What is Electrolysis?

Electrolytes are fused or aqueous solutions of substances that undergo chemical decomposition; electricity is passed through the fused state or aqueous solution of salts, bases and acids. Electrolytes are of two types:

• Strong electrolytes (which dissociate entirely into ions)
• Weak electrolytes (which do not ionise completely in an aqueous or molten state)

Electrodes

Electrodes are the materials that conduct electricity to or from the cell due to the movement of electrons. An electrode may be in the form of wire, rod or sheet.

Electrochemical Cell

In an electrochemical cell, chemical energy is converted into electrical energy. In this cell, chemical redox reactions are carried out, producing electricity. An electrochemical cell is also called a Voltaic or Galvanic cell. The most important example of an electrolytic cell is the Daniel cell.

Electrolysis

Electrolysis is defined as a process of breaking down ionic composites into their rudiments by passing electric current. The cations undergo reduction at the cathode, and anions undergo oxidation at the anode. The main factors needed for conducting electrolysis are an electrolyte, electrodes and some form of external power source. A partition similar to an ion-exchange membrane or a swab ground is also used, but this is voluntary. These are used substantially to keep the products from diffusing near the contrary electrode.

Electrolytic Process

In electrolysis, there’s an interchange of ions and atoms due to the addition or discarding of electrons from the external circuit. Principally, cations move to the cathode on passing a current, take electrons from the cathode (given by the force source battery), and are discharged into the neutral atom. If the neutral atom exists in solid form, it is deposited on the cathode, and if the neutral atom exists in solid form, it moves above. This is referred to as the reduction process, and the cation is reduced at the cathode electrode.

Cell Potential or Voltage

The electrolysis process’s minimal potential depends on the individual ions’ capability to absorb or release electrons. Also called decomposition potential or decomposition voltage, the minimal voltage (difference in electrode potential) between the anode and cathode of an electrolytic cell enables electrolysis.

Energy Changes during Electrolysis

In an electrolytic reaction, the electrical form of energy changes into a chemical form of energy. The potential difference to force the electrochemical process reaction to occur is the difference in potential between the two half-reactions at the two electrodes of the cell. But actually, the potential difference in which the electrolysis reaction takes place is much higher in value.

Factors Affecting Electrolysis

The rate of electrolysis is affected by several factors:

• Composition, chemical nature and state of the electrolyte
• Chemical nature and electrode potential of ions present in the electrolyte
• Nature of electrode considered
• Overvoltage at the electrodes

Examples of Electrolysis in Daily Life

• Estimation of the original weight of substances
• Metallurgy of alkali and alkaline earth metals and compounds
• Purification of metal ores
• Manufacture of gases in their purest state
• Manufacture of composites like sodium hydroxide, sodium carbonate, potassium chlorate, etc.
• Electroplating for making metals and objects resistant to corrosion, electroplating of ornaments, etc.

Conclusion

Electrolysis is the process of breaking down ionic composites into their rudiments by passing an electric current. The main factors needed for electrolysis are an electrolyte, electrodes and an external power source. In electrolysis, there’s an interchange of ions and atoms due to the addition or discarding of electrons from the external circuit.