Calculate E°cell and ∆rG° for the following reaction at 25°C.
A2+(aq) + B+(aq) → A3+(aq) + B(s)
[Given KC = 1010, 1F = 96500 C, R = 8.314 JK–1 mol–1]
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E°cell = 0.081 volts
∆rG° = -15633
Explanation:
The chemical reaction given in the question is:
A²⁺(aq) + B⁺(aq) → A³⁺(aq) + B(s)
The cell potential at equilibrium is given by the formula:
E°cell = (2.303 RT)/(nF) × log Kc
Where,
T = 273 K
R = 8.314 JK⁻¹mol⁻¹
n = 2
1F = 96500 C
Kc = 1010
On substituting the values, we get,
E°cell = (2.303 × 8.314 × 273)/(2 × 96500) × log (1010)
∴ E°cell = 0.081 volts
The ∆rG° is given by the formula:
∆rG° = -nFE°
On substituting the values, we get,
∆rG° = -(2 × 96500 × 0.081)
∴ ∆rG° = -15633
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