The logarithm of the equilibrium constant of the cell reaction corresponding to the cell X(s)| X2+(a q) | Y+(a q)| Y(s) with standard cell potential, E text cell °=1.2 V is given by

Question

The logarithm of the equilibrium constant of the cell reaction corresponding to the cell X(s)| X2+(a q) | Y+(a q)| Y(s) with standard cell potential, E text cell °=1.2 V is given by (A) 12.5 (B) 21.5 (C) 40.5 (D) 47.2

Tardigrade Admin · Accepted Answer

<img class="img-fluid question-image" alt="image" src="https://cdn.tardigrade.in/img/question/chemistry/09966cd0bb63ed2ed9b78f5837da5bc2-.png" /> Thus, n=2 E text cell ° =(0.0591/n) log Kc 1.2 =(0.0591/2) log Kc log Kc =(1.2 × 2/0.0591) =40.6

Q. The logarithm of the equilibrium constant of the cell reaction corresponding to the cell $X (s) ∣ ∣ X^{2 +} (a q) ∥ Y^{+} (a q) ∣ ∣ Y (s)$ with standard cell potential, $E_{cell}^{\circ} = 1.2 V$ is given by

12.5

21.5

40.5

47.2

Thus, $n = 2$
$E_{cell}^{\circ} = \frac{0.0591}{n} lo g K_{c}$
$1.2 = \frac{0.0591}{2} lo g K_{c}$
$lo g K_{c} = \frac{1.2 \times 2}{0.0591}$
$= 40.6$

Q. The logarithm of the equilibrium constant of the cell reaction corresponding to the cell X(s)∣∣​X2+(aq)∥Y+(aq)∣∣​Y(s) with standard cell potential, Ecell ∘​=1.2V is given by