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Combine the half-reactions shown into three different spontaneous redox reactions, calculating E°cell for each one and ranking the three reactions in order of increasing strength:   NO3–(aq) + 4 H+(aq) + 3e– --------à NO(g) + 2 H2O(l)                        E° = +0.96 V N2(g) + 5 H+ + 4e– ----------à N2H5+(aq)                                                    E° = –0.23 V   MnO2 + 4 H+(aq) + 2e– ---------à Mn2+(aq) + 2 H2O(l)                        E° = +1.23 V

Combine the half-reactions shown into three different spontaneous redox reactions, calculating E°cell for each one and ranking the three reactions in order of increasing strength:   NO3–(aq) + 4 H+(aq) + 3e– --------à NO(g) + 2 H2O(l)                        E° = +0.96 V N2(g) + 5 H+ + 4e– ----------à N2H5+(aq)                                                    E° = –0.23 V   MnO2 + 4 H+(aq) + 2e– ---------à Mn2+(aq) + 2 H2O(l)                        E° = +1.23 V

Chemistry by OpenStax (2015-05-04)
Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Chapter17: Electrochemistry
Section: Chapter Questions
Problem 24E: For each reaction listed, determine its standard cell potential at 25 C and whether the reaction is...
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  1. Combine the half-reactions shown into three different spontaneous redox reactions, calculating E°cell for each one and ranking the three reactions in order of increasing strength:

 

NO3–(aq) + 4 H+(aq) + 3e– --------à NO(g) + 2 H2O(l)                        E° = +0.96 V

N2(g) + 5 H+ + 4e– ----------à N2H5+(aq)                                                    E° = –0.23 V

 

MnO2 + 4 H+(aq) + 2e– ---------à Mn2+(aq) + 2 H2O(l)                        E° = +1.23 V

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