How much H2 is generated from the electrolysis of 150 grams of H2O

Electrolysis is the decomposition of a chemical element under the effect of an electric current. So, electrolysis of water is the process of decomposing the H₂O molecule into separate oxygen and hydrogen gases due to an electric current passing through the water.

The balanced equation of electrolysis of water is:

2 H₂O → O₂ + 2H₂

Being:

H: 1 g/mole
O: 16 g/mole

then the molar mass of the compounds that participate in the reaction is:

H₂O: 2*1 g/mole + 16 g/mole= 18 g/mole
H₂: 2*1 g/mole= 2 g/mole
O₂: 2*16 g/mole= 32 g/mole

If the following amounts in moles are reacted by stoichiometry (that is, the relationship between the amount of reagents and products in a chemical reaction):

H₂O: 2 moles
H₂: 2 moles
O₂: 1 mole

the amount of mass, by stoichiometry, that reacts and is produced is:

H₂O: 2 moles*18 g/mole=36 g
H₂: 2 moles* 2 g/mole= 4 g
O₂: 1 mole* 32 g/mole= 32 g

Then you can apply the following rule of three: if by stoichiometry 36 g of H₂O generate 4 g of H₂, 150 g of H₂O how much mass of H₂ will it generate?

[tex]massofH_{2} =\frac{150 grams of H_{2}O*4 grams ofH_{2} }{36 grams of H_{2}O}[/tex]

mass of H₂= 16.67 grams

16.67 grams of H₂ is generated from the electrolysis of 150 grams of H₂O