Section B : Numerical Type Questions Consider the following cell reaction, {\Cd}({\s})+{\Hg}_{2} {\SO}_{4}({\s})+\frac{9}{5} {\H}_{2} {\O}({\l})⇌ {\CdSO}_{4} . \frac{9}{5} {\H}_{2} {\O}({\s})+2 {\Hg}({\l}) The value of \E_{{\cell }}^\circ is 4.315 {\V} at 25^\circ {\C}. If \\Delta\H^\circ=-825.2 {\kJ} {\mol}^{-1}, the standard entropy change \\Delta\S^\circ in \J{\K}^{-1} \is ... . (Nearest integer) [Given, Faraday constant =96487 {\C} {\mol}^{-1}] [31 Aug 2021 Shift 1]

Electrochemistry Part 1

Section: Chemistry

Question : 2 of 100

Marks: +1, -0

Section B : Numerical Type Questions
Consider the following cell reaction,

Cd(s)+Hg2SO4(s)+

H2O(l)⇌CdSO4.

H2O(s)+2‌Hg(l)

The value of Ecell° is 4.315V at 25°C. If ΔH°=−825.2‌kJ‌mol−1, the standard entropy change ΔS° in JK−1‌is.... (Nearest integer)
[Given, Faraday constant =96487Cmol−1]

[31 Aug 2021 Shift 1]

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