Lead Acid Batteries
In lead-acid batteries, the chemical reactions occur between lead dioxide (PbO2) at the positive electrode (cathode), lead (Pb) at the negative electrode (anode), and sulfuric acid (H2SO4) electrolyte. These reactions produce electrical energy that powers the battery.
Positive Electrode (Cathode) Reaction:
At the positive electrode (cathode), lead dioxide undergoes reduction and reacts with sulfate ions (SO42-) from the electrolyte to form lead sulfate (PbSO4) and water.
Cathode (Reduction): PbO2 + 4H+ + SO42−+ 2e−→PbSO4 + 2H2O
This reaction results in the conversion of lead dioxide to lead sulfate and the production of water.
Negative Electrode (Anode) Reaction:
At the negative electrode (anode), lead metal reacts with sulfate ions (SO42-) from the electrolyte to form lead sulfate (PbSO4) and release electrons.
Anode (Oxidation): Pb+SO42−→PbSO4 + 2e−
This reaction results in the conversion of lead metal to lead sulfate and the release of electrons.
Applications of Chemistry in Battery
A chemical cell, or a battery, is a device that converts chemical energy into electrical energy through electrochemical reactions. Some of the examples of these batteries are alkaline batteries, lithium ion batteries, lead acid batteries, etc. The functioning of these batteries are based on various chemical reactions. In this article, we will discuss the application of chemistry in batteries, i.e., how chemistry is involved in the functioning of these batteries.