The electrochemical cell shown below is a concentration cell.M/M2+(saturated solution of a sparingly soluble salt MX2∥M2+0.00001moldm−3/MThe emf of the cell depends on the difference in concentration of M2+ ions at the two electrodes. The emf of the cell at 298 is 0.059 V.The value of ΔGkJ mol−1 for the given cell is (take 1F=96500 C mol−1)

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-5.7

5.7

11.4

-11.4

answer is D.

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Detailed Solution

ΔG=−nEF=−2×0.059×965001000kJ=−11.4kJ

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