Final answer:
To determine the grams of water produced in the given reaction, divide the given mass of oxygen by its molar mass to find the moles of O₂ used. Use the ratio from the balanced equation to calculate the moles of H₂O produced. Finally, convert the moles of water to grams using its molar mass.
Step-by-step explanation:
To determine the grams of water produced in the given reaction, we first need to find the amount of oxygen used. From the balanced equation, we can see that for every 7 moles of O₂ used, 6 moles of H₂O are produced. We can calculate the moles of O₂ used by dividing the given mass of oxygen (955.291 grams) by its molar mass (32.0 grams/mole):
Moles of O₂ = 955.291 g / 32.0 g/mol = 29.85 moles
Now, we can use the ratio from the balanced equation to calculate the moles of water produced:
Moles of H₂O = (6/7) * 29.85 moles ≈ 25.53 moles
Finally, we can convert the moles of water to grams using its molar mass (18.02 grams/mole):
Grams of H₂O = 25.53 moles * 18.02 g/mol ≈ 459.98 grams
Therefore, approximately 459.98 grams of water will be made.