4 kJ/kg



d) 279.4°C, 439.7kJ/kg, 79.4kJ/kg, 3.0327kJ/(kg)(K), 602.1 kJ/kg

Formula of #1and #2: ∆u = u2 –u1, W = p(v2-v1), ∆s =s2-s1, Q = h2 –h1

383. At throttling calorimeter receives steam from a boiler drum at0.11MPa and is superheated by 10 degrees. If the boiler drum pressure is 1.55 MPa, what is the quality of the steam generated by the boiler? 

a) 95.20%



b) 70.10%



c) 65.60%



d) 95.56%

Formula: h1 = hf1 + x1hfg1 384. A steam calorimeter receives steam from a pipe at 0.1 MPa and 20°SH. For a pipe steam pressure of 2 MPa, what is the quality of the steam? 

a) 95.56%



b) 70.10%



c) 95.20%



d) 85.10%

Formula: h1 = hf1 + x1hfg1 385. A 1-kg steam-water mixture at 1.0 MPa is contained in an inflexible tank. Heat is added until the pressure rises to 3.5 MPa and the temperature to 400°. Determine the heat added. 

a) 1378.7 kJ



b) 1348.5 kJ



c) 1278,7 kJ



d) 1246,5 kJ

Formula: Q = (h2 – p2v2) –(h1 –p1v1) 386. Water vapor at 100 KPa and 150°C is compressed isothermally until half the vapor has condensed. How much work must be performed on the steam in this compression process per kilogram? 

a) -1384.7 kJ



b) 1384.7 kJ



c) -2384.7 kJ



d) 2384.7 kJ

387. Wet steam at 1 MPa flowing through a pipe is throttled to a pressure of 0.1 MPa. If the throttling temperature is110°C, What is the quality of the steam in the pipe? 

a) 96%



b) 86%



c) 76%



d) 66%

388. Steam is throttled to 0.1 MPa with 20 degrees of superheat. (a) What is the quality of throttled steam if its pressure is 0.75 MPa (b) What is the enthalpy of the process? 

a) 97.6%,2713 kJ/kg



b) -97.6%, 2713 kJ/kg



c) 87.6%,3713 kJ/kg



d) -87.6%, 3713 kJ/kg

389. The pressure gauge on a 2000 m³ tank of oxygen gas reads 600 kPa. How much volumes will the oxygen occupied at pressure of the outside air 100 kPa? 

a) 14026.5 m³



b) 15026.5 m³



c) 13026.5 m³



d) 16026.5 m³

Formula: P1V1/T1 =P2V2/T2 390. Assuming compression is according to the Law PV = C, Calculate the initial volume of the gas at a pressure of 2 bars w/c will occupy a volume of 6m³ when it is compressed to a pressure of 42 Bars.



a) 130m³



b) 136m³



c) 120m³



d) 126m³

Formula: P1V1/T1 =P2V2/T2 391. A Gas tank registers1000 kPa. After some gas has been used, the gauge registers 500 kPa. What percent of the gas remains in the tank? 

a) 64.40%



b) 74.60%



c) 58.40%



d) 54.60%

Formula: Pabs = Patm + Pgage & %= P2/P1 * 100% 392. The volume of a gas under standard atmospheric pressure & 76 cmHg is 200m³. What is the volume when pressure is 80 cmHg if the temperature is unchanged? 

a) 180 in³



b) 170 in³



c) 160 in³



d) 190 in³

Formula: P2V2 = P1V1 393. While swimming at depth of120m in a fresh water lake, A fish emits an air bubbles of volume 2.0mm³ atmospheric pressure is 100kPa. What is the pressure of the bubble? 

a) 217.7 kPa



b) 317.7 kPa



c) 417.7 kPa



d) 517.7 kPa

Formula: P= δh 394. How many joules of work is the equivalent of 15000 cal of heat? 

a) 62850 joules



b) 3579.95 joules



c) 14995.81 joules



d) 15004.19 joules

Formula: J =Work/Heat J = mechanical equivalent of heat whose value is 4.19 joules/calorie 395. Two thick slices of bread, when completely oxidized by the body, can supply 200,000 cal of heat. How much work is this equivalent to? 

a) 4,190,000 joules



b) 8,390,000 joules



c) 839,000 joules



d) 419 000 joules

Formula: J =Work/Heat J = mechanical equivalent of heat whose value is 4.19 joules/calorie 396. 3 horsepower (hp) = _____________watts? 

