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292. Calculate the equilibrium constant for the reaction at 298 K
$Cu (s) + {Cl}_{2} (g) ⇌ {CuCl}_{2} (aq)$
Given: $E °_{{Cu}^{2 +} / Cu} = 0.34 V; E °_{{Cl}^{2 +} / {Cl}^{-}} = 1.36 V, R = 8.314 J K^{- 1} {mol}^{- 1}$

R = 96500 C {mol}^{- 1} E °_{cell} = E °_{cathode} - E °_{anode} = 1.36 - 0.34 = 1.02 V

Equilibrium constant,

\log K_{C} = E °_{cell} \times \frac{nF}{2.303 RT}

\log K_{C} = \frac{1.02 \times 2 \times 96500}{2.303 \times 8.314 \times 298} = 34.57

K_{C} = Antilog (34.57) = 3.715 \times 10^{34}

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293. Calculate the equilibrium constant K_c for the reaction at 298 K.

3 {Sn}^{4 +} + 2 Cr ⇋ 3 {Sn}^{2 +} + 2 {Cr}^{3 +}

(Given E °_{{Sn}^{4 +} / {Sn}^{2 +}} = 0.15 V; E °_{{Cr}^{3 +} / Cr} = - 074 V) . = 0.34 V;

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294. Calculate the equilibrium constant for the cell reaction:

4 {Br}^{-} + O_{2} + 4 H^{+} \to 2 {Br}_{2} + 2 H_{2} O

(Given

E °_{cell} = 0.16

)

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Long Answer Type

295. Calculate the potential (emf.) of the cell
Cd | Cd²⁺ (0.10 M) || H⁺(0.20 M) | Pt, H₂ (0.5 atm)
(Given : E° _{Cd2+ / Cd} = – 0.403 V, R = 8.314 K^–1 K^–1 mol^–1, F = 96500 C mol^–1)

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Short Answer Type

296. Calculate ΔG° for the reaction

{Cu}^{2 +} (aq) + Fe (s) \to {Fe}^{2 +} (aq) + Cu (s) (Given E °_{{Cu}^{2 +} / Cu} = 0.34 V, E °_{{Fe}^{3 +} / Fe} = - 0.44 V, F = 96500 e {mol}^{- 1})

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297. The standard electrode potential for Daniell cell is 1.1 V. Calculate the standard Gibbs energy for the reaction:

Zn (s) + {Cu}^{2 +} (aq) \to {Zn}^{2 +} (aq) + Cu (s)

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298.

Calculate the Δ_r G° and the equilibrium constant for the reaction
2Cr(s) + 3Cd²⁺ (aq) 2Cr³⁺ (aq) + 3Cd(s)
(Given E°_Cr3+_/Cr = 0.74 V, E°_{Cd2+/ Cd} = – 0.40 V)

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299.

Calculate the cell e.m.f. and ΔG for the cell reaction at 298 K for the cell
Zn(s) | Zn²⁺ (0.0004 M) || Cd²⁺(0.2 M) | Cd(s)
(Given E°_Zn²⁺/Zn = 0.763 V, E°_{cd 2+ / cd} = 0.403 Vat 298 K, F = 96500 C mol^–1)

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300. Calculate the cell emf and AG for the cell rection at 25°C for the cell
Zn(s) | Zn²⁺ (0.0004 M) || Cd²⁺ (0.2 M) | Cd(s) E° values at 25°C, Zn²⁺/Zn = – 0.763 V, Cd²⁺/ Cd = – 0.403 V F = 96500 C mol^–1, R = 8.314 J K^–1 mol^–1

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