The value of the equilibrium constant for the given reaction at 25°C is 5.67 x 10³⁵.
For the given reaction
Oxidation : Ni -------------> Ni+2 + 2e-
Reduction : 2 Ag+ + 2e- ------------> 2 Ag
E₀cell = E₀red - E₀oxida
= 0.80 - (- 0.257)
= 1.057 V
Δ G₀ = - n F E₀cell
= - 2 x 96485 x 1.057 x 10^-3
= - 203.97 kJ/mol
Δ G₀ = - R T ln K
- 203.97 = - 8.314 x 10⁻³x 298 x ln Keq
Keq = 5.67 x 10³⁵
Therefore, the equilibrium constant = 5.67 x 10³⁵
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