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The electrochemical cell shown below is ...

The electrochemical cell shown below is a concentration cell.
`M|M^(2+)` (saturated solution of a sparingly soluble salt, `MX_2` || `M^(2+)` (0.001 mol `dm^(-3)`) |M
The emf of the cell depends on the difference in concentration of `M^(2+)` ions at the two electrode The emf of the cell at 298 is 0.059 V
The value of `DeltaG (kJ " mol"^(-1))` for the given cell is ( take` 1F = 96500 C " mol"^(-1)`)

A

`-5.7`

B

`5.7`

C

`11.4`

D

`-11.4`

Text Solution

Verified by Experts

The correct Answer is:
D
`DeltaG = -nFE = -2 xx 96.5 xx 0.059 = -11.41 `KJ/mole
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