a) 1492 watts



b) 2238 watts



c) 746 watts



d) 2238 kilowatts

Formula: 1hp= 746 watts 397. How many Newton’s (N) in 900,000 dynes? 

a) 8 Newton’s



b) 9 Newton’s



c) 7 Newton’s



d) 6 Newton’s

Formula: 1Newton (N)=100,000dynes 398. Calculate the power output in horsepower of an 80-kg man that climbs a flight of stairs 3.8 m high in 4.0 s. 

a) 744.8 hp



b) 0.998 hp



c) 746 hp



d) 1.998 hp

Formula: Power = Fd/t = mgh/t F = W = mg d=h 399. How many calories of heat will be needed to raise the temperature of 200 g of iron from 27°C to 80°C? (c = 0.11 cal/g. °C) 

a) 1.16 kcal



b) 2166 cal



c) 3.16 kcal



d) 4166 cal

Formula: H = mc∆T 400. 100g of iron was heated to 100°C and mixed with 22g of water at 40°C. The final temperature of the mixture was 60°C. Show that the heat given off by the iron equals the heat absorbed by the water. 

a) 440 cal



b) 540 cal



c) 340 cal



d) 640 cal

Formula: H (given off by iron) = H (absorbed by water), mc∆T(iron)= mc∆T(water)

401. An engineering science primarily concerned with heat and work conversions. 

a. Thermodynamics



b. Mechanics



c. Physics



d. Electromagnetic

402. “If the temperature o f a fixed quantity of a gas is held constant during a change of state, the volume varies inversely with the absolute pressure. 

a. Charle’s Law



b. Boyle’s Law



c. Dalton’s Law



d. Amagat’s Law

403. Avogadro’s Number NA 

a. 6.2205 x 10^23 mol-1



b. 6.2025 x 10^23 mol-1



c. 6.0225 x 10^23 mol-1



d. 6.2250 x 10^23 mol-1

404. The first law of thermodynamics may be expressed in the following equivalent 

a. the net heat transfer id equal to the network



b. the sum of the total energy forms leaving the system boundary is always equal to the energy input



c. energy can neither be created nor destroyed but only converted from one form to another



d. all of the above

405. A system whose boundary does not allow the exchange of either matter or energy with the surrounding 

a. open system



b. closed system



c. isolated system



d. none of the above

406. The specific terms used in phase transitions 

a. melting



b. evaporation



c. freezing



d. sublimation

407. The density of water at 4°C is 

a. 1 gm/cm³



b. 2 gm/cm³



c. 3 gm/cm³



d. 4 gm/cm³

408. Archimedes principle states that 

a. when a body is inversed in a fluid, the fluid exerts a downward force on the body whose magnitude is equal to the weight of the displaced fluid



b. when a body is inversed in a fluid, the fluid exerts a upward force on the body whose magnitude is equal to the weight of the displaced fluid.



c. when a body is inversed in a fluid, the fluid exerts a downward force on the body whose magnitude is greater than the weight of the displaced fluid.



d. when a body is inversed in a fluid, the fluid exerts a downward force on the body whose magnitude is lower than the weight of the displaced fluid.

409. Types of system except one 

a. closed



b. open



c. isolated



d. solid

410. Isometric process is 

a. T = P



b. P = C



c. V = C



d. T = V

411. The ratio of the change in energy in the form of the heat 

a. relative density



b. specific heat



c. specific gravity



d. none of the above

412. Specific heat ratio is always 

a. > 1



b. < 1



c. = 1



d. none of the above

413. It states that mass is a commodity that can neither be heated nor destroyed with the exception of nuclear processes where the conversion of mass into energy is a fundamental principle 

