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)`)

Options

A. `-5.7`
B. `5.7`
C. `11.4`
D. `-11.4`

Answer

D

Explanation

`becauseDeltaG=-2EF,M-2e^(-)rarrM^(2+),thereforen=2`
`DeltaG=-2xx0.059xx96500=-11,387"J mol"^(-1)`
`=-11,4:kJ mol"^(-1)`