Using standard electrode potentials calculate ΔG∘ and use its value to estimate the equilibrium constant for...

Using standard electrode potentials calculate ΔG∘ and use its value to estimate the equilibrium constant for each of the reactions at 25 ∘C. Part A Cu2+(aq)+Zn(s)→Cu(s)+Zn2+(aq) USE ANY OF THESE VALUES Cu 2+ (aq) + e - ¡Cu^+ (aq) =0.16 e cell reduction Cu + (aq) + e - ¡ Cu(s) 0.52 ecell reduction potential Zn 2+ (aq) + 2 e - ¡ Zn(s) -0.76 cell reduction potential

Solutions

Expert Solution

Cu ^2+ (aq) + e - ----------->Cu^+ (aq) E0=0.16

Cu^+(aq) -+e^- ------------> Cu(s) E0 = 0.52

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Cu^2+ (aq) + 2e^- -----------> Cu(s) E0cell = 0.68v

Zn(s) --------------------> Zn^2+ (aq) + 2e^- E0 = 0.76v oxidation

Cu^2+ (aq) + 2e^- -----------> Cu(s) E0 = 0.68v reduction

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Zn(s) + Cu^2+ (aq) -----------> Zn^2+ (aq) + Cu(s) E0cell = 1.44v

n = 2

F = 96500c

G⁰ = -nE0cell *F

= -2*1.44*96500 = -277920J

G⁰ = -RTlnK

-277920 = -8.314*298*2.303logK

-277920 = -5705.84logK

logK = 277920/5705.84

logK = 48.7

K = 10^48.7 = 5*10^48

queen_honey_blossom answered 1 year ago

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