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Electrochemistry question

2018 · Shift 2 · Q12

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JEE Advanced
Chemistry
Electrochemistry
2018 · Shift 2 · Q12

Electrochemistry question

2018 · Shift 2 · Q12

JEE AdvancedChemistryElectrochemistryNumerical+3 / −1

Consider an electrochemical cell :

A\left( s \right)\left| {{A^{n + }}\left( {aq,2M} \right)} \right|{B^{2n + }}\left( {aq,1M} \right)\left| {B\left( s \right).} \right.

The value of

\Delta {H^ \circ }

for the cell reaction is twice that of

\Delta {G^ \circ }

at

300K.

If the

emf

of the cell is zero, the

\Delta {S^ \circ }

(in

J\,{K^{ - 1}}mo{l^{ - 1}}

) of the cell reaction per mole of

B

formed at

300K

is

\underline{\hspace{2cm}}

. (Given:

\ln \left( 2 \right) = 0.7,R

(universal gas constant)

= 8.3J\,{K^{ - 1}}\,mo{l^{ - 1}}.H,S

and

G

are enthalpy, entropy and Gibbs energy, respectively.)

Numerical answer

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