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Equilibrium Constant from Nernst Equation

The standard ...

Question

The standard electrode potential of ${Z n}^{2 +} | Z n$ is $- 0.76 V$ and that of ${C u}^{2 +} | C u$ is $0.34 V$ . The emf $(V)$ and the free energy change $(k J {m o l}^{- 1})$ , respectively, for a Daniel cell will be:

A

- 0.42

and

81

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B

1.1

and

- 213

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C

- 1.1

and

213

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D

0.42

and

- 81

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Solution

The correct option is B $1.1$ and $- 213$
$E_{C e l l}^{0} = E_{C u^{2 +} / C u}^{0} - E_{Z n^{2 +} / Z n}^{0} = 0.34 - (- 0.76) = 1.1 V$

$Δ G = - n F E_{C e l l}^{0} = - 2 \times 96500 \times 1.1 = - 212300 J / m o l \approx - 213 k J / m o l$

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