Question

What is the theoretical yield of oxygen when 29.2 g of water are decomposed by electrolysis according to the balanced equation: 2H2O yields 2H2 + O2

Answer 1

Taking into account the reaction stoichiometry, the theoretical yield of oxygen when 29.2 g of water are decomposed by electrolysis is 25.956 grams.

Reaction stoichiometry

In first place, the balanced reaction is:

2 H₂O → 2 H₂ + O₂

By reaction stoichiometry (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of moles of each compound participate in the reaction:

• H₂O: 2 moles
• H₂: 2 moles
• O₂: 1 mole

The molar mass of the compounds is:

• H₂O: 18 g/mole
• H₂: 2 g/mole
• O₂: 32 g/mole

Then, by reaction stoichiometry, the following mass quantities of each compound participate in the reaction:

• H₂O: 2 moles ×18 g/mole= 36 grams
• H₂: 2 moles ×2 g/mole= 4 grams
• O₂: 1 mole ×32 g/mole= 32 grams

Definition of theorical yield

The theoretical yield is the amount of product acquired through the complete conversion of all reagents in the final product, that is, it is the maximum amount of product that could be formed from the given amounts of reagents.

Theorical yield of O₂

The following rule of three can be applied: if by reaction stoichiometry 36 grams of water form 32 grams of oxygen, 29.2 grams of water form how much mass of oxygen?

$mass of oxygen=\frac{29.2 grams of waterx32 grams of oxygen}{36 grams of water}$

mass of oxygen= 25.956 grams

Finally, the theoretical yield of oxygen when 29.2 g of water are decomposed by electrolysis is 25.956 grams.

Learn more about the reaction stoichiometry:

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