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.

By Now $4.49, New York’s next best seller!