$\mathrm{Cu(s)} + \mathrm{Sn^{2+}}$ (0.001M) $\rightarrow \mathrm{Cu^{2+}}$ (0.01M) + $\mathrm{Sn(s)}$ The Gibbs free energy change for the above reaction at 298 K is $x \times 10^{-1}$ kJ $\mathrm{mol^{-1}}$. The value of $x$ is ____. [nearest integer] [Given : $E^\ominus_{\mathrm{Cu^{2+}/Cu}}$ =0.34V ; $E^\ominus_{\mathrm{Sn^{2+}/Sn}}$ =−0.14V ; F=96500 C $\mathrm{mol^{-1}}$]

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JEE Main 26 June 2022, Shift 2, Chemistry Q87

Question 87 of 90 in this shift, Chemistry question 27 of 30, Section B.

\mathrm{Cu(s)} + \mathrm{Sn^{2+}}

(0.001M)

\rightarrow \mathrm{Cu^{2+}}

(0.01M) +

\mathrm{Sn(s)}

The Gibbs free energy change for the above reaction at 298 K is

x \times 10^{-1}

\mathrm{mol^{-1}}

. The value of

x

is ____. [nearest integer] [Given :

E^\ominus_{\mathrm{Cu^{2+}/Cu}}

=0.34V ;

E^\ominus_{\mathrm{Sn^{2+}/Sn}}

=−0.14V ; F=96500 C

\mathrm{mol^{-1}}

]

Official answer

983

NTA final key.