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

`:' DeltaG = -nFE`
`M - 2e^(-) rarr M^(2+)`
`:. n = 2`
`DeltaG = -2 xx 0.059 xx 96500 = -11,387 J "mol"^(-1)`
`= -11.4 kJ "mol"^(-1)`