1. Write the balanced chemical equation:

2 H₂ + O₂ → 2 H₂O

This equation tells us that 2 moles of hydrogen (H₂) react with 1 mole of oxygen (O₂) to produce 2 moles of water (H₂O).

2. Determine the limiting reactant:

We need to know how much oxygen is present to determine the limiting reactant. The limiting reactant is the substance that gets used up first and limits the amount of product formed. Since the amount of oxygen isn't given, we can't determine the limiting reactant.

3. Calculate moles of water produced (assuming excess oxygen):

* Assume excess oxygen: If there is an excess of oxygen, the amount of hydrogen will limit the amount of water produced.

* Convert grams of hydrogen to moles: You'll need to look up the molar mass of hydrogen (H₂) which is approximately 2 g/mol.

* moles of H₂ = (45.3 g H₂) / (2 g/mol H₂) = 22.65 moles H₂

* Use the mole ratio from the balanced equation:

* The equation shows 2 moles of H₂ producing 2 moles of H₂O. This means the mole ratio is 1:1.

* Calculate moles of water:

* moles of H₂O = 22.65 moles H₂ * (2 moles H₂O / 2 moles H₂) = 22.65 moles H₂O

Conclusion:

If there is an excess of oxygen, 45.3 grams of hydrogen will produce 22.65 moles of water.

Important Note: If you have a specific amount of oxygen, you'll need to use that information to calculate the limiting reactant and determine the actual amount of water produced.