The standard emf of a galvanic cell involving 3 moles of electrons in its redox reaction is 0.59 V. The equilibrium constant for the reaction of the cell is

Question

The standard emf of a galvanic cell involving 3 moles of electrons in its redox reaction is 0.59 V. The equilibrium constant for the reaction of the cell is (A) 1020 (B) 1025 (C) 1030 (D) 1015

Tardigrade Admin · Accepted Answer

E text cell ° =(0.0591/n) log Kc 0.59 =(0.0591/3) log Kc (0.59 × 3/0.059) = log Kc ∴ log Kc =30 Kc = antilog 30 =1030

Q. The standard emf of a galvanic cell involving $3$ moles of electrons in its redox reaction is $0.59 V$ . The equilibrium constant for the reaction of the cell is

$1 0^{20}$

$1 0^{25}$

$1 0^{30}$

$1 0^{15}$

$E_{cell}^{\circ} = \frac{0.0591}{n} lo g K_{c}$

$0.59 = \frac{0.0591}{3} lo g K_{c} \frac{0.59 \times 3}{0.059} = lo g K_{c}$

$∴ lo g K_{c} = 30$

$K_{c} =$ antilog $30$

$= 1 0^{30}$

Q. The standard emf of a galvanic cell involving 3 moles of electrons in its redox reaction is 0.59V. The equilibrium constant for the reaction of the cell is

1020

1025

1030

1015