ELECTROLYSIS OF WATER Meaning and
Definition
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Electrolysis of water refers to a chemical reaction that occurs when an electric current is passed through water, resulting in the decomposition of water molecules into their constituent elements: hydrogen and oxygen gas. This reaction takes place in an electrolytic cell, which consists of two electrodes placed in the water – a positively charged anode and a negatively charged cathode. The electrodes are typically made of inert materials such as platinum or graphite.
During the process, water molecules near the anode lose electrons and are oxidized to produce oxygen gas and positively charged hydrogen ions (protons). Simultaneously, water molecules near the cathode gain electrons and are reduced, resulting in the formation of hydrogen gas. The overall reaction of electrolysis of water can be represented by the equation: 2H2O(l) → 2H2(g) + O2(g).
Electrolysis of water is an important industrial process used to generate hydrogen gas, which has various applications such as fuel cell technology, chemical manufacturing, and as a potential alternative energy source. It also plays a vital role in the production of oxygen gas used in industrial processes and medical applications. Furthermore, electrolysis of water is an educational tool to demonstrate principles of electrochemistry, as electric current is used to drive a non-spontaneous chemical reaction.
