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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 concentrations of `Mn^(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
`DeltaG=-nFE_(cell)=2xx96500xx0.059xx10^(-3)kJ//`mole
`=-11.4kJ//`mole.
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