a. Law of Conservation of Mass



b. Law of Conservation of Energy



c. Law of Conservation of Power



d. Law of Conservation of Heat

414. The energy that stored in a system as a result of its position in the earth’s gravitational field 

a. elastic energy



b. kinetic energy



c. potential energy



d. flow energy

415. It involves a force deforming a solid body 

a. non-elastic work



b. non-flow work



c. flow work



d. elastic work

416. Developed the Fahrenheit scale 

a. Gabriel Daniel Fahrenheit



b. Daniel Gabriel Fahrenheit



c. Gabriel Danelle Fahrenheit



d. Danelle Gabriel Fahrenheit

417. Developed the centigrade or Celsius 

a. Andres Celsius



b. Anders Celsius



c. Andrew Celsius



d. Anthony Celsius

418. Instrument used to measure the absolute pressure of the atmosphere 

a. galvanometer



b. thermometer



c. barometer



d. pressure gages

419. A vector quantity whose direction is the same as the direction of the velocity 

a. Force



b. Momentum



c. Friction



d. Resultant

420. Conceptualize that the heat was an energy form and that there was a precise relationship between heat and work. 

a. Count Rumford



b. Sir Humpry Davey



c. James Prescott



d. all of the above

421. Which is true: 

a. Energy is a scalar quantity



b. Energy is a vector quantity



c. Energy is vector & scalar



d. None of the above

422. It is a region enclosed by specified boundaries, which may be imaginary, either fixed or moving 

a. Isolated system



b. Open system



c. System



d. None of the above

423. Amount or volume of liquid that pass in a given limit of time



a. Flow rate



b. Volume



c. Time



d. None of the above

424. Ability to do work 

a. Power



b. Energy



c. Work



d. None of the above

425. Amount of heat needed to rate the temperature of a substance by 1°C 

a. Heat Exchange



b. Heat Engine



c. Specific Heat



d. None of the above

426. Study of transformation of heat energy to mechanical energy to other forms of energy. 

a. Thermodynamics



b. Physics



c. Mechanics



d. None of the above

427.Heat cannot be created, nor destroyed, but it can be changed from one form to another. The energy in the universe remains constant.   

a. 1st Law of Energy Conservation b. 2nd Law of Energy Conservation c. 3rd Law of Energy Conservation



d. None of the above

428. Quantities that describe both magnitude & direction 

a. Physical Quantity



b. Scalar Quantity



c. Vector Quantity



d. None of the above

429. The sum of energies of all the molecules in a system, energies that appear in several complex forms. 

a. External Energy



b. Internal Energy



c. Kinetic Energy



d. None of the above

430. The value of atomic charge e is   

a. 1.60210 x 10-19 coulomb b. 1.68910 x 10-19 coulomb c. 1.20160 x 1019 coulomb



d. None of the above

431. p1V1= p2V2 

a. Charle's Law



b. Boyle's Law



c. Ideal Gas Law



d. Joule's Law

432. A _______ is used to measure atmospheric pressure. 

a. Thermometer



b. Barometer



c. Manometer



d. None of the above

433. Work done in pushing a fluid across a boundary, Usually into or out of a system 

a. Flow Work



b. Flow Energy



c. Both a & b



d. None of the above

434. Which is not true about Heat (Q): 

a. Q is positive when heat is added to the body or system



b. Q is negative when heat is rejected by the body or system



c. Q is positive when heat is rejected by the body or system



d. None of the above

435. The standard reference atmospheric pressure 

a. 760 mmHg



b. 1 atm



c. 14.696 psia



d. All of the above

436. ______ is that property of a substance which remains constant if no heat enters or leaves the substance, while it does work or alters its volume, but which increases or diminishes should a small amount of heat enter or leave. 

a. Entrophy



b. Enthalpy



c. Specific Heat



d. None of the above

437.The acceleration of a particular body is directly proportional to the resultant force acting on it & inversely proportional to its mass. 

