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Q.

The standard cell potential involving the reaction ${Cl}_{2} (g) + 2 {Br}^{-} (aq) \to {Br}_{2} (l) + 2 {Cl}^{-} (aq)$
$Δ_{r} G^{\circ} = - 50.61 kJ {mol}^{- 1}$ is

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a

- 0.524 V

b

0.524 V

c

0.262 V

d

-0.262 V

answer is C.

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Detailed Solution

$Δ_{r} G^{\circ} = - n F E_{cell}^{\circ}; E_{cell}^{\circ} = - Δ_{r} G^{\circ} / n F; E_{cell}^{\circ} = + (50.61 \times 10^{3} J {mol}^{- 1}) / (2) (96500 C) = + 0.262 V$

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The standard cell potential involving the reaction Cl2(g)+2Br−(aq)→Br2(l)+2Cl−(aq)ΔrG∘=−50.61 kJ mol−1 is