For given cell reaction n=2
and ΔG∘=−nFE∘,cellΔG∘=ΔH∘−TΔS
Then ΔH∘=825.2×103J/mole
T=298K
E∘cell=4.315V
F=96487C
ΔS∘=T−(−nFE∘cell−ΔH)
ΔS∘=298−(−2×96487×4.315−(−825.2×103))=298832.682×103−825.2×103=2987482×103
ΔS∘=25.1J/k
Consider the following cell reaction Cd(s)+Hg2SO4(s)+59H2O(l)⇌CdSO4⋅59H2O(s)+2Hg(l).
The value of Ecell0 is 4.315V at 25∘C. If ΔH∘=−825.2kJmol−1, the standard entropy change ΔS∘ in JK−1 is _________ . (Nearest integer)
[Given : Faraday constant =96487Cmol−1]
Held on 31 Aug 2021 · Verified 6 Jul 2026.
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