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Nernst Equation

At temperatur...

Question

At temperature of 298K, the emf of the following electrochemical cell will be:
$A g (s) | A g^{+} (0.1 M) | | Z n^{2 +} (0.1 M) | Z n (s)$
(Given, $E_{c e l l}^{o} = - 1.562 V$ )

- 1.532 V

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- 1.503 V

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1.532 V

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- 3.06 V

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Solution

The correct option is C $- 1.532 V$
From the given cell, the cell reaction is

$2 A g (s) + Z n^{2 +} (0.1 M) ⟶ 2 A g^{+} (0.1 M) + Z n (s)$

The Nerst equation is

$E_{c e l l} = E_{c e l l}^{o} - \frac{0.0591}{n} l o g \frac{[A g^{+}]^{2}}{[Z n^{2 +}]}$

or, $E_{c e l l} = (- 1.562) - \frac{(0.0591)}{2} l o g \frac{(0.1)^{2}}{(0.1)}$ (where, $E_{c e l l}^{o} = - 1.562 V$ )

or, $E_{c e l l} = (- 1.562) - \frac{0.0591}{2} l o g 10^{- 1}$

$= - 1.562 + \frac{0.0591}{2}$

$= - 1.562 + 0.02955$

$= - 1.532 V$

Suggest Corrections

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