A chemist designs a galvanic cell that uses these two half-reactions: half-reaction Br₂(1)+2e → 2 Br (aq) N₂(g) + 4H₂O()+4e N₂H₂(aq) +4 OH (aq) - Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode. Write a balanced equation for the half-reaction that happens at the anode. Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written. standard reduction potential E=+1.065 V red EO -1.16 V red
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction Br₂(1)+2e → 2 Br (aq) N₂(g) + 4H₂O()+4e N₂H₂(aq) +4 OH (aq) - Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode. Write a balanced equation for the half-reaction that happens at the anode. Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written. standard reduction potential E=+1.065 V red EO -1.16 V red
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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