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The cell potential (Ecell) of a reaction is related as ΔG=nF Ecell, where ΔG represents maximum useful electrical work.
n = no. of moles of electrons exchanged during the reaction.
For reversible cell reaction d(ΔG)=(ΔV)dp(ΔS)dT
At const. P, d(ΔG)=(ΔS)dT
At const. P, ΔG=ΔHTΔS. (1)
ΔG=ΔH+T(d(ΔG)ΔT)P. (2)
(dEcelldT)p is known as temperature coefficient of the emf of the cell.

At 300K, ΔH for the reaction Zn+2AgClZnCl2+2Agis218 kJ/mole while emf of the cell was 1.015V.(dEdT)p of the cell is

A
4.2×104VK1
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B
3.81×104VK1
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C
0.11VK1
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D
7.62×104VK1
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Solution

The correct option is B 3.81×104VK1
ΔH=ΔG+TΔS
=nFE+nF(dEdT)T
218×103=2×96500×1.015+2×96500×300(dEdT)p
dEdT=3.81×104VK1

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