a. Pascal's Law



b. Joule's Law



c. Newton's Law



d. None of the above

438. Mass (not weight) per unit volume 

a. Specific Weight



b. Specific Volume



c. Density



d. None of the above

439. Composite property applicable to all fluids 

a. Entropy



b. Enthalpy



c. Specific Heat



d. None of the above

440. A classification of system in which mass does not cross its boundaries. 

a. Nonflow System



b. Open System



c. Closed System



d. None of the above

441. Gas being heated at constant volume is undergoing the process of. 

a. isometric



b. specific heat



c. enthalpy



d. isothermal

442. The heat per unit mass per degree change in temperature 

a. specific heat



b. isometric



c. conservation of energy



d. none of the above

443. A unit of pressure used in high vacuum technology, which is equal to 1mmhg. 

a. specific heat



b. isometric



c. isobaric



d. torr

444. The gas constant is equal to 

a. Cp – Cv



b. Cp + Cv



c. Cp – Cv + k



d. None of the above

445. The 1st Law of Thermodynamics on what principle? 

a. Conservation of Energy



b. Conservation of mass



c. Enthalpy



d. Isometric

446. A system having a rigid boundary that energy, work and mass does not cross its boundaries 

a. Specific Heat



b. Specific Gravity



c. Isolated System



d. Enthalpy

447. Sum of the internal energy of a substance and the product of pressure and volume. 

a. Specific Heat



b. Specific Gravity



c. Isolated System



d. Enthalpy

448. The ratio of the weight of a substance to the weight of some standard substance is called? 

a. Specific Heat



b. Specific Gravity



c. Isothermal



d. Specific Weight

449. Specific heat capacity in SI unit. 

a. kJ / kg.k



b. kJ / kg



c. kN / kg



d. None of the above

450. The Law of Thermodynamics that provides the basis for measuring the thermodynamic property of temperature. 

a. Charle’s Law



b. Boyle’s Law



c. Zeroth Law



d. Gas Law

451. The pressure of the confined gas is held constant, the volume directly proportional to the absolute temperature. 

a. Charle’s Law



b. Boyle’s Law



c. Zeroth Law



d. Gas Law

452. Regardless of the process, the change in enthalpy firm moles of ideal gas is 

a. Heat



b. Enthalpy



c. Entropy



d. Density

453. Ideal process are ________ process 

a. Irreversible



b. Reversible



c. Isothermal



d. Isometric

454. A state occurs when a system is in equilibrium 

a. Natural Environment



b. Closed System



c. Surrounding



d. Isentropic

455. A state occurs in isentropic process 

a. The change in entropy is 0



b. The change in entropy is 1



c. The change in enthalpy is 0



d. The change in enthalpy is 1

456. The SI unit of mass 

a. kg



b. g



c. N



d. None of the above

457. Anything that is outside the system boundary is called ________. 

a. Surrounding



b. Natural Environment



c. Closed System



d. Open System

458. A Thermodynamic Term That refers to any fixed region in a space 

a. Control Volume



b. Volume



c. Density



d. Natural Gas

459. The process that has no heat transfer 

a. Density



b. Isentropic Process



c. Isometric Process



d. Adiabatic

460. Another name of reversible adiabatic process 

a. Isentropic Process



b. Isometric Process



c. Isobaric Process



d. Isothermal Process

461. ______ of a Body is the absolute quantity of a matter in it. 

a. Mass



b. Weight



c. Density



d. Volume

462. _______ of a body means the force of the gravity Fg on the body 

a. Mass



b. Weight



c. Density



d. Volume

463. The law of conservation of mass states that ______. 

a. mass is indestructible



b. mass is destructible



c. mass is indestructible



d. none of the above

464. __________ is the energy stored within a body or substance by virtue of the activity and configuration of its molecules. 

a. Internal Energy



b. External Energy



c. Kinetic Energy



d. Potential Energy

465. The Product of the displacement of the body and the component if the force in the direction of the displacement. 

a. Nonflow Work



b. Flow Work



c. Work



d. None of the above

466. Is the energy in transit (on the move) from the one body or system to another solely because of a temperature between the bodies or systems. 

a. Work



b. Heat



c. Energy



d. None of the above

467. A classification of a system in which mass crosses its boundaries. 

a. Closed System



b. Open System



c. Isolated System



d. None of the above

468. The SI unit of pressure 

a. Pa



b. N



c. J



d. None of the above

469. The volume of a confined gas is held constant, the pressure is directly proportional to the absolute temperature. 

a. Charle’s Law



b. Boyle’s Law



c. Joule’s Law



d. Specific Heat

470. The compression of the gas in two or more cylinders in place of a single cylinder compressor 

a. Single Staging



b. Double Staging



c. Multistaging



d. None of the above

471 Is define as the ratio of the actual pressure of the vapor



a. Relative Humidity



b. Humidity Ratio



c. Dew Point



d. Adiabatic Saturation

472. Heat engine deriving its power from the energy liberated by the explosion of a mixture of some hydrocarbon, in a gaseous or vaporized form. 

