Water

Water
Electrolysis is the process of decomposing water (H₂O) into hydrogen (H₂) and oxygen (O₂) gas by passing an electric current through it.
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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 not achievable in real-world conditions. Actual energy consumption and hydrogen yield will be lower due to energy losses as heat and other factors.

Would you like to explore the concept of efficiency in electrolysis or any other related topics?
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