Final answer:
From 63.5 g of H2O, 56.416 grams of O2 can be produced by using the stoichiometry of the chemical reaction 2H2(g) + O2(g) -> 2H2O(g) and converting moles of H2O to moles of O2, and then to grams.
Step-by-step explanation:
The question asks how many grams of O2 can be produced from 63.5 g of H2O. To solve this, you can use the stoichiometry of the balanced chemical equation for the decomposition of water:
2H2(g) + O2(g) -> 2H2O(g)
Firstly, calculate the number of moles of H2O using the molar mass of water (18.02 g/mol):
- 63.5 g H2O / 18.02 g/mol = 3.526 mol H2O
According to the balanced equation, 2 moles of H2O produce 1 mole of O2. So, the moles of O2 produced from 3.526 mol H2O are:
- 3.526 mol H2O × (1 mol O2 / 2 mol H2O) = 1.763 mol O2
Finally, convert the moles of O2 to grams using the molar mass of O2 (32.0 g/mol):
- 1.763 mol O2 × 32.0 g/mol = 56.416 g O2
So, 56.416 grams of O2 can be produced from 63.5 g of H2O.