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The electrochemical cell shown below is ...

The electrochemical cell shown below is 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 depends on the difference in concentration `M^(2+)` ions at the two electrodes. The emf of the cell at 298 K is `0.059" V"`
The value of `DeltaG (kJ" mol"^(-1)` for the given cell is `("take" 1 F =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
(d) `DeltaG =-nEF`
As `M-2e^(-) to M^(2+)`.
`DeltaG=-2xx0.059xx96500=-11.387 "joule"//"mol"`
`=-11.4" kJ"//"mol"`
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