Electrochemical cell 2

Chemistry Level 2

The electrochemical cell shown below is a concentration cell.

M I M2+ (saturated solution of a sparingly soluble salt, $MX_2$ ) II M2+ (0.001 mol dm $^{-3}$ ) I M

The emf of the cell depends on the difference in concentrations of M $^{2+}$ ions at the two electrodes. The emf of the cell at 298 K is 0.059 V.

The value of $\delta G$ (kJ moI $^{-1}$ ) for the given cell is (take IF = 96500 C mo1 $^{-1}$ )

11.4 -5.7 5.7 -11.4

1 solution

Vikas Kumar
Feb 15, 2018

Since, ◇G = -nEF. ,
And it is given , E=0.059V , and the no of electrons transfer(n)= 2 and F =96500 C/mol So , ◇G = -2×0.059×96500 J/mol= -11,387 J/mol= - 11.3 kJ/mol

Electrochemical cell 2

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