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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+)(0.001mol dm^(-3))|M`
The emf of the cell depends on the difference in concentration of `M^(2+)` ions at the electrodes. The emf of the cell at `298K` is `0.059V`
The solubility product `(K_(sp), mol^(3) dm^(-9))` of `MX_(2)` at `298K` based on the information available for the given concentration cell is (take `2.303 xx R xx 298//F = 0.059V)`

A

`-5.7`

B

`5.7`

C

`11.4`

D

`-11.4`

Text Solution

Verified by Experts

The correct Answer is:
D
`:' DeltaG =- nFE`
`DeltaG =- 2 xx 96500 xx 0.059` Joule
`=- 11.4` kJ/mole
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