
In Cu-Zn cell
(1) Reduction occurs at the copper cathode
(2) Oxidation occurs at the copper cathode
(3) Reduction occurs at the anode
(4) Chemical energy is converted to light energy
Answer
162.3k+ views
Hint: The electrochemical cell defines the cell that produces electricity from the chemical reaction. A dryer is an electrochemical cell or we can say a battery used mostly in the portable electronic device and equipment of houses. The copper zinc cell is an electrochemical cell.
Complete Step by Step Solution:
Let’s understand copper-zinc cell in detail. This cell can be prepared from zinc and copper metal with sulphate solution of each. That means, a zinc electrode is dipped in the solution of zinc sulphate and a copper electrode is dipped in the solution of copper sulphate and these two solutions (copper sulphate and zinc sulphate) are connected with the help of a salt bridge. And the two electrodes are connected by wires.
The oxidation reaction happens at the anode of zinc. Zinc lost two electrons and form cations and the reaction is,
\[{\rm{Zn}} \to {\rm{Z}}{{\rm{n}}^{2 + }} + 2{e^ - }\]
The reduction reaction happens at the cathode of copper. The copper ions take up electrons to form copper metal and get deposited. The chemical reaction is,
\[{\rm{C}}{{\rm{u}}^{{\rm{2 + }}}} + 2{e^ - } \to {\rm{Cu}}\]
Therefore, in the Cu-Zn cell, the reduction happens at the electrode of copper.
Hence, option A is right.
Note: There are many useful applications of Cu-Zn cells. They are used in the production of electricity or storage of electricity. They are used in the field of electrical telegraphy and battery development.
Complete Step by Step Solution:
Let’s understand copper-zinc cell in detail. This cell can be prepared from zinc and copper metal with sulphate solution of each. That means, a zinc electrode is dipped in the solution of zinc sulphate and a copper electrode is dipped in the solution of copper sulphate and these two solutions (copper sulphate and zinc sulphate) are connected with the help of a salt bridge. And the two electrodes are connected by wires.
The oxidation reaction happens at the anode of zinc. Zinc lost two electrons and form cations and the reaction is,
\[{\rm{Zn}} \to {\rm{Z}}{{\rm{n}}^{2 + }} + 2{e^ - }\]
The reduction reaction happens at the cathode of copper. The copper ions take up electrons to form copper metal and get deposited. The chemical reaction is,
\[{\rm{C}}{{\rm{u}}^{{\rm{2 + }}}} + 2{e^ - } \to {\rm{Cu}}\]
Therefore, in the Cu-Zn cell, the reduction happens at the electrode of copper.
Hence, option A is right.
Note: There are many useful applications of Cu-Zn cells. They are used in the production of electricity or storage of electricity. They are used in the field of electrical telegraphy and battery development.
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