Question

# 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=ΔH−TΔS. (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+2AgCl→ZnCl2+2Agis−218 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 −3.81×10−4VK−1ΔH=ΔG+TΔS =−nFE+nF(dEdT)T −218×103=−2×96500×1.015+2×96500×300(dEdT)p dEdT=−3.81×10−4VK−1

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