The electrochemical cell shown below is a concentration cell. $M ∣ M^{2 +}$ (saturated solution of a sparingly soluble salt, $M X_{2}) ∣ ∣ ∣ M^{2 +} (0.001 mol dm^{- 3}) ∣ ∣ M$
The emf of the cell depends on the difference in concentrations of $M^{2 +}$ ions at the two electodes. The emf of the cell at 298 K is 0.059 V.

The value of $Δ G (kJ mol^{- 1})$ for the given cell is (take $1 F = 96500 C mol^{- 1})$

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Michael Discussed

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 mol dm^{- 3}) ∣ ∣ M

The emf of the cell depends on the difference in concentrations of

M^{2 +}

ions at the two electodes. The emf of the cell at 298 K is 0.059 V.

The value of

Δ G (kJ mol^{- 1})

for the given cell is (take

1 F = 96500 C mol^{- 1})

5 mins ago

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