Consider the following electrochemical cell (battery): Mg(s) │ Mg2+(aq) ║ Cl- (aq) │ Cl2 (g) │ Pt(s) all gases 1 atm, all solutions 1.0 M 1. Write the respective reduction half-reactions occurring on each side of the salt bridg, and from some reference, get the half-cell potential (in volts) for each. 2. Determine what reaction occurs overall, and calculate the Eocell for this electrochemical cell. 3. Make a drawing of this cell, and label the ANODE and the CATHODE. Show what direction the electrons flow in the external circuit.
Consider the following electrochemical cell (battery): Mg(s) │ Mg2+(aq) ║ Cl- (aq) │ Cl2 (g) │ Pt(s) all gases 1 atm, all solutions 1.0 M 1. Write the respective reduction half-reactions occurring on each side of the salt bridg, and from some reference, get the half-cell potential (in volts) for each. 2. Determine what reaction occurs overall, and calculate the Eocell for this electrochemical cell. 3. Make a drawing of this cell, and label the ANODE and the CATHODE. Show what direction the electrons flow in the external circuit.
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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Consider the following
Mg(s) │ Mg2+(aq) ║ Cl- (aq) │ Cl2 (g) │ Pt(s) all gases 1 atm, all solutions 1.0 M
1. Write the respective reduction half-reactions occurring on each side of the salt bridg, and from some reference, get the half-cell potential (in volts) for each.
2. Determine what reaction occurs overall, and calculate the Eocell for this electrochemical cell.
3. Make a drawing of this cell, and label the ANODE and the CATHODE. Show what direction the electrons flow in the external circuit.
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