The equilibrium constant for the following reaction - Hg2- - Hg - Hg2-2 E-Hg - Hg2- - - 0-788 V- E-Hg2-2 - 2Hg2- - - 0-92 V is Keq - 2-98 - 10xThe value of x is -

Anode : Hg → Hg^2+ + 2e^ E^⊖_red = 0.788 V Cathode : 2Hg^⊕ + 2e^ → Hg^2+_2 E^⊖_(red) = 0.92 V At equilibrium, E^⊖_cell = ...

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Effective Equilibrium Constant

The equilibri...

Question

The equilibrium constant for the following reaction :

$H g^{2 +} + H g \to H g_{2}^{2 +}$

$E_{(H g | H g^{2 +})}^{⊖} = - 0.788 V; E_{(H g_{2}^{2 +} | 2 H g^{2 +})}^{⊖} = - 0.92 V$ is $K_{e q} = 2.98 \times 10^{x}$
The value of $x$ is ______.

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