Electrochemical Cell
An electrochemical cell is a device that converts chemical energy into electrical energy through spontaneous redox reactions. It consists of two half-cells connected by a conductive bridge.
Example: Daniel Cell (Zinc-Copper cell)
Cathode reaction: Cu2+(aq) + 2e⁻ → Cu(s)
Anode reaction: Zn(s) → Zn2+(aq) + 2e⁻
Some of other examples of electrochemical cell are dry cell and galvanic cell.
Dry cell
A dry cell is a common type of electrochemical cell used in batteries. It contains a paste electrolyte and is typically used in household applications.
Example: Leclanché Cell
Cathode reaction: 2MnO2(s) + 2NH4Cl(aq) + 2Zn(s) → Mn2O3(s) + 2NH4+(aq) + 2Zn2+(aq) + H2O(l)
Anode reaction: Zn(s) → Zn2+(aq) + 2e⁻
Galvanic cell
A galvanic cell is a type of electrochemical cell that generates electrical energy from spontaneous redox reactions. It consists of two different metal electrodes connected by a salt bridge or porous membrane.
Example: Voltaic Pile
Cathode reaction: Cu2+(aq) + 2e⁻ → Cu(s)
Anode reaction: Zn(s) → Zn2+(aq) + 2e⁻
Now, let’s understand chemistry behind various batteries that we see around ourselves
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.