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Question

Chemistry Question on Equilibrium Constant

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){Zn(s) + cu^{2+} (aq) <=> Zn^{2+} (aq) + Cu(s)} at 300 K is approximately. (R=8  JK1  mol1,F=96000  C  mol1){(R = 8 \; JK^{-1} \; mol^{-1} , F = 96000 \; C \; mol^{-1})}

A

e160e^{160}

B

e320e^{320}

C

e160e^{ - 160}

D

e80e^{ - 80}

Answer

e160e^{160}

Explanation

Solution

ΔG=RT  lnk=  nFEcell{\Delta G^{\circ} = - RT \; lnk = - \; nFE^{\circ}_{cell}}
Ink=n×F×ER×T=2×96000×28×300{Ink = \frac{ n \times F \times E^{\circ}}{R \times T} = \frac{2 \times 96000 \times 2}{8 \times 300}}
Ink = 160
k=e160k = e^{160}