If the standard electrode potential for a cell is 2 V at 300 K, the equilibrium constant (K) for the reaction Zn(s) + cu2+ (aq) Zn2+ (aq) + Cu(s) at 300 K is approximately. (R = 8 JK-1 mol-1 , F = 96000 C mol-1)

Question

If the standard electrode potential for a cell is 2 V at 300 K, the equilibrium constant (K) for the reaction Zn(s) + cu2+ (aq) <=> Zn2+ (aq) + Cu(s) at 300 K is approximately. (R = 8 JK-1 mol-1 , F = 96000 C mol-1) (A) e160 (B) e320 (C) e - 160 (D) e - 80

Tardigrade Admin · Accepted Answer

Δ G° = - RT lnk = - nFE°cell Ink = ( n × F × E°/R × T) = (2 × 96000 × 2/8 × 300) Ink = 160 k = e160

Q. If the standard electrode potential for a cell is 2 V at 300 K, the equilibrium constant (K) for the reaction
$Zn (s) + cu X^{2 +} (aq) Zn X^{2 +} (aq) + Cu (s)$ at 300 K is approximately.
$(R = 8 JK X^{- 1} mol X^{- 1}, F = 96000 C mol X^{- 1})$

$e^{160}$

$e^{320}$

$e^{- 160}$

$e^{- 80}$

$ΔG X^{\circ} = - RT lnk = - n FE X_{cell}^{\circ}$
$Ink = \frac{n \times F \times E X ^{\circ}}{R \times T} = \frac{2 \times 96000 \times 2}{8 \times 300}$
Ink = 160
$k = e^{160}$

Q. If the standard electrode potential for a cell is 2 V at 300 K, the equilibrium constant (K) for the reaction Zn(s)+cuX2+(aq)​ZnX2+(aq)+Cu(s) at 300 K is approximately. (R=8 JKX−1 molX−1,F=96000 C molX−1)

e160

e320

e−160

e−80