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Nernst Equation

The electroch...

Question

The electrochemical cell shown below is a concentration cell.
$M | M^{2 +}$ (saturated solution of a sparingly soluble salt, $M X_{2}$ ) $| | M^{2 +} (0.001 m o l d m^{- 3}) | M$
The emf of the cell depends on the difference in concentrations of $M^{2 +}$ ions at the two electrodes.
The emf of the cell at $298$ is $0.059 V$ .
The value of $Δ G$ ( kJ mol $^{- 1}$ ) for the given cell is:
[take 1F $= 96500$ C mol $^{- l}$ ]

- 5.7

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11.4

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- 11.4

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Solution

The correct option is D $- 11.4$
$At cathode : M^{+ 2} (a q) + 2 e^{-} \to M (s)$
$At anode : M (s) + 2 X^{-} (a q) \to M X_{2} (a q) + 2 e^{-}$
$n$ - factor of the cell reaction is $2$ .
$Δ G = - n F E_{c e l l} = - 2 \times 96500 \times 0.059 = - 11.4 k J m o l e^{- 1}$

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