a. Dual Combustion Engine



b. Internal Combustion Engine



c. External Combustion Engine



d. None of the above

473. Also called absolute humidity and specific humidity. 

a. Related humidity



b. Humidity ratio



c. Dew point



d. Adiabatic ratio

474. Is a steady flow process at total constant pressure through a control volume for which there is no heat? 

a. Adiabatic Saturation Process



b. Dew point



c. Adiabatic Ratio



d. None of the above

475. Fuels that may classified conveniently in solid, liquid and gaseous. 

a. Unleaded fuel



b. Diesel fuel



c. Fossil fuel



d. All of the above

476. Is a general name, without specific meaning unless the way in which it is measured or define by the context. 

a. Natural Value



b. Heating Value



c. Burning Value



d. Internal Value

477. Is the force of gravity on unit volume? 

a. Specific Weight



b. Specific Heat



c. Specific Pressure



d. Specific Volume

478. Give a reading as the length of some liquid column: water, alcohol, etc. 

a. Banometer



b. Nanometer



c. Thermometer



d. Manometer

479. If any one or more properties of a system change, the system is said to have undergone a _______. 

a. Cycle



b. System



c. Process



d. None of the above

480. Is a thermodynamic system that operates continuously with only energy (heat and work) crossing its boundaries? 

a. Heat Engine



b. Heat Reservoir



c. Heat Source



d. Heat Sink

481. _______________ is the temperature at which liquids start to boil or the temperature at which vapors begin to condense. 

a. Saturation Temperature



b. Sub cooled Liquid



c. Compressed Liquid



d. Saturated Liquid

482. ________________ is one which has a temperature lower than the saturation temperature corresponding to the existing pressure. 

a. Saturation Temperature



b. Sub cooled Liquid



c. Compressed Liquid



d. Saturated Liquid

483. _________________ is one which has a pressure higher than the saturation pressure corresponding to the existing temperature. 

a. Saturation Temperature



b. Sub cooled Liquid



c. Compressed Liquid



d. Saturated Liquid

484. __________________ is a liquid at the saturations which has temperature equal to the boiling point corresponding to the existing pressure. 

a. Saturation Temperature



b. Sub cooled Liquid



c. Compressed Liquid



d. Saturated Liquid

485. __________________ is the name given to a gaseous phase that is in contact with the liquid phase, or that is in the vicinity of a state where some of it might be condensed. 

a) Vapor



b) Saturated Vapor



c) Superheated Vapor



d) Wet Vapor

486. ___________________ is a vapor at the saturation conditions (saturation temperature and saturation pressure). 

a) Vapor



b) Saturated Vapor



c) Superheated Vapor



d) Wet Vapor

487. ___________________ is a vapor having a temperature higher than the saturation temperature corresponding to the existing pressure. 

a) Vapor



b) Saturated Vapor



c) Superheated Vapor



d) Wet Vapor

488. __________________ is a combination of saturated vapor and saturated liquid. 

a) Vapor



b) Saturated Vapor



c) Superheated Vapor



d) Wet Vapor

489. ___________________ represents the highest pressure and highest temperature at which liquid and vapor can coexist in equilibrium.



a) Critical Point



b) Boiling Point



c) Quality Point



d) None of the above

490. Heat that cause change in temperature at without a change in phase. 

a) Sensible Heat



b) Latent Heat



c) Thermo Heat



d) None of the above

491. Heat that cause change in phase without a change in temperature. 

a) Sensible Heat



b) Latent Heat



c) Thermo Heat



d) None of the above

492. What is the formula to convert °C to °F? 

a) °F = °C + 273



b) °F = 5/9 (°C - 32)



c) °F = 9/5 (°C)+32



d) None of the above

493. What is the formula to convert °F to °C? 

a) °C = °F + 273



b) °C = 5/9 (°F - 32)



c) °C = 9/5 (°F)+32



d) None of the above

494. ______________ is the base unit of thermodynamics temperature.



a) Celsius



b) Fahrenheit



c) Kelvin



d) None of the above

495. __________ is the unit of force. 

a) Newton



b) Pascal



c) Hertz



d) Joule

496. __________ is the unit of pressure and stress. 

a) Newton



b) Pascal



c) Hertz



d) Joule

97. _____________ is the difference between the actual temperature of superheated vapor and the saturation temperature for the existing pressure. 

a) Degrees of Superheat, °SH



b) Degrees of Sub cooled, °SB



c) Both a and b



d) None of the above

498. ____________is the difference between the saturation temperature for the given pressure and the actual sub cooled liquid temperature. 

