Elektrolízise

Elektrolízise is a process that uses direct electric current to drive an otherwise non-spontaneous chemical reaction. In essence, it is the decomposition of a substance by passing an electric current through it. This is typically achieved by submerging two electrodes, an anode and a cathode, into an electrolyte, which is a substance containing free ions. When a voltage is applied, the ions migrate towards the electrode with the opposite charge. At the anode, oxidation occurs, meaning electrons are lost. At the cathode, reduction occurs, meaning electrons are gained.

Common applications of elektrolízise include the production of aluminum from bauxite ore, the refining of copper, and the production of chlorine gas and sodium hydroxide. The electrolytic cell, the apparatus used for elektrolízise, consists of the electrodes, the electrolyte, and a power source. The choice of electrolyte and electrode materials is crucial for the efficiency and outcome of the process. For instance, in the electrolysis of water to produce hydrogen and oxygen, an electrolyte like sulfuric acid or potassium hydroxide is added to increase conductivity, as pure water is a poor conductor of electricity. The overall reaction in the electrolysis of water is 2H₂O(l) → 2H₂(g) + O₂(g). Elektrolízise is a fundamental process in electrochemistry and plays a vital role in various industrial and scientific fields.