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JEE Main 31 August 2021, Shift 1, Chemistry Q55

Question 55 of 90 in this shift, Chemistry question 25 of 30, Section B.

Consider the following cell reaction

\mathrm{Cd_{(s)}+Hg_2SO_{4(s)}+\frac{9}{5}H_2O_{(\mathit{l})}\rightleftharpoons CdSO_4\cdot\frac{9}{5}H_2O_{(s)}+2Hg_{(\mathit{l})}}

. The value of

\mathrm{E^0_{cell}}

is 4.315 V at 25°C. If

\Delta\mathrm{H}^\circ=-825.2

kJ mol

^{-1}

, the standard entropy change

\Delta\mathrm{S}^\circ

in J K

^{-1}

is __________. (Nearest integer) [Given : Faraday constant

=96487

C mol

^{-1}

]

Official answer

NTA final key.

Same idea in other shifts