a) Degrees of Superheat, °SH



b) Degrees of Sub cooled, °SB



c) Both a and b



d) None of the above

499. ___________ is the percent by weight that is saturated vapor. 

a) Quality, x



b) Percent Moisture, y



c) Vapor



d) Liquid

500. ____________ is the percent by weight that is saturated liquid. 

a) Quality, x



b) Percent Moisture, y



c) Vapor



d) Liquid

                       

1. Heat power 2. Lord Kelvin 3. First law of Thermodynamics 4. Second law of Thermodynamics 5. Classical thermodynamics 6. Statistical thermodynamics 7. System 8. Conservation of energy 9. Surroundings 10. Boundary 11. Closed system 12. Isolated system 13. Open system 14. All of the above 15. Control surface 16. Property 17. Intensive and extensive 18. Intensive property 19. Extensive property 20. Mass 21. Density 22. Specific properties 23. Thermal 24. Mechanical

                                        

25. 26. 27. 28. 29. 30. 31. 32. 33. 34. 35. 36. 37. 38. 39. 40. 41. 42. 43. 44. 45. 46. 47. 48. 49. 50. 51. 52. 53. 54. 55. 56. 57. 58. 59. 60. 61. 62. 63. 64. 65.

Phase Chemical State postulate Kj Simple compressible Process Path 2 Quasi-state or quasi- equilibrium process Control mass Control volume Thermal, phase, mechanical and chemical Cycle Isothermal process Isobaric process Isochoric or isometric process Remains constant No change with time No change with location Steady-flow process Internal energy Microscopic form of energy Macroscopic form of energy Thomas Young Translational energy Rotational kinetic energy Spin energy Sensible energy Latent energy Chemical energy Nuclear energy Heat transfer and work Zeroth law of thermodynamics R.H. Fowler Kelvin scale Rankine scale Ideal gas temperature scale Constant-volume gas thermometer Coulomb repulsion Constant-volume gas thermometer Triple point of water

                                        

66. Pressure 67. N/m^2 68. 14.223 psi 69. Pa 70. 10^5 71. 101,325 72. Absolute pressure 73. Vacuum pressure 74. Gage 75. Pitot tube 76. Barometer 77. 760 78. Pascal’s Law 79. Bourdon pressure gage 80. Heat 81. Joule 82. Kg ∙ m^2/s^2 83. 4.184 84. 10^-7 85. Law of conservation of energy 86. Thermodynamics 87. Enthalpy 88. Heat capacity 89. Molar heat 90. Specific heat 91. Hess’s Law 92. Entropy 93. Joule/Kelvin 94. Enthalpy 95. Compressed or subcooled 96. Saturated 97. Saturated 98. Superheated 99. Pure 100. Saturation temperature 101. Saturation pressure 102. Heat of fusion 103. Heat of vaporation 104. Latent heat 105. 333.7 kJ/kg 106. 2257.1 kJ/kg

                                        

107. 108. 109. 110. 111. 112. 113. 114. 115. 116. 117. 118. 119. 120. 121. 122. 123. 124. 125. 126. 127. 128. 129. 130. 131. 132. 133. 134. 135. 136. 137. 138. 139. 140. 141. 142. 143. 144. 145. 146. 147.

Maximum point Sublimation Kilocalorie BTU 1054 Heat Quality Pressure, temperature and specific volume Gas constant Universal gas constant to molar mass 8.314 Molar mass Specific heat Specific heat capacity 4185 J/kg∙ °C Specific volume of density Adiabatic Not to be passed All of the above Radiation Convection Conduction Conservation of mass principle PV = nRT Both heat transfer = 0; isentropic: reversible PV = nRT Thermal conductivity Greenhouse effect Boundary work 0.1 to 100 µm Emissive power Kirchhoff’s radiation law Black body Gray body Less than It is independent with the surface condition of the material 1 1 Stefan-Boltzmann law Conservation of energy principle

                                        

148. 149. 150. 151. 152. 153. 154. 155. 156. 157. 158. 159. 160. 161. 162. 163. 164. 165. 166. 167. 168. 169. 170. 171. 172. 173. 174. 175. 176. 177. 178. 179. 180. 181. 182. 183. 184. 185. 186. 187. 188.

