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 J 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 from 32.0 to 37.4°C. What is the specific heat per gram and per mole of this substance? (continued on next page) 125

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 J 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 from 32.0 to 37.4°C. What is the specific heat per gram and per mole of this substance? (continued on next page) 125

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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