For the cell Al | Al^3+ (0.01 M) || Sn^2+ (0.1 M) | Sn at 298 K, E deg(Al^3+/Al) = -1.66 V and E deg(Sn^2+/Sn) = -0.14 V. The cell EMF in mV is (nearest integer; take 2.303RT/F = 0.0591 V).

JEE Main levelNumerical answerDifficulty 2 of 3ec081

For the cell $Al ∣ Al X^{3 +} (0.01 M) ∣∣ Sn X^{2 +} (0.1 M) ∣ Sn$ at 298 K, $E^{\circ} (Al X^{3 +} / Al) = - 1.66 V$ and $E^{\circ} (Sn X^{2 +} / Sn) = - 0.14 V$ . The cell EMF in mV is (nearest integer; take $2.303 RT / F = 0.0591 V$ ).

Numerical answer type, answer in mV, tolerance 1.

Cell reaction:

2 Al + 3 Sn X^{2 +} 2 Al X^{3 +} + 3 Sn

n = 6

E_{cell}^{\circ} = - 0.14 - (- 1.66) = 1.52 V

Q = \frac{[ Al X ^{3 +} ] ^{2}}{[ Sn X ^{2 +} ] ^{3}} = \frac{1 0 ^{- 4}}{1 0 ^{- 3}} = 0.1

E = 1.52 - \frac{0.0591}{6} lo g (0.1) = 1.52 + 0.00985 = 1.5299 V \approx 1530 mV