Consider the redox reaction, 2A+3aq +2B−aq → 2A+2aq +B2aq; Ecell0 = 0.3V .. Standard Gibb’s energy Δ0G of the reaction will be

A+3+e− → A+2×2B− → 12B2+e− ×22A+3+2B− → 2A+2+B2n = 2ΔG0 = −nFE0 = −2965000.3J = −296.50.3kJ = −57.9kJ

Consider the redox reaction, 2A+3aq +2B−aq → 2A+2aq +B2aq; Ecell0 = 0.3V .. Standard Gibb’s energy Δ0G of the reaction will be

A+3+e− → A+2×2B− → 12B2+e− ×22A+3+2B− → 2A+2+B2n = 2ΔG0 = −nFE0 = −2965000.3J = −296.50.3kJ = −57.9kJ

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Consider the redox reaction, $2 {A^{+ 3}}_{(aq)} + 2 {B^{-}}_{(aq)} \to 2 {A^{+ 2}}_{(aq)} + B_{2 (aq)}; E_{cell}^{0} = 0 .3 V$ .. Standard Gibb’s energy $(Δ^{0} G)$ of the reaction will be

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-28.95 kJ/mole

-57.9 kJ/mole

+28.95kJ/mole

+57.9 kJ/mole

answer is B.

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Detailed Solution

$\begin{array}{l} [A^{+ 3} + e^{-} \to A^{+ 2}] \times 2 \\ [B^{-} \to \frac{1}{2} B_{2} + e^{-}] \times 2 \\ 2 A^{+ 3} + 2 B^{-} \to 2 A^{+ 2} + B_{2} \\ n = 2 \\ {ΔG}^{0} = - {nFE}^{0} \\ = - 2 (96500) (0 .3) J \\ = - 2 (96 .5) (0 .3) kJ \\ = - 57 .9 kJ \end{array}$