ElectrochemistryHard
Question
The theoretical efficiency of a hypothetical cell is about 84% which involves the following reaction
A(s) + B2+ (aq) → A2+ (aq) + B(s); ΔH = −285 kJ, then, the standard EMF of the cell is
Options
A.1.10 V
B.1.24 V
C.2.48 V
D.2.20 V
Solution
Theoretical efficiency = $\frac{- \Delta G^{o}}{- H^{o}} \Rightarrow 0.84 = \frac{- \Delta G^{o}}{285}$
$\therefore\Delta G^{o} = - 0.84 \times 285\text{ KJ = } - nF.E_{cell}^{o} $$$\text{Or, 0.84} \times \text{285} \times \text{1}\text{0}^{3} = 2 \times 96500 \times E_{cell}^{o} \Rightarrow E_{cell}^{o} = 1.24\text{ V}$$
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