🔋 Simulation of Water Electrolysis
Observe the distribution of water into hydrogen and oxygen under the influence of an electric current.
🔬 Principle of Electrolysis
1. Ionization of Substances
When dissolved in water, an electrolyte (e.g., H₂SO₄) dissociates into ions. Water also partially dissociates into H⁺ and OH⁻ ions. These ions become carriers of charge in the solution.
2. Voltage Supply
When a constant voltage is applied between the electrodes, an electric field is created. Positive ions (cations) move towards the cathode, negative (anions) to the anode.
3. Electrochemical Reactions
At the cathode, reduction occurs: 2H⁺ + 2e⁻ → H₂ (hydrogen production). At the anode, oxidation takes place: 4OH⁻ - 4e⁻ → 2H₂O + O₂ (oxygen production).
4. Faraday's Law
The amount of substance released at the electrode is directly proportional to the amount of electricity that has passed through the solution. This allows for precise control of the process.
⚡ Application of Electrolysis
MINERAL OBTAINMENT
Electrolysis is used to obtain pure metals from their salts (aluminum, copper, zinc). This is one of the main methods of metallurgy and metal purification.
Daily energy production
Electrolysis of water - the primary method for producing hydrogen for fuel cells. Hydrogen can be used as an eco-friendly fuel for transportation and energy.
ELECTROPLATING
Electrolysis allows depositing thin metal layers on products' surfaces (chroming, nickel plating, zinc plating) for protection against corrosion and decorative purposes.
Waste Water Cleaning
Electrolytic methods are used for removing heavy metals and other pollutants from industrial effluents.
❓ FREQUENT QUESTIONS
Pure water has very low electrical conductivity because it only weakly dissociates into ions (H⁺ and OH⁻). To electrolyze it, you need to add an electrolyte (acid, base, or salt), which increases the ion concentration.
The theoretical voltage for water electrolysis is 1.23 V, but practically 1.5-2 V is needed due to electrode polarization and internal resistance of the solution. Higher voltage speeds up the process.
At the cathode (negative electrode), hydrogen ions (H⁺) are reduced to H₂. At the anode (positive electrode), hydroxide ions (OH⁻) are oxidized to O₂. This is defined by the electrochemical potentials of the reactions.
POLARIZATION IS THE CHANGE IN ELECTRODE POTENTIAL DURING ELECTROLYSIS AS A RESULT OF PRODUCT ACCUMULATION AT THE SURFACE. THIS INCREASES THE REQUIRED VOLTAGE AND CAN REDUCE PROCESS EFFICIENCY.
Electrolysis can be applied only to ionic compounds (salts, acids, bases) in solution or molten state. Covalent compounds (organic substances) do not electrolyze.