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Question

When 1 moe of ice melts at 0oC and at constant pressure of 1 atm, 1440 calories of heat are absorbed by the system. The molar volume of ice and water are 0.0196 and 0.0180 litre respectively. Which of the following is correct?

A
ΔUΔH
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B
ΔU=1548 cal
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C
ΔU=1056 cal
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D
None of the above
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Solution

The correct option is A ΔUΔH
Given, p=1 atm=76×13.6×981 dynecm2V1=18 cm3,V1=19.6 cm3
Since ΔH=qp
= heat absorbed by the system at constant pressure
=1440 calories

In the equation, ΔH=ΔU+pΔV
ΔHΔU=pΔV
pΔV=1×(0.0180.0196) atm L
pΔV=0.0016×101.3 J=0.16 J
pΔV=0.164.2 calories
pΔV=0.038 calories
Since pΔV is very small as compared to ΔU, pΔV can be neglected.
Thus, ΔHΔU=1440 calories

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