This problem is providing us with a reaction whereby hydrogen and oxygen react to produce water, so the mass of the product is required when 20.0 g of oxygen is consumed. At the end, the result turns out to be 22.5 g due to the following:
Stoichiometry:
In chemistry, we use stoichiometry as a tool to perform mole-mass relationships based on given balanced chemical equations. In such a way, since this problem provides 20.0 grams of oxygen and we need water, we can write the following stoichiometric setup:
[tex]20.0gO_2*\frac{1molO_2}{32.00gO_2} *\frac{2molH_2O}{1molO_2}*\frac{18.02gH_2O}{1molH_2O} \\\\[/tex]
Where 32.00 is the molar mass of diatomic oxygen, 2:1 is the mole ratio of water to oxygen and 18.02 is the molar mass of water. Hence, we obtain:
[tex]22.5g H_2O[/tex]
Learn more about stoichiometry: https://brainly.com/question/9743981
