If the standard electrode potential for a cell is 2 V at 300 K , the equilibrium constant K for the reaction. Z n s + C u 2 + a q ⇌ Z n 2 + a q + C u s at 300 K is approximately: R = 8 J K - 1 m o l - 1 , F = 96000 C m o l - 1

Step-by-step solution

∆ G = ∆ G o + R T l n Q At equilibrium ∆ G = 0 ,   Q = k 0 = ∆ G o + R T   l n K ∆ G o = - R T   l n K   ∴ ∆ G o = - n F E o So - n F E o = - R T   l n k ′ n ′ factor for the above cell = 2 So - 2 × 96000 × 2 = - 8 × 300   l n k l n k = 160 k = e 160