Firstly, an electrolysis cell is prepared, typically consisting of two electrodes and an electrolyte solution. The electrodes are usually made of inert metals such as platinum. The electrolyte solution can be pure water or a water solution containing electrolytes like alkaline or acidic solutions.

 A direct current (DC) is applied to the two electrodes of the electrolysis cell. The cathode is connected to the negative terminal, while the anode is connected to the positive terminal of the power supply. The electric current flows through the electrolyte solution between the electrodes.

As the electric current passes through the electrolyte solution, water molecules undergo oxidation-reduction reactions at the cathode and anode. At the cathode, water molecules accept electrons and undergo reduction, producing hydrogen gas (H2): 2H2O + 2e- -> H2 + 2OH-

At the anode, water molecules lose electrons and undergo oxidation, generating oxygen gas (O2):

4OH- -> 2H2O + O2 + 4e-

It can be observed that during the electrolysis process, hydrogen gas is released at the cathode, while oxygen gas is released at the anode.

Electrolytic hydrogen production involves the electrolysis of water by applying an electric current through an electrolyte solution, resulting in the separation of hydrogen and oxygen gases. This process is based on Faraday's law and utilizes the oxidation-reduction reactions occurring in the electrolyte solution. Electrolytic hydrogen production is widely used in various fields such as hydrogen energy production, storage, and utilization.