Electric Cell
Definition and meaning of Electric Cell in chemistry.
Electric cell is a device that converts chemical energy directly into electrical energy through a spontaneous oxidation-reduction (redox) reaction. It consists of two electrodes, an anode and a cathode, in contact with an electrolyte, generating a flow of electrons through an external circuit.
In more detail
Inside the cell, oxidation occurs at the anode (releasing electrons) and reduction occurs at the cathode (accepting electrons), while ions move through the electrolyte to maintain charge balance and complete the internal circuit. The resulting potential difference between the electrodes is the cell's electromotive force (EMF), which drives current through any connected external circuit. Cells are classified as primary (non-rechargeable, discarded once the reactants are consumed) or secondary (rechargeable, since the reaction can be reversed by an external current). Two or more electric cells connected together form what is commonly called a battery.
Key facts
| Field | Physical Chemistry |
|---|---|
| Daniell cell EMF | ≈1.10 V (standard conditions) |
| Key parts | Anode, cathode, electrolyte, salt bridge |
| Main types | Primary (non-rechargeable) and secondary (rechargeable) |
The Daniell cell has a zinc electrode in zinc sulfate solution (anode) connected via a salt bridge to a copper electrode in copper sulfate solution (cathode); zinc oxidizes to Zn2+ while Cu2+ is reduced to copper metal, producing a standard EMF of about 1.10 V.
Frequently asked questions
What is the difference between an electric cell and a battery?
A single electric cell is one electrochemical unit; a battery is two or more cells connected in series or parallel to deliver a higher voltage or current.
Is an electric cell the same as an electrolytic cell?
No. An electric (galvanic) cell produces electrical energy from a spontaneous redox reaction, whereas an electrolytic cell consumes electrical energy to drive a non-spontaneous reaction.