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 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 and per mole of this substance?

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 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 and per mole of this substance?

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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