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Chemistry I

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Class 10 Class 12

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;

E °_{cell} = E °_{{Sn}^{4 +} / {Sn}^{2 +}} - E °_{{Sn}^{4 +} / {Sn}^{2 +}} - E °_{{Cr}^{3 +} / Cr} = 0.15 - (- 0.74) = 0.89 V

It is clear from the given equation that electrons involved in the reaction (n) = 6

\log K_{C} = \frac{E °_{cell} \times n}{0.059}

\log K_{C} = \frac{0.89 \times 6}{0.059} = 90.508

K_{C} = antilog 90.508

K_{C} = 3.221 \times 10^{90} .

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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

)

we have given that
E⁰ = 0.16

\log K_{C} = \frac{nE °_{cell}}{0.0591} E °_{cell} = 0.16 V, n = 4

\log K_{C} = \frac{(4) \times (0.16 V)}{(0.0591 V)} = 10.8 K_{C} = Antilog 10.8 = 6.31 \times 10^{10}

181 Views

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})

E °_{cell} = E °_{cathode} - E °_{anode} = E °_{{Cu}^{2 +} / Cu} - E °_{{Fe}^{3 +} / Fe} = 0.34 V - (- 0.44 V) = 0.78 V ∆_{r} G = - nFE ° = - 2 \times 96500 \times 0.78 (∵ n = 2) = - 150540 J = - 150.54 kJ

128 Views

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}

784 Views

∆_{r} G ° = - nFE ° n = 2 and F = 96500 C E °_{cell} = + 1.10

∆_{r} G ° = - 2 \times 96500 \times 1.10

∆_{r} G ° = - 212300 J

W_{\max} = - ∆_{r} G ° = 212300 J

1162 Views