Calculate the ΔrG° and log Kc for the following cell reaction : Fe (s) + Ag⁺ (aq) ⇌ Fe²⁺(aq) + Ag (s) Given : E°(Fe²⁺/Fe) = – 0·44 V, E°(Ag⁺/Ag) = + 0·80 V, 1 F = 96500 C mol⁻¹

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TextNernst Equation for Cell PotentialFaraday's Second Law of ElectrolysisCBSE PYQ

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Calculate the e.m.f. of the following cell at 298K : Fe(s) | Fe²⁺ (0.001 M) || H⁺ (0.01M) | H₂(g) (1 bar) | Pt(s) Given that E°cell = +0.44 V [log 2 = 0.3010 log 3 = 0.4771 log 10 = 1]

TextEMF of a Cell and Its CalculationNernst Equation for Cell Potential

Calculate the emf of the following cell at 25°C: Zn (s) | Zn²⁺ (0.1 M) || H⁺ (0.01 M) | H₂ (g) (1 bar), Pt (s) [Given: E°(Zn²⁺/Zn) = – 0.76 V, E°(H⁺/H₂) = 0.00 V, log 10 = 1]

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