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

At anode: `M(s) +2X_((aq))^(-) rarr MX_(2(aq)) +2e^(-)`
At cathode: `M_((aq))^(+2) +2e^(-) rarr M(S)`
n-factor for the cell reaction is 2.
`DeltaG =- nFE_(cell) =- 2 xx 96500 xx 0.059`
`=- 113873 J//"mole"`
`=- 11.387 KJ//"mole" =- 11.4 KJ//"mole"`