Question

What are Galvanic cells? Explain the working of Galvanic cells with one example.

Answer 1

Galvanic cell $\to$ A galvanic cell is an electrochemical cell that converts the chemical energy of a spontaneous redox reaction into electrical energy.

Working of galvanic cell $\to$

It involves a chemical reaction that makes the electric energy available. During a redox reaction, a galvanic cell utilizes the energy transfer between electrons to convert chemical energy into electric energy.

In a Galvanic cell, the following reaction occurs-

${Zn}_{\left(s\right)}+{{Cu}^{2+}}_{(aq.)}⟶{{Zn}^{+2}}_{(aq.)}+{Cu}_{\left(s\right)}$

Galvanic cell utilizes the ability to separate the flow of electrons in the process of oxidization and reduction. This flow of electrons is essentially called a current. Such current can be made to flow through a wire to complete a circuit and obtain its output in any device such as a television or a watch.

A galvanic cell can be made out of any two metals. These two metals can form the anode and the cathode if left in contact with each other. This combination allows the galvanic corrosion of that metal which is more anodic. A connecting circuit shall be required to allow this corrosion to take place.

E.g.- In this cell, there is a container in which a solution of concentrated Copper Sulphate $\left(CuS{O}_4\right)$ is kept inside it and a copper rod is inserted inside the solution of $CuS{O}_4$ which act like cathode. Inside this, the container a porous container is kept in which concentrated Sulphuric Acid $\left(H_{2}S{O}_4\right)$ is filled in which a zinc rod is inserted in it which acts as an anode. Thus when a wire is connected through the copper rod and zinc rod an electric current starts to flow.