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The standard electrode potentials for the reduction of N2 to N2H4 and of O2 to H2O at 298 K are –1.155 V and +0.401 V, respectively, both under alkaline conditions. (i) Write a balanced equation for both of the half cell reactions under alkaline conditions. For the cell reaction where the hydrazine electrode is on the left, calculate the standard EMF of the cell at 298 K. (ii) In a practical cell the concentrations of N2H4 and OH- are 0.5 M and 1.0 M, respectively, and the pressure of O2 and N2 are 0.2 bar and 0.8 bar, respectively. Use the Nernst equation to estimate the cell EMF at 298 K, assuming all activity coefficients are unity.

The standard electrode potentials for the reduction of N2 to N2H4 and of O2 to H2O at 298 K are –1.155 V and +0.401 V, respectively, both under alkaline conditions. (i) Write a balanced equation for both of the half cell reactions under alkaline conditions. For the cell reaction where the hydrazine electrode is on the left, calculate the standard EMF of the cell at 298 K. (ii) In a practical cell the concentrations of N2H4 and OH- are 0.5 M and 1.0 M, respectively, and the pressure of O2 and N2 are 0.2 bar and 0.8 bar, respectively. Use the Nernst equation to estimate the cell EMF at 298 K, assuming all activity coefficients are unity.

Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter19: Principles Of Chemical Reactivity: Electron Transfer Reactions
Section19.9: Corrosion: Redox Reactions In The Environment
Problem 2.5ACP: Assume the following electrochemical cell simulates the galvanic cell formed by copper and zinc in...
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8. In a fuel cell, hydrazine, N2H4, is oxidized to nitrogen, and oxygen is reduced to water. The standard electrode potentials for the reduction of N2 to N2H4 and of O2 to H2O at 298 K are –1.155 V and +0.401 V, respectively, both under alkaline conditions. (i) Write a balanced equation for both of the half cell reactions under alkaline conditions. For the cell reaction where the hydrazine electrode is on the left, calculate the standard EMF of the cell at 298 K. (ii) In a practical cell the concentrations of N2H4 and OH- are 0.5 M and 1.0 M, respectively, and the pressure of O2 and N2 are 0.2 bar and 0.8 bar, respectively. Use the Nernst equation to estimate the cell EMF at 298 K, assuming all activity coefficients are unity.
Transcribed Image Text:8. In a fuel cell, hydrazine, N2H4, is oxidized to nitrogen, and oxygen is reduced to water. The standard electrode potentials for the reduction of N2 to N2H4 and of O2 to H2O at 298 K are –1.155 V and +0.401 V, respectively, both under alkaline conditions. (i) Write a balanced equation for both of the half cell reactions under alkaline conditions. For the cell reaction where the hydrazine electrode is on the left, calculate the standard EMF of the cell at 298 K. (ii) In a practical cell the concentrations of N2H4 and OH- are 0.5 M and 1.0 M, respectively, and the pressure of O2 and N2 are 0.2 bar and 0.8 bar, respectively. Use the Nernst equation to estimate the cell EMF at 298 K, assuming all activity coefficients are unity.
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