   # Suppose you burned 1.500 g of benzoic acid, C 6 H 5 CO 2 H, in a constant-volume calorimeter and found that the temperature increased from 22.50 °C to 31.69 °C. The calorimeter contained 775 g of water, and the bomb had a heat capacity of 893 J/K. Calculate Δ U per mole of benzoic acid. ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640

#### Solutions

Chapter
Section ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640
Chapter 5, Problem 45PS
Textbook Problem
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## Suppose you burned 1.500 g of benzoic acid, C6H5CO2H, in a constant-volume calorimeter and found that the temperature increased from 22.50 °C to 31.69 °C. The calorimeter contained 775 g of water, and the bomb had a heat capacity of 893 J/K. Calculate ΔU per mole of benzoic acid.

Interpretation Introduction

Interpretation:

The internal energy per mole per mole of benzoic acid has to be determined.

Concept Introduction:

Sum of all energies transferred as heat in the system

qr + qbomb +qwater=0

Heat energy required to raise the temperature of 1g of substance by 1K.Energy gained or lost can be calculated using the below equation.

q=C×m×ΔT

Where, q= energy gained or lost for a given mass of substance (m), C =specific heat capacity, ΔT= change in temperature.

### Explanation of Solution

Given,

Specific heat capacity of bomb=893J/K

qwater=4.184JK/g(775g)(9.19K)=2.9×104J

qbomb=893J/K×9.19K =8.20×103J

Substitute in qr + qbomb +

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