JEE Advanced · 2012 · 08 Apr 2012 · Paper 2 · Redox Reactions and Electrochemistry

The electrochemical cell shown below is a concentration cell.

M ∣ M^{2 +}

(saturated solution of a sparingly soluble salt,

MX_{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 electrodes. 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}

)

(A)-5.7
(B)5.7
(C)11.4
(D)-11.4✓ Correct

Answer: (D)

Solution

For the cell reaction, n = 2 (two electrons transferred). Using ΔG = -nFE: ΔG = -2 × 96500 × 0.059 = -11387 J/mol ≈ -11.4 kJ/mol. The answer is (D).

JEE Advanced · 2012 · 08 Apr 2012 · Paper 2 · Single correct option

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