The electrochemical cell shown below is a concentration cell.M|M2+ (Saturated solution of a sparingly soluble salt, MX2)||M2+(0.001 mol dm−3)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 0.059The value of ΔG(kJmol−1) for the given cell is: (take1F=96500 C mol−1)

The electrochemical cell shown below is a concentration cell.M|M2+ (Sa

1.	The electrochemical cell shown below is a concentration cell.M\|M2+ (Saturated solution of a sparingly soluble salt, MX2)\|\|M2+(0.001 mol dm−3)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 0.059The value of ΔG(kJmol−1) for the given cell is: (take1F=96500 C mol−1)
Answer» The electrochemical cell shown below is a concentration cell. $M \| M^{2 +}$ (Saturated solution of a sparingly soluble salt, $M X_{2}) \| \| M^{2 +} (0.001 m o l d m^{- 3}) M .$ The emf of the cell depends on the difference in concentration of $M^{2 +}$ ions at the two electrodes. The emf of the cell at 298K is 0.059 The value of $Δ G (k J m o l^{- 1})$ for the given cell is: (take $1 F = 96500 C m o l^{- 1})$