Electrochemistry oxidation and reduction
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Electrochemistry - Oxidation and Reduction. Given the following reaction: Zn (s) + CuSO 4  ZnSO 4 + Cu. a) Identify the oxidation values for each element in the reaction. Zn (s) + CuSO 4  ZnSO 4 + Cu 0 +2 +6 -2 +2 +6 -2 0.

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Electrochemistry - Oxidation and Reduction

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Electrochemistry - Oxidation and Reduction

Given the following reaction: Zn (s) + CuSO4 ZnSO4 + Cu

a) Identify the oxidation values for each element in the reaction

Zn (s) + CuSO4 ZnSO4 + Cu

0 +2 +6 -2 +2 +6 -2 0

b) write the oxidation half-reaction and the reduction half-

reaction for the reaction

oxidation: Zn  Zn 2+ + 2 e -

reduction: Cu 2++ 2 e- Cu


Given the following reaction: Zn (s) + CuSO4  ZnSO4 + Cu

c) Identify the oxidizing agent and the reducing agent

Oxidizing agent = substance reduced = Cu2+

Reducing agent = substance oxidized = Zn


Electrochemical Cell Also called a Voltaic Cell or Galvanic Cell

Oxidizing and Reducing Agents are physically separated

so that electrons flow between the agents through an outside

conductor

The oxidizing and reduction agents must also be connected

by a salt bridge or semiporous barrier so that charged ions

can move between the agent in order to equilibrate overall

charge


Electrochemical Cell

Oxidizing and Reducing Agents are separated and electrons

flow between the agents through an outside conductor


Electrochemical Cell


Electrochemical Cell


Anode

a) Uusally written on the left side of a diagram;

b) Negative half cell - electrons formed in the anode and

flow from the anode left to right

c) Oxidation occurs in this half cell; contains the reducing

agent

Notes:

Anode and oxidation both

start with vowels

Electrons usually flow

from left to right

Anode related to anions

which have a neg charge


Cathode

a) Usually written on the right side of a diagram

b) Positive half cell; electrons move toward the cathode

c) Reduction occurs in this half cell; Contains the

oxidizing agent


Electrons flow from the anode to the cathode

The difference in potential energy between the anode and

cathode drives the electrons and is termed the electromotive

force or cell potential - measured in volts

volt = 1 J of work per charge


Electrons flow from the anode to the cathode.

The Cell Potential ( E cell ) for this example is 1.10 Volts.

Note that the value of the cell potential is positive.


At the anode, Zn is being oxidized to Zn 2+,

producing 2 electrons


At the cathode, Cu 2+ is being reduced to Cu,

gaining 2 electrons


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