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The value of Delta G (kJ mol| -1) for th...

The value of `Delta G (kJ mol| -1)` for the given cell is (take 1 F = 96500 `C mol^(-1)`)

A

`-5.7`

B

`5.7`

C

`11.4`

D

`-11.4`

Text Solution

Verified by Experts

The correct Answer is:
D
`Delta G = - n F E_(cell) = -2 xx 96500 xx 0.059 J mol^(-1)`
=`-11387 J mol^(-1)`
`= -11.38 kJ mol^(-1) = -11.4 k J mol^(-1)`
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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) )

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