Question

Determine the values of equilibrium constant (K_C) and ∆G° for the following reaction:

Ni(s) + 2Ag⁺(aq) → Ni²⁺(aq) + 2Ag(s), E° = 1.05 V

(1 F = 96500 C mol^–1)

Answer 1

(i) Calculate of ΔG^∘ for the reaction

\(Ni(s) + 2Ag^+(aq) \to Ni^{2 + }(aq) + 2Ag(s)\)

\(\Delta G° = - nFE^\circ_{cell}\)

\(= (-2) \times (96500 \,C \,mol^{-1}) \times (1.05V)\)

\(= -202650 \,CV \,mol^{-1}\)

\(= -202650 \,J\, mol^{-1}\)

\(= -202.65\,kJ\, mol^{-1}\)

(ii) Calculate of equilibrium constant (K_c) for the reaction

\(E°= \frac{2.303 RT}{nF}\log K_c\)

\(= \frac{0.0591}{n} \log K_c\)

\(\log K_c = \frac{n \times E°}{0.0591 V}\)

\(= \frac{2 \times (1.05V)}{(0.0591 V)}\)

\(= 35.53\)

K_c = Antilog 35.53

= 3.41 × 10³⁵

Answer 2

The values of equilibrium constant (K_C) and ∆G°