   Chapter 5, Problem 43PS

Chapter
Section
Textbook Problem

Sulfur (2.56 g) was burned in a constant-volume calorimeter with excess O2(g). The temperature increased from 21.25 °C to 26.72 °C. The bomb has a heat capacity of 923 J/K, and the calorimeter contained 815 g of water. Calculate ΔU per mole of SO2 formed for the reactionS8(s) + 8 O2(g) → 8 SO2(g)

Interpretation Introduction

Interpretation:

The change in internal energy per mole of SO2 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.

The internal energy, U is the sum of kinetic energy and the potential energy inside the system.

Change in internal energy,ΔU, is the measures of energy that is transferred as heat and work from the system or to the system.

ΔU=qv+Wv

Where q = heat energy absorbed or released, W =work done to the system or from the system.

W=-P(ΔV)

Where,ΔV is the change in volume, =0, at constant volume and P is the pressure.

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,

ΔV= 0

Work done at constant volume, Wv=0

Change in internal energy, ΔU=qv+Wv

Specific heat capacity of bomb=923J/K

Mass of Sulphur=2.56g

Mass of water=815g

qwater=4.184JK/g(815g)(5.47K)=18.65KJ

qbomb=923J/K×5.7K =52

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