Quantum EnergyBy Buddy Paul
Electrolysis is the process of decomposing water (H₂O) into hydrogen (H₂) and oxygen (O₂) gas by passing an electric current through it.
The overall reaction is: 2H₂O(l) → 2H₂(g) + O₂(g)
Energy Calculation
To determine the energy required to break down 1 mol of water, we need to consider the enthalpy of formation of water, which is the energy released when 1 mol of water is formed from its elements (hydrogen and oxygen). The enthalpy of formation of water is approximately -285.8 kJ/mol.
Since we want to reverse this process (breaking down water), the energy required will be the opposite sign: +285.8 kJ/mol.
Therefore, 285.8 kJ of energy is required to break down 1 mol of water with 100% efficient electrolysis.
Hydrogen Production
From the balanced equation, we can see that 2 moles of water produce 2 moles of hydrogen gas. 2H₂O(l) → 2H₂(g) + O₂(g)
So, 1 mol of water will produce 1 mol of hydrogen gas.
Therefore, you will get 1 mol of H₂ from the electrolysis of 1 mol of water.
Note: This calculation assumes 100% efficiency, which is possible with the Pulsar electrolizer.
Production from Electrolysis of Water
From the balanced equation: 2H₂O(l) → 2H₂(g) + O₂(g)
We can see that 2 moles of water produce 1 mole of oxygen gas.
Therefore, if we start with 1 mole of water, we will produce 0.5 moles of oxygen gas.
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