Electrochemical CellsMany oxidation

Electrochemical Cells
Many oxidation-reduction reactions occur spontaneously, giving off energy. An example involves the spontaneous reaction that occurs when zinc metal is placed in a solution of copper ions as described by the net ionic equation shown below.
Cu 2 (aq) Zn (s) -------> Cu(s) Zn 2 (aq)
The zinc metal slowly "dissolves" as its oxidation produces zinc ions which enter into solution. At the same time, the copper ions gain electrons and are converted into copper atoms which coats the zinc metal or sediments to the bottom of the container. The energy produced in this reaction is quickly dissipated as heat, but it can be made to do useful work by a device called, an electrochemical cell. This is done in the following way.
An electrochemical cell is composed to two compartments or half-cells, each composed of an electrode dipped in a solution of electrolyte. These half-cells are designed to contain the oxidation half-reaction and reduction half-reaction separately as shown below.

Electrochemical Cells
Many oxidation-reduction reactions occur spontaneously, giving off energy. An example involves the spontaneous reaction that occurs when zinc metal is placed in a solution of copper ions as described by the net ionic equation shown below.
Cu+2 (aq) + Zn (s) -------> Cu(s) + Zn+2 (aq)
The zinc metal slowly "dissolves" as its oxidation produces zinc ions which enter into solution. At the same time, the copper ions gain electrons and are converted into copper atoms which coats the zinc metal or sediments to the bottom of the container. The energy produced in this reaction is quickly dissipated as heat, but it can be made to do useful work by a device called, an electrochemical cell. This is done in the following way.
An electrochemical cell is composed to two compartments or half-cells, each composed of an electrode dipped in a solution of electrolyte. These half-cells are designed to contain the oxidation half-reaction and reduction half-reaction separately as shown below.

Electrochemical Cells
Many oxidation-reduction reactions occur spontaneously giving off, energy. An example involves the. Spontaneous reaction that occurs when zinc metal is placed in a solution of copper ions as described by the net ionic equation. Shown below.
Cu 2 (AQ) Zn (s) ------- > Cu (s) Zn 2 (AQ)
.The zinc metal slowly "dissolves" as its oxidation produces zinc ions which enter into solution. At the, same time the. Copper ions gain electrons and are converted into copper atoms which coats the zinc metal or sediments to the bottom of. The container. The energy produced in this reaction is quickly dissipated as heat but it, can be made to do useful work. By a, device calledAn electrochemical cell. This is done in the following way.
An electrochemical cell is composed to two compartments or. Half-cells each composed, of an electrode dipped in a solution of electrolyte. These half-cells are designed to contain. The oxidation half-reaction and reduction half-reaction separately as shown below.
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