Mock 3R Chemistry Q

learnfastreview.com.ph (0917) 327-9436, (02) 523-0475 NMAT CHEMISTRY SIMULATIONS (MOCK 3R) DIRECTIONS: Select the best answer to each of the following questions and blacken the appropriate space on your answer sheet. 1. Given:

𝑃 → 𝑃𝐻3 + 𝐻2 𝑃𝑂2 − (alkaline) When balanced, what will be the sum of the coefficients of the products? a. 3 b. 4 c. 13 d. 14 2. Which of the following is not a conjugate acid-base pair? a. 𝑁𝐻4 +, 𝑁𝐻3 c. 𝐻2 𝑂, 𝑂𝐻 − − b. 𝑁𝐻3 , 𝑁𝐻2 d. 𝐻2 𝑆𝑂4 , 𝑂𝐻 −

For numbers 10 and 11, consider this situation. Paul found a certain unknown compound to be 31.0% carbon, 5.2% hydrogen, 27.6% oxygen, and 36.2% nitrogen. The molecular weight was experimentally determined to be approximately 460. Atomic Weights: H=1 C = 12 N = 14 O = 16

3. What nuclear process occurred if 226 88𝑋 results from the emission of particle by 226 𝑌 ? 89 a.  decay b. - decay c. + decay d. K-electron capture

10. What is the empirical formula of the compound? a. C3H6O2N3 c. C6H10O5N5 b. C5H2ON3 d. C10H20O7N10

4. In the combustion of ethyne in oxygen, 8 g of O2 was present. Ideally, what amount of ethyne could have reacted with all that O2, and how much CO2 could have been produced? a. 13 g ethyne; 11 g CO2 b. 2.3 g ethyne; 7.3 g CO2 c. 3.2 g ethyne; 6.4 g CO2 d. 2.6 g ethyne; 8.8 g CO2

11. Which is a possible molecular formula for the compound? a. C4H2O(NO)5(CO)2(NH2)5(CH)6(OH)2 b. C4(NO)4(CO)2(NH2)8(CH)6(OH)2 c. C18H2O2(CO)2(NH2)4(CH3)4(OH)2 d. C18H2(CO)2(NH2)6(CH3)4(OH)2

5. What kind of particle was emitted if 258 101𝐴 underwent decay and the result was 254 99𝐵 ? a. alpha particle c. positron b. electron d. gamma ray 6. Fusion is most likely to occur with the: a. Combination of 2 1H nuclei b. Combination of 2 2H nuclei c. Splitting apart of a single 244 95𝐴𝑚 nucleus d. Splitting apart of a single 245 95𝐴𝑚 nucleus

For numbers 12 and 13 consider this situation. A sample of 0.025 M KOH stands at 250C, where 100.4  2.5 12. What is the pH of this sample? a. 1.6 c. 13 b. 12.4 d. 13.6 13. What is the pOH of this sample? a. 1.6 c. 13 b. 12.4 d. 13.6 14. Given this graph:

7. Mike can prepare methanol from bromomethane by adding _____ to the latter. a. Hydrogen gas c. Sulfuric acid b. Sodium hydroxide d. Heat energy and light 8. At 250C in the equilibrium 𝑁2 (𝑔) + 𝑂2 (𝑔) ↔ 2𝑁𝑂 Kp = 4.8 x 10-31 which species will dominate? a. NO and O2 c. N2 and O2 b. N2 and NO d. None 9. If the equilibrium constant KC for 𝐹2 (𝑔) ↔ 2𝐹 (𝑔) At a certain temperature is 7.3 x 10-13, what is KC for 1 𝐹2 (𝑔) ↔ 𝐹 (𝑔)? a. √7.3 × 10−13 b. 3.65 x 10-13

2

What type of reaction does the forward reaction represent? a. Endothermic c. Both A and B b. Exothermic d. Neither A nor B

c. 1.37 x 10-12 d. 7.3 x 10-13

1

15. NO2 is a gas whose density is 73.5 g/L. What pressure will it exert at a temperature of 270C? a. 43.05 atm c. 86.10 atm b. 81.81 atm d. 1808.10 atm 16. If 25 13𝐾𝑦 emits a gamma ray, then the daughter nucleus is: a. 24 c. 21 11𝑁𝑐 13𝐾𝑦 25 b. 13𝐾𝑦 d. 24 14𝑆ℎ𝑓 For numbers 17 and 18, refer to the following periodic table.

21. What happens to aluminium in the reaction: 2𝐴𝑙 + 3𝑁𝑖(𝑁𝑂3 )2 → 2𝐴𝑙(𝑁𝑂3 )3 + 3𝑁𝑖 a. Reduced and its oxidation number increases b. Reduced and its oxidation number decreases c. Oxidized and its oxidation number increases d. Oxidized and its oxidation number decreases 22. The Law of Multiple Proportions applies to what pair of compounds? a. KCl and KClO3 c. H2O and H2O2 b. MgSO4 and MnSO4 d. NaBr and NaCl 23. Which procedure is most likely to increase the solubility of a gas in a liquid? a. Constant stirring c. Adding more solvent b. Heating the solution d. Increasing the pressure

17. Which pair of elements below has the highest and lowest electron affinities, respectively? a. He and Rn c. Ac and F b. F and Fr d. Li and Nb 18. Which of the following are all metalloids? a. Sc, Lr, Zn, Uub c. Ge, As, Te b. B, O, F, Ne d. Ne, Ar, Kr 19. What will be the product of the following reaction?