Energy balance Mass and energy content of the control volume Network output to total heat input Second law of thermodynamics Kelvin-Planck statement Combustion efficiency Overall efficiency Energy efficiency rating Second law of thermodynamics Clausius statement Perpetual-motion machine Perpetual-motion machine of the first kind Perpetual motion machine of the second kind 1824 Sadi Carnot 4 Two isothermal and two adiabatic Carnot efficiency Carnot heat engine Carnot principle Second law of thermodynamics Isentropic True Internally reversible, adiabatic process Third law of thermodynamics Third law of thermodynamics Entropy balance relation Second law of thermodynamics Heat It is always zero Its saturated vapor pressure equals to the atmospheric pressure 0 degree Celsius and one atmosphere Zero Boyle’s Law V1/T1=V2/T2 Thickness of material/ thermal conductivity of material 186,000 miles/second Eff = 1 – (T2/T1) EER = 3.42 COP Absorbed heat and work required Law of Dulong and Petit

                                        

189. 190. 191. 192. 193. 194. 195. 196. 197. 198. 199. 200. 201. 202. 203. 204. 205. 206. 207. 208. 209. 210. 211. 212. 213. 214. 215. 216. 217. 218. 219. 220. 221. 222. 223. 224. 225. 226. 227. 228. 229.

Avogadro’s Perfect gas All of the above Amagat’s law Throttling process Joule-Thomson coefficient Sink reservoir Isentropic flow Ignition temperature Dalton’s law Joule’s law An ideal gas is a gas that is not a superheated vapor movement of heat Kelvin heat latent heat thermal expansion thermal stress Internal Energy Specific Heat Capacity Equilibrium Vapor Pressure temperature Phase diagram Internal Energy calorie temperature Zero-Point Energy 10 K Helmholtz free energy 0.67 m 0.18 in 1400 J Gibbs free energy heat relative humidity Sublimation Convection change three times increases no pressure

                                        

230. 231. 232. 233. 234. 235. 236. 237. 238. 239. 240. 241. 242. 243. 244. 245. 246. 247. 248. 249. 250. 251. 252. 253. 254. 255. 256. 257. 258. 259. 260. 261. 262. 263. 264. 265. 266. 267. 268. 269. 270.

the relative humidity decreases convection current blackbody Conduction gram-mole Maxwell speed Distribution Forced Convection point function path function boundary control mass control volume -256 heat enters the substance. 15 shape of the object metals glass increases Kelvin temperature reduced by half it increases by a factor of square root of 2 entropy Isochoric process isobaric increases Closed system normal boiling point wet steam flash steam dryness fraction thermopile any holes in the object expand as well one BTU pressure Sir James Dewar Isobaric raising the temp and lowering the temp the second law of thermodynamics Clausius statement mean free path

                                        

271. 272. 273. 274. 275. 276. 277. 278. 279. 280. 281. 282. 283. 284. 285. 286. 287. 288. 289. 290. 291. 292. 293. 294. 295. 296. 297. 298. 299. 300. 301. 302. 303. 304. 305. 306. 307. 308. 309. 310. 311.

9.86 x 10^4 N/m^2 6 x 10^15 tons standard atmospheric pressure Pascal’s law Gauge Pressure 62.4 lb surface tension Torricelli’s Theorem diffusion 1948 dew point cycle Bulk Properties Joule-Thomson process Otto Cycle 24.6 J/K conservation of energy 1700 J 12 kJ 17.66 % Sensible heat Joseph Black Latent Heat Third Law of thermodynamics 1/860 W.h Polytropic process steady flow Carnot Cycle 733.33 kPa Sadi Carnot 13.33 ft^3/lbm 3300 lbf-ft/lbm 24.9 ft^3 z = pV/ RT 1.79 kJ/ kg-˚C 2 x10^6 kJ 3.16 kg 1.1577 BTU/lbm-˚R 15.7 BTU 0.179 K/s 4474.23 N

                                        

312. 313. 314. 315. 316. 317. 318. 319. 320. 321. 322. 323. 324. 325. 326. 327. 328. 329. 330. 331. 332. 333. 334. 335. 336. 337. 338. 339. 340. 341. 342. 343. 344. 345. 346. 347. 348. 349. 350. 351. 352.

