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Question

The standard emf of the cell,Cd(s)|CdCl2(aq)(0.1 M)||AgCl(aq)|Ag(s).


In which the cell reaction is Cd(s)+2AgCl(s)2Ag(s)+Cd2+(aq)+2Cl(aq) is 0.6915 V at 0oC and 0.6573 V at 25oC.

The enthalpy change of the reaction at 25oC is:

A
+48.179 kJ
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B
234.7 kJ
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C
+0.28 kJ
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D
167.26 kJ
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Solution

The correct option is D +0.28 kJ
Given E0 at 00C=273K=0.6915V
Given E0 at 250C=298K=0.6573V
Applying Gibbs Helmholtz equation
ΔG=ΔHTΔS Eq1
According to the formula
ΔG1(273K)=nFE0=2×96500×0.6915=11.96kJ
ΔG1(298K)=nFE0=2×96500×0.6574=13.03kJ
Using Eq 1
11.96=ΔH1273ΔS
13.03=ΔH2298ΔS
Finding for ΔS
13.0311.96=(298+273)ΔS
ΔS=0.0428kJK
ΔH2=13.03298×0.0428=0.28kJ

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