   Chapter 5, Problem 46PS

Chapter
Section
Textbook Problem

A 0.692-g sample of glucose, C6H12O6, was burned in a constant-volume calorimeter. The temperature rose from 21.70 °C to 25.22 °C. The calorimeter contained 575 g of water, and the bomb had a heat capacity of 650 J/K. What is ΔU per mole of glucose?

Interpretation Introduction

Interpretation:

The change in internal energy per mole of C6H12O6 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

Given,

Specific heat capacity of bomb=650JK

Mass of C6H12O6=0.692g

Mass of water= 575g

qwater=4.184JK/g(575g)(3.52K)=8

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