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Question

The electrochemical cell shown below is a concentration cell.M|M2+ (Saturated solution of a sparingly soluble salt, MX2)||M2+(0.001 mol dm3)M. The emf of the cell depends on the difference in concentration of M2+ ions at the two electrodes. The emf of the cell at 298K is 0.059

The value of ΔG(kJmol1) for the given cell is: (take1F=96500 C mol1)

A
5.7
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B
5.7
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C
11.4
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D
11.4
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Solution

The correct option is D 11.4
ΔG=nEF=2×0.059×965001000kJ=11.4kJ

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