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:

$(R = 8 J K^{- 1} m o l^{- 1}, F = 96000 C m o l^{- 1})$

Question

TestHub · Accepted Answer

∆ 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

Chemistry - Electrochemistry Question with Solution | TestHub

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