The Δ G° for the Daniell cell has been found to be -212.3 kJ at 25° C. Calculate the equilibrium constant for the cell reaction.

Question

The Δ G° for the Daniell cell has been found to be -212.3 kJ at 25° C. Calculate the equilibrium constant for the cell reaction. (A)  11.64× 1030  (B)  1.64× 1037  (C)  0.1064× 1035  (D)  21.64× 1039

Tardigrade Admin · Accepted Answer

Δ G°=-R T ln Kc -212300 J=-(8.314 J K-1 mol -1)(298 K) ln Kc=(212300/8.314 × 293)=85.69 Kc=1.64 × 1037

Q. The $Δ G^{\circ}$ for the Daniell cell has been found to be $- 212.3 k J$ at $2 5^{\circ} C$ . Calculate the equilibrium constant for the cell reaction.

$11.64 \times 10^{30}$

$1.64 \times 10^{37}$

$0.1064 \times 10^{35}$

$21.64 \times 10^{39}$

$Δ G^{\circ} = - RT ln K_{c}$
$- 212300 J = - (8.314 J K^{- 1} m o l^{- 1}) (298 K)$
$ln K_{c} = \frac{212300}{8.314 \times 293} = 85.69$
$K_{c} = 1.64 \times 1 0^{37}$

Q. The ΔG∘ for the Daniell cell has been found to be −212.3kJ at 25∘C. Calculate the equilibrium constant for the cell reaction.

11.64×1030

1.64×1037

0.1064×1035

21.64×1039