   Chapter 5, Problem 44PS

Chapter
Section
Textbook Problem

Suppose you burned 0.300 g of C(s) in an excess of O2(g) in a constant-volume calorimeter to give CO2(g).C(s) + O2(g) → CO2(g)The temperature of the calorimeter, which contained 775 g of water, increased from 25.00 °C to 27.38 °C. The heat capacity of the bomb is 893 J/K. Calculate ΔU per mole of carbon.

Interpretation Introduction

Interpretation:

The change in internal energy per mole of Carbon under constant volume 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=837J/K

Mass of carbon =1g

Mass of water=775g

qwater=4.184JK/g(775g)(2.32K)

qwater=7.52×104J

qbomb=837J/K×2.32K =1

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