The electrochemical cell shown below is a concentration cell. `M|M^(2+)(` saturated solution of sparingly soluble salt, `MX_(2))||M^(2+)(0.001 mol dm^(-3))|M`
The `emf` of the cell depends on the difference in the concentration of `M^(2+)` ions at the two electrodes. The `emf` of the cell at `298` is `0.059V`.
The solubility product `(K_(sp),mol^(3) dm^(-9))` of `MX_(2)` at 298 based on the information available the given concentration cell is `(` Take `2.303xxRxx298//F=0.059V)`

Options

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

Answer

D

Explanation

`:' DeltaG =- nFE`
`DeltaG =- 2 xx 96500 xx 0.059` Joule
`=- 11.4` kJ/mole