The equilibrium constant for the reaction $\mathrm{Zn(s)+Sn^{2+}(aq)}$ $\rightleftharpoons$ $\mathrm{Zn^{2+}(aq)+Sn(s)}$ is $1\times10^{20}$ at 298 K. The magnitude of standard electrode potential of $\mathrm{Sn/Sn^{2+}}$ if $\mathrm{E_{Z{n^{2 + }}/Zn}^\Theta = - 0.76~V}$ is __________ $\times 10^{-2}$ V. (Nearest integer) Given : $\mathrm{\frac{2.303RT}{F}=0.059~V}$

Question

The equilibrium constant for the reaction

$\mathrm{Zn(s)+Sn^{2+}(aq)}$ $\rightleftharpoons$ $\mathrm{Zn^{2+}(aq)+Sn(s)}$ is $1\times10^{20}$ at 298 K. The magnitude of standard electrode potential of $\mathrm{Sn/Sn^{2+}}$ if $\mathrm{E_{Z{n^{2 + }}/Zn}^\Theta = - 0.76~V}$ is __________ $\times 10^{-2}$ V. (Nearest integer)

Given : $\mathrm{\frac{2.303RT}{F}=0.059~V}$

Correct Answer

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