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Prelaboratory Questions Name Laboratory Section 1. The temperature of a 15.0 g sample of a metal (specific heat 0.040 J/g-°C) is raised by 18.2°C. How much heat (in J) has been absorbed by the metal? 2. A calorimeter and its contents have a heat capacity of 70 J/°C. A reaction occurs in this calorimeter at atmospheric pressure. The temperature of the system rises 10.5°C when one mole of product is formed. Calculate the heat change for this reaction. 3. If 100 g of a solution (specific heat of 0.32 J/g.°C) undergoes a reaction in which 74.84 T of heat is released, what is the temperature change (AT) of this solution? Does the tem- perature of the solution increase or decrease? 4. 30.0 g of a substance (molar mass: 46 g/mol) required 262 J of heat to raise its temperature S0.02 0 to 37.4°C. What is the specific heat per gram and per mole of this substance? (continued on next page) 125

Prelaboratory Questions Name Laboratory Section 1. The temperature of a 15.0 g sample of a metal (specific heat 0.040 J/g-°C) is raised by 18.2°C. How much heat (in J) has been absorbed by the metal? 2. A calorimeter and its contents have a heat capacity of 70 J/°C. A reaction occurs in this calorimeter at atmospheric pressure. The temperature of the system rises 10.5°C when one mole of product is formed. Calculate the heat change for this reaction. 3. If 100 g of a solution (specific heat of 0.32 J/g.°C) undergoes a reaction in which 74.84 T of heat is released, what is the temperature change (AT) of this solution? Does the tem- perature of the solution increase or decrease? 4. 30.0 g of a substance (molar mass: 46 g/mol) required 262 J of heat to raise its temperature S0.02 0 to 37.4°C. What is the specific heat per gram and per mole of this substance? (continued on next page) 125

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Prelaboratory Questions Name Laboratory Section 1. The temperature of a 15.0 g sample of a metal (specific heat 0.040 J/g-°C) is raised by 18.2°C. How much heat (in J) has been absorbed by the metal? 2. A calorimeter and its contents have a heat capacity of 70 J/°C. A reaction occurs in this calorimeter at atmospheric pressure. The temperature of the system rises 10.5°C when one mole of product is formed. Calculate the heat change for this reaction. 3. If 100 g of a solution (specific heat of 0.32 J/g.°C) undergoes a reaction in which 74.84 T of heat is released, what is the temperature change (AT) of this solution? Does the tem- perature of the solution increase or decrease? 4. 30.0 g of a substance (molar mass: 46 g/mol) required 262 J of heat to raise its temperature S0.02 0 to 37.4°C. What is the specific heat per gram and per mole of this substance? (continued on next page) 125
Transcribed Image Text:Prelaboratory Questions Name Laboratory Section 1. The temperature of a 15.0 g sample of a metal (specific heat 0.040 J/g-°C) is raised by 18.2°C. How much heat (in J) has been absorbed by the metal? 2. A calorimeter and its contents have a heat capacity of 70 J/°C. A reaction occurs in this calorimeter at atmospheric pressure. The temperature of the system rises 10.5°C when one mole of product is formed. Calculate the heat change for this reaction. 3. If 100 g of a solution (specific heat of 0.32 J/g.°C) undergoes a reaction in which 74.84 T of heat is released, what is the temperature change (AT) of this solution? Does the tem- perature of the solution increase or decrease? 4. 30.0 g of a substance (molar mass: 46 g/mol) required 262 J of heat to raise its temperature S0.02 0 to 37.4°C. What is the specific heat per gram and per mole of this substance? (continued on next page) 125
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