Experiment-7-Specific Heat of Metals

Group 8

Section: 2D-MT

Members: Harvey Mher M. Rarang Maika L. Regala Chelejan Mhare U. Regino Erik Kristian B. Sabio Mica Gienela A. Sanchez Arianne Nicole Denise T. Yoro

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Date Performed: November 13, 2015 Date Submitted: November 27, 2015

EXPERIMENT 7 – SPECIFIC HEAT OF METALS I. Abstract The experiment aimed to determine the specific heat of a metal with the known mass, in our case Aluminum, by observing the behaviour of the temperature or the transfer of heat between the metal and the calorimeter and water. The metal was heated at 85.9°C and dropped in the 14.8°C calorimeter with water. The data gathered were taken down for the specific heat computation. Based on the results that we have obtained, the specific heat of the Aluminum is 0.566 cal/gCº and calculated 163% of error because the standard heat capacity of an Aluminum metal is 0.215 cal/gCº. In conclusion, the amount of heat lost by the metal is equal to the amount of heat absorbed by the water and colorimeter. II. Question and Answer 1. Define the following: A. Heat – it is a form of energy that is transferred between a system and the surroundings in a manner of higher temperature to lower temperature. B. Heat capacity – it is the amount of energy needed by a metal or an object to increase its temperature by one degree. 2. Why is it desirable to have the water a few degrees colder than room temperature when the initial temperature is taken? As mentioned above, heat flows from a higher temperature to a lower temperature giving us hint that the water must be few degrees colder than the room temperature to increase its ability in absorbing heat and be able to have an observable result.(2nd Law of Thermodynamics) 3. Why is the mass of the outer shell of the calorimeter and the insulating ring not included in the data for this experiment?

The insulating ring and the outer shell of the calorimeter is not included in the data of this experiment because they are not part of the isolated system. The insulating ring and the outer shell of the calorimeter just minimize the flow of heat into or out of the apparatus. 4. What does this experiment show about the specific heat of water? The experiment shows that the water was able to absorb more heat than the calorimeter because it has higher specific heat. 5. How does the heat conductivity of the metal is used in this experiment affect the accuracy of the results? The different extensive and intensive properties of every metal can directly affect the rate of heat conduction that causes on the variation in the accuracy of the results obtained. 6. Why should the hot metal be dry before it is introduced to the cold water? The metal should be dry before introducing to the cold water for the improvement of the heat exchange occurring between the objects. Maximizing the surface area of the metal in contact to the water and calorimeter is necessary. 7. 837 calories of heat are required to heat 100.00 grams of copper from 10.0ºC to 100.0ºC. What is the specific heat of copper? Qcopper= (mcopper)(ccopper)(t) 837 cal = (100g)(ccopper)(100°C-10°C) 837 cal = (100g)(90°C)(ccopper) 837 cal = 9000 g C° (ccopper) 9000 g C° 9000 g C° 0.093 cal= ccopper g C°