Calculate E degree and indicate whether the overall reaction shown is spontaneou

Question

Calculate E degree and indicate whether the overall reaction shown is spontaneous or nonspontaneous. Co^3+ (aq) + e^- Co^2+(aq); E degree = 1.82 V MnO_4(aq) + 2H_2O(l) + 3e^- MnO_2(s) + 4OH^+ (aq); E degree = 0.59 V Overall reaction: MnO^-_4(aq) + 2H_2O(l) + 3Co^2+(aq) rightarrow MnO_2(s) + 3Co^3+(aq) - 4OH^+(aq) A) E_cell degree =-1.23 V, spontaneous B) E_cell degree = -1.23 V, nonspontaneous C) E_cell degree = 1.23 V, spontaneous D) E_cell degree = 1 .23 V, nonspontaneous E) E_cell degree = -0.05 V, nonspontaneous

Explanation / Answer

Eºcell = Eºcathode (reduction) - Eº anode( oxidation).
MnO4- (aq) + H2O (l) + 3Co2+ <--------> MnO2 (s) + 3Co3+ (aq) + 4OH- (aq)

Eºcell = 1.82 V - 0.59 V = 1.23 V

G = - n F Eocell

{ G > 0 than reaction will be non spontaneous and G < 0 than reaction will be spontaneous, n = number of electron transfer (3), f = faraday constant = 96500 }

G = - 3 x 96500 x 1.23

G = -356085 J/mol

so aver all reaction be spontaneous

option C is correct

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