Question

The electrode potential E(Zn²⁺ + Zn) E + of a zinc electrode at
25°C with an aqueous solution of 0.1 M ZnSO₄ is
[ E°(Zn²⁺ + Zn) = – 0.76 V. Assume 2.303RT/F = 0.06 at 298 K].
(a) + 0.73 (b) – 0.79
(c) – 0.82 (d) – 0.70

Answer 1

The electrode potential E(Zn²⁺ + Zn) E + of a zinc electrode at  25°C with an aqueous solution of 0.1 M ZnSO₄ is EZn2+ / Zn = −0.79 V

Option (B) is correct.

Explanation:

For  Zn2+  → Zn

EZn2+/Zn = E∘Zn2+ / Zn − 2.303 RT / nF log ([Zn])  / [Zn2+])

= − 0.76 − 0.06 / 2 log 1 / [(0.1]) = − 0.76 − 0.03

EZn2+ / Zn = −0.79 V

Thus the electrode potential E(Zn²⁺ + Zn) E + of a zinc electrode at  25°C with an aqueous solution of 0.1 M ZnSO₄ is EZn2+ / Zn = −0.79 V

Also learn more

The standard reduction potential of a silver|silver chloride|chloride ion electrode is 0.2 V and that of a silver electrode is 0.79 V. The maximum amount of AgCl that can dissolve in 106 L of a 0.1 M AgNO3 solution is  ?

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