Electrolytic cell - working, reaction i

An electrolytic cell is a type of cell that uses electricity to drive a non-spontaneous chemical reaction. Here's how it works, step by step:

1. Setup: An electrolytic cell consists of two electrodes (an anode and a cathode) connected to a power source. The electrodes are immersed in an electrolyte, a solution that contains ions.

2. Power Supply: When the power supply is turned on, it provides the energy needed to move electrons from the anode to the cathode, driving the chemical reaction.

3. Oxidation: At the anode, oxidation occurs. This means that electrons are lost from the chemical species at the anode. These electrons are then drawn up into the circuit.

4. Reduction: At the cathode, reduction occurs. This means that electrons are gained by the chemical species at the cathode. The electrons come from the circuit.

5. Ion Movement: The movement of ions in the electrolyte completes the circuit. Cations (positively charged ions) move towards the cathode and anions (negatively charged ions) move towards the anode.

6. Product Formation: The chemical reaction at each electrode often produces new substances. For example, if the electrolyte is a solution of copper sulfate, the reaction at the cathode will produce copper metal.

The overall reaction in an electrolytic cell is the sum of the oxidation and reduction reactions. For example, in the electrolysis of water, the overall reaction is:

2H2O(l) → 2H2(g) + O2(g)

This means that two molecules of water are broken down into two molecules of hydrogen gas and one molecule of oxygen gas.