Electrochemistry (Oxidation/Reduction)
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Transcript of Electrochemistry (Oxidation/Reduction)
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Electrochemistry (Oxidation/Reduction)
CHEM 2124 – General Chemistry II
Alfred State College
Professor Bensley
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Learning Objectives Define oxidation-reduction reaction. Learn the oxidation number rules and assign
oxidation numbers. Write the half-reactions of an oxidation-
reduction reaction. Determine the species undergoing oxidation
and reduction. Describe and construct basic galvanic cells Calculate cell potential for basic galvanic cells
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Oxidation and Reduction
I. General Features
II. Oxidation Numbers
Assign oxidation numbers to Carbon in each of the following compounds:Assign oxidation numbers to Carbon in each of the following compounds:
1. Carbon Monoxide1. Carbon Monoxide 2. Carbon Dioxide2. Carbon Dioxide
3. C3. C66HH1212OO6 6 (Glucose)(Glucose) 4. Sodium Bicarbonate4. Sodium Bicarbonate
For each of the following chemical reactions, determine whether or not the reaction is an example of an oxidation-reduction reaction.
LiOH + HCN H2O + LiCN
LiCl + AgNO3 AgCl + LiNO3
P4 (s) + 5O2 (g) P4O10 (s)
CuCl2 (aq) + Al (s) AlCl3 (aq) + Cu (s)
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Oxidation and Reduction
III. Half Reactions
What happens when copper wire is placed What happens when copper wire is placed in a silver nitrate solution? in a silver nitrate solution?
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For each of the following Redox reactions, write the individual half-reactions.1. Fe (s) + CuSO4 (aq) Cu (s) + FeSO4 (aq)
2. Co (s) + Cl2 (g) CoCl2 (g)
In each of the following reactions, identify the oxidizing agent and the reducing agent.
1. Co (s) + Cl2 (g) CoCl2 (g)
2. 2Al (s) + 3F2 (g) 2AlF3 (s)
3. PbS (s) + 4H2O2 (aq) PbSO4 (aq) + 4H2O (l)
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Oxidation and Reduction
1. Combination Reactions
2. Decomposition Reactions
3. Displacement Reactions
4. Combustion Reactions
IV. Examples of Oxidation–Reduction Reactions
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Oxidation and ReductionOxidation and Reduction
V. Galvanic or voltaic cells
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AnodeZn (s) Zn 2+ (aq) + 2e-
CathodeCu 2+ (aq) + 2e- Cu (s)
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Oxidation and Reduction
VI. Galvanic Cell TerminologyA. Half cellsB. AnodeC. CathodeD. Salt BridgeE. Cell NotationF. Cell Potential
E0 (cell) = E0 (red) – E0 (ox)
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Order the following oxidizing agents from weakest to strongest.
Cu2+ (aq), Fe2+ (aq), Fe3+ (aq)
Order the following reducing agents from weakest to strongest.
H2 (g), Al (s), Cu (s)
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Example
• Sketch the cell formed by Cd in Cd(NO3)2 and Ag in AgNO3.
• Write the half-reactions, label the anode, cathode, salt bridge, and direction of electron flow.
• Write the cell notation.
• Calculate the overall cell potential for this cell.
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VII. Biological Applications
• Respiration– Oxidation of glucose to CO2
– Reduction of O2 to H2O
C6H12O6 (s) + 6O2 (g) 6CO2 (g) + 6H2O (g)
• Photosynthesis– Oxidation of H2O to O2
– Reduction of CO2 to glucose– 6CO2 (g) + 6H2O (g) + light C6H12O6 + 6O2 (g)
Oxidation and Reduction