2474.23 N 42.41 ft^3 28.6 psia 108 hp W = mRTln (V2/V1) 1124 cal -364 BTU/lbm 12 kJ 0.02 ft^3/lbm 66 kgf 1000 kgf/m3 286 Both a & b 209 psia 416 999 K 3800 1620 °R 0.2148 lb 121 100 125 J 443 kPa 48.75 N 4875 j 300 kJ 1 485 672 298.645 65.23 psi 70 450 N 900,000lb/hr;625 ft/s981 N 981 N T2=1.620ºR, ▲H = 122.83 Btu 70.658 kpa 900,000 lb/hr;625 ft/s 11,772 N-m and 6.26m/s 10m/s 217.17 kpa

                                        

353. 354. 355. 356. 357. 358. 359. 360. 361. 362. 363. 364. 365. 366. 367. 368. 369. 370. 371. 372. 373. 374. 375. 376. 377. 378. 379. 380. 381. 382. 383. 384. 385. 386. 387. 388. 389. 390. 391. 392. 393.

796.32 L 7.85 375 kg/s 87°C 0.085 m³/min 24m/s 33.9 ft 625 fpm 50 lbm 33.9 ft 1.38 -420Btu 7.9 °C 1.3 x 108 J -540 J 0.77 kg liter-1 11,120N 5.18 l 18 kg 111 psi 1214Btu / lb 394 lb –1664 kJ/min 7.849 ft3 1.356 339.4 K 1620°R 710°R 265.4°C, 430.7kJ/kg, 71.4kJ/kg, 1.0327kJ/(kg)(K),502.1 kJ/kg 204.2°C, -703.2 kJ/kg, -84.15 kJ/kg, -1.7505 kJ/(kg)(K),-787.4 kJ/kg 95.20% 95.56% 1378.7 kJ -1384.7 kJ 96% 97.6%,2713 kJ/kg 14026.5 m³ 126m³ 54.60% 190 in³ 217.7 kPa

                                      

394. 62850 joules 395. 419 000 joules 396. 2238 watts 397. 9 Newton’s 398. 0.998 hp 399. 1.16 kcal 400. 440 cal 401. Thermodynamics 402. Boyle’s Law 403. 6.0225 x 10^23 mol-1 404. all of the above 405. isolated system 406. evaporation 407. 1 gm/cm³ 408. when a body is inversed in a fluid, the fluid exerts a upward force on the body whose magnitude is equal to the weight of the displaced fluid. 409. solid 410. V = C 411. specific heat 412. > 1 413. Law of Conservation of Mass 414. potential energy 415. elastic work 416. Gabriel Daniel Fahrenheit 417. Anders Celsius 418. barometer 419. Momentum 420. all of the above 421. Energy is a scalar quantity 422. System 423. Flow rate 424. Energy 425. Specific Heat 426. Thermodynamics 427. 1st Law of Energy Conservation 428. Vector Quantity 429. Internal Energy 430. 1.60210 x 10-19 coulomb 431. Boyle's Law 432. Barometer

                                        

433. 434. 435. 436. 437. 438. 439. 440. 441. 442. 443. 444. 445. 446. 447. 448. 449. 450. 451. 452. 453. 454. 455. 456. 457. 458. 459. 460. 461. 462. 463. 464. 465. 466. 467. 468. 469. 470. 471. 472. 473.

Both a & b Q is positive when heat is rejected by the body or system All of the above Entrophy Newton's Law Density Enthalpy Closed System isometric specific heat torr Cp – Cv Conservation of Energy Isolated System Enthalpy Specific Gravity kJ / kg.k Zeroth Law Charle’s Law Heat Reversible Natural Environment The change in entropy is 0 kg Surrounding Control Volume Adiabatic Isentropic Process Mass Weight mass is indestructible Internal Energy Work Heat Open System Pa Boyle’s Law Multistaging Relative Humidity Internal Combustion Engine Humidity ratio

                          

474. 475. 476. 477. 478. 479. 480. 481. 482. 483. 484. 485. 486. 487. 488. 489. 490. 491. 492. 493. 494. 495. 496. 497. 498. 499. 500.

Adiabatic Saturation Process Fossil fuel Heating Value Specific Weight Manometer Process Heat Engine Saturation Temperature Sub cooled Liquid Compressed Liquid Saturated Liquid Vapor Saturated Vapor Superheated Vapor Wet Vapor Critical Point Sensible Heat Latent Heat momentum °C = 5/9 (°F - 32) Kelvin Newton Pascal Degrees of Superheat, °SH Degrees of Sub cooled, °SB Quality, x Percent Moisture, y