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Electrochemistry

Question

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The emf (E°_cell) of the cell reaction : 3Sn⁴⁺ + 2Cr → 3Sn²⁺ + 2Cr³⁺ is 0.89 V. Calculate ΔG° for the reaction. (F = 96,500 (mol^–1 and VC ≡ J)

Solution

we have given the emf of the cell reaction :

3 {Sn}^{4 +} + 6 e^{-} \to 3 {Sn}^{2 +} At cathode 2 Cr \to 2 {Cr}^{3 +} + 6 e^{-} At anode n = 6, E °_{cell} = 0.89 V, F = 96500 C {mol}^{- 1}

ΔG = –nE°F
= – 6 x 0.89 V x 96500 C mol^–1= – 515310 J = – 515.310 kJ.

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