The value of the equilibrium constant (K) at 25°C is 1.059 × 10.
For the given reaction;
2Ag(s) +Mn²⁺(aq) ⇄ 2Ag⁺(aq) + Mn(s)
Ag⁺(aq) + e⁻ → Ag(s) E° = +0.80V
Mn²⁺(aq) +2e⁻ → Mn(s) E° = -1.18V
E°cell = -1.18V - 0.08V = -1.98V
ΔG° = -nFE°cell
ΔG° = -Rt㏑K
or, -Rt㏑K = -nFE°cell
㏑K = nFE°cell/RT
㏑K = 2 × 96485 × (-1.98) / 8.314 ×298
㏑K = -154.216
or, K = e⁻¹⁵⁴°²¹⁶ = 1.059 × 10
K = 1.059 × 10
Therefore, the value of the equilibrium constant is 1.059 × 10.
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