Given the following reduction half-reactions: Fe^3^+(aq) + e^- rightarrow Fe^2+(

Question

Given the following reduction half-reactions: Fe^3^+(aq) + e^- rightarrow Fe^2+(aq) E_red^degree = + 0.77 v S_2O_6^2-(aq) + 4H^+(aq) + 2e^- rightarrow 2H_2SO_3(aq) E_red^degree = +0.60 V N_2O(g) + 2H^+(aq) + 2H^+(aq) + 2e6- rightarrow N_2(g) + H_2O(t) E_red^degree = -1.77 V VO_2^+(aq) + 2H^+(aq) + e^- rightarrow VO^2+(aq) + H_2O(l) E_red^degree = +1.00 V Calculate the equilibrium constant K for this reaction at 298 K express your answer using one significant figure Write balanced chemical equation tor the oxidation of Fe^2+(aq) by N_2O (g) Express your answer as a chemical equation Identify all of the phases in your answer. Calculate delta G degree for this reaction at 298 K Express your answer using two significant figures. Calculate the equilibrium constant K for this reaction at 298 K Express your answer using one significant figure.

Explanation / Answer

Part D : balanced equation,

Fe2+(aq) + N2O(g) + 2H+(aq) ---> Fe3+(aq0 + N2(g) + H2O(l)

Part E : dGo,

dGo = -nFEo

Eo = Ecathode - Eanode = -1.77 - 0.77 = -2.54 V

dGo = -1 x 96485 x -2.54 = 245.072 kJ

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