The efficiency of a cell is $60$ %. Its cell reaction is:

$A (s) + B^{2 +} (a q .) \to A^{2 +} (a q .) + B; Δ H = - 240 k J$

The standard electrode potential of cell is:

0.746 V

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0.37 V

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1.48 V

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2.96 V

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Solution

The correct option is A $0.746 V$
Thermodynamic efficiency is given by the ratio of the Gibbs function change to the Enthalpy change in the overall cell reaction.

$η = \frac{Δ G}{Δ H} = \frac{60}{100}$
$∴ Δ G = - \frac{240 \times 10^{3} \times 60}{100}$ (as $Δ H = - 240 k J / m o l$ )
$Δ G = - n E^{o} F = - 144000$

(Note: As n factor is 2)

$E^{o} = \frac{144000}{2 \times 96500} = 0.746 V$

Option A is correct.

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The efficiency of a cell is 60 %. Its cell reaction is:A(s)+B2+(aq.)→A2+(aq.)+B; ΔH=−240 kJThe standard electrode potential of cell is:

The efficiency of a cell is $60$ %. Its cell reaction is:

$A (s) + B^{2 +} (a q .) \to A^{2 +} (a q .) + B; Δ H = - 240 k J$

The standard electrode potential of cell is: