8. The following redox reaction occurs at 25.0°C:5F22*(aq) + MnO4 (aq) + 8H*(aq) → Mn²*(aq) + 4H2O(1) + 5FE³*(aq)a.Calculate the E°cell for the redox reaction.Half ReactionE(V)MnO4 (aq) + 8H*(aq) + 5e¨ → Mn²*(aq) + 4H2O(1I)Fe3 (aq) + e → Fe2*(aq)+1.51+0.77b. Calculate the AG° in kJ/mol at 25.0°C.Calculate the AG when the following concentrations are used at 25.0°C.[Fe?*] = 0.200 M[MnO4] = 0.440M[H*] = 0.200 M[Mn2*] = 0.750 M[Fe3*] = 0.850 Mс.%3D%3D%3D

Answered: 8. The following redox reaction occurs…

Chemistry

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ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

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8. The following redox reaction occurs at 25.0°C:
5F22*(aq) + MnO4 (aq) + 8H*(aq) → Mn²*(aq) + 4H2O(1) + 5FE³*(aq)
a.
Calculate the E°cell for the redox reaction.
Half Reaction
E(V)
MnO4 (aq) + 8H*(aq) + 5e¨ → Mn²*(aq) + 4H2O(1I)
Fe3 (aq) + e → Fe2*(aq)
+1.51
+0.77
b. Calculate the AG° in kJ/mol at 25.0°C.
Calculate the AG when the following concentrations are used at 25.0°C.
[Fe?*] = 0.200 M
[MnO4] = 0.440M
[H*] = 0.200 M
[Mn2*] = 0.750 M
[Fe3*] = 0.850 M
с.
%3D
%3D
%3D

Expert Solution

Introduction

Electrochemistry is the branch of chemistry which studies the change of chemical energy into electrical energy during a chemical energy. Standard electrode potential is the potential of the individual electrode which can be determined experimentally. It is represented by. Its unit is Volt (V).

Given data

$E_{{MnO}_{4}^{2 -} / {Mn}^{2 +}}^{\circ} = + 1.51 V E_{{Fe}^{3 +} / {Fe}^{2 +}}^{\circ} = + 0.77 V$

Faraday’s constant, F = 96500 C mol^-1

No. of electrons, n = 5

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