24. Along a row in the periodic table, elements have the same: a. Energy level c. Atomic radius b. Electronegativity d. Ionization energy 25. What is the correct identity of X in the reaction: 234 0 91𝑃𝑎 → 𝑋 + −1𝛽 ? 234 234 a. 92𝑈 c. 90𝑇ℎ b. 235 d. 232 92𝑈 90𝑇ℎ 26. The half-life, t1/2, of radioactive phosphorous, 32P, is 14 days. Given 1.0 mg 32P, how much will remain after 42 days? a. 0.5 mg c. 0.125 mg b. 1.25 mg d. None 27. Which statement is NOT true? a. An element melts at a definite temperature. b. An element is changed into another substance by heat in the absence of air or another substance. c. An element may combine with another to form a compound. d. An element is made of the same kind of atom. 28. Which of the following is a property of all metals? a. All are hard. b. All are combined easily with oxygen. c. All are solids at room temperature. d. All are conductors of heat and electricity. 29. No two electrons in the same atom can have the same set of quantum numbers is the statement of: a. Hund’s Rule of Multiplicity b. Dalton’s Atomic Theory c. Heisenberg’s Uncertainty Principle d. Pauli’s Exclusion Principle

20. In which substance is the oxidation state of nitrogen zero? a. N2 c. NO2 b. NH3 d. N2O

30. As you enter a building, you observe a beam of light from the glass roof. What is the phenomenon? a. Brownian movement c. Tyndall effect b. Peptization d. Adsorption

2

31. Which of the following substances will exhibit the highest boiling point? a. CCl4 c. CH4 b. CO2 d. Cl2HCCHCl2

39. The molecular weight of a substance is 128 and its equivalent weight in a particular reaction is 24. A 1.0 M solution of this substance will have a normality of: a. 5.33 N b. 0.50 N c. 2 N d. 0.25 N

32. Which of the following is/are true? a. At 1 atm the boiling point of water is 1000C. b. The vapour pressure of 40 mL of water heated at 400C is twice the vapour pressure of 20 mL of water heated at the same temperature. c. Generally, non-polar substances have higher boiling points than polar substances. d. Choices a and b are true.

40. What volume of 0.1 M NaOH is needed to neutralize 25 mL of 0.1 M H2SO4? a. 12.5 mL b. 25 mL c. 50 mL d. 100 mL

33. Which substance evaporates more rapidly at a given temperature? a. Substance that has high vapour pressure at room temperature b. Substance with molecules having strong forces of attraction c. Substance with high boiling temperature d. Substance with high heat of vaporization 34. What is the maximum number of grams of water at 100C that can be heated to 300C by the addition of 40 calories of heat? a. 1.0 c. 20 b. 2.0 d. 30

41. What is the normality of an acid solution if 50 mL of the solution requires 48.16 mL of 0.1879 N alkali for neutralization? a. 0.4000 N c. 0.1827 N b. 0.2678 N d. 0.1274 N 42. Which is the conjugate base of H2SO4? a. SO3-2 b. S-2 c. HSO3d. HSO443. Which statement best describes a solution with a pH of 3? a. It has an H+ concentration of 1 x 103 and is acidic. b. It has an H+ concentration of 1 x 10-3 and is acidic. c. It has an H+ concentration of 1 x 103 and is basic. d. It has an H+ concentration of 1 x 10-3 and is basic. 44. Which of the following will produce a solution with a pH less than 7? a. KCN b. K2SO4 c. NH4Cl d. NaNO3

35. Exothermic is a term used to describe a reaction: a. That occurs at a low temperature b. For which heat is a reactant c. For which heat is a product d. That occurs at a high temperature

45. In any of the p, d, or f orbitals, separate orbitals before any orbital This principle is referred to as: a. de Broglie’s Principle b. Pauli’s Exclusion Principle

36. Which type of reaction does the Haber process below represent? 𝑁2 (𝑔) + 3𝐻2 (𝑔) → 2𝑁𝐻3 (𝑔) + 𝐻𝑒𝑎𝑡 a. Exothermic, with an increase in entropy b. Exothermic, with a decrease in entropy c. Endothermic, with an increase in entropy d. Endothermic, with a decrease in entropy

46. If 75% of the isotopes of an element have a mass of 35 amu and 25% of the isotopes have a mass of 37 amu, what is the atomic mass of the element? a. 35 amu c. 36 amu b. 35.5 amu d. 37 amu

37. Which change would most likely increase the rate of a chemical reaction? a. Decreasing the reactants’ concentration b. Decreasing the reactants’ surface c. Cooling the reaction mixture d. Adding a catalyst to the reaction mixture 38. Given the reaction below at equilibrium. 𝑋2 (𝑔) + 2𝑌2 (𝑔) ↔ 2𝑋𝑌2 (𝑔) + 80 𝑘𝑐𝑎𝑙 The equilibrium point will shift to the left if the pressure is: a. Increased and the temperature is increased b. Increased and the temperature is decreased c. Decreased and the temperature is increased d. Decreased and the temperature is decreased

electrons tend to occupy can have two electrons. c. Aufbau’s Principle d. Hund’s Principle

47. Which of the following molecules is the most acidic? a. CH3COOH c. CHCl2CH2COOH b. CH2ClCOOH d. CH3CCl2COOH 48. If propylene is shaken with cold neutral KMnO4 solution, the primary organic compound will be: a. CH3CH(OH)CH2OH c. CH3CH2CH2OH b. CH3CH2CH2MnO4 d. CH2(OH)CH(OH)CH2OH 49. When propyne reacts with 2 moles of HBr, the major product formed is : a. 1,1-dibromopropane c. 2,2-dibromopropane b. 1,2-dibromopropane d. 1-bromopropane 50. Which compound contains double bonds, does not decolorize bromine water, and reacts with chlorine in the presence of ferric chloride? a. Ethyl alcohol c. Benzene b. Butane d. Cyclohexene

3