The charge in the cell is raised until a reaction is achieved Given the following half equations: Mg2+(aq) + 2e- → Mg(s) E0 = -2.36V K+(aq) + e- → K(s) E0 = -2.93V Br2(g) + 2e- → 2Br-(aq) E0 = +1.09V Cl2(g) + 2e- → 2Cl-(aq) E0 = +1.36V 2H+(aq) + 2e- → H2(g) E0 = 0v O2(g) + 4e- + 4H+→ 2H2O(l) E0 = +1.23V Given the Cell is in pH=0 Which reaction would occur in the Cathode? Which reaction would occur in the Anode? Write the full balanced reaction of the cell and the required charge for the reaction. The cell is run at 1A for 100 seconds, what is the amount of product in both anode and cathode?
The charge in the cell is raised until a reaction is achieved Given the following half equations: Mg2+(aq) + 2e- → Mg(s) E0 = -2.36V K+(aq) + e- → K(s) E0 = -2.93V Br2(g) + 2e- → 2Br-(aq) E0 = +1.09V Cl2(g) + 2e- → 2Cl-(aq) E0 = +1.36V 2H+(aq) + 2e- → H2(g) E0 = 0v O2(g) + 4e- + 4H+→ 2H2O(l) E0 = +1.23V Given the Cell is in pH=0 Which reaction would occur in the Cathode? Which reaction would occur in the Anode? Write the full balanced reaction of the cell and the required charge for the reaction. The cell is run at 1A for 100 seconds, what is the amount of product in both anode and cathode?
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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the following compounds are in solution in an electrolytic cell with two Pt electrodes: 1.0M KBr and 1.0M MgCl2
The charge in the cell is raised until a reaction is achieved
Given the following half equations:
Mg2+(aq) + 2e- → Mg(s) E0 = -2.36V
K+(aq) + e- → K(s) E0 = -2.93V
Br2(g) + 2e- → 2Br-(aq) E0 = +1.09V
Cl2(g) + 2e- → 2Cl-(aq) E0 = +1.36V
2H+(aq) + 2e- → H2(g) E0 = 0v
O2(g) + 4e- + 4H+→ 2H2O(l) E0 = +1.23V
Given the Cell is in pH=0
- Which reaction would occur in the Cathode?
- Which reaction would occur in the Anode?
- Write the full balanced reaction of the cell and the required charge for the reaction.
- The cell is run at 1A for 100 seconds, what is the amount of product in both anode and cathode?
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