Calculate the emf and ΔG for the given cell at 25°C: Cr(s)/Cr3+(0.1M) // Fe2+(0.01M)/Fe(s) Given: E°Cr3+/Cr = -0.74V, E°Fe2+/Fe = -0.44V (1F = 96500 C, R = 8.314 JK-1 mol-1)

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TextEMF of a Galvanic CellNernst Equation for Electrode and Cell PotentialRelation Between Gibbs Energy and EMF of Cell

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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 Galvanic CellNernst Equation for Electrode and 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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