Final answer:
By using molar masses and a stoichiometric calculation, we would expect more than 45 grams of water to be produced when 100 grams of silicon dioxide completely react with HF, according to the balanced chemical equation. The available answer choices do not match the calculated result.
Step-by-step explanation:
Given the balanced chemical equation SiO₂ + 4HF → SiF₄ + 2H₂O, we need to calculate how many grams of H₂O (water) are produced from 100 grams of SiO₂ (silicon dioxide).
First, we calculate the molar mass of SiO₂, which is 28.09 (Si) + 32.00 (O₂) = 60.09 g/mol. The molar mass of H₂O is 18.02 g/mol. Applying stoichiometry, we find that for every 60.09 grams of SiO₂, 2 moles of H₂O are produced. Therefore, we can set up a conversion factor from the mass of SiO₂ to the mass of H₂O:
(100 g SiO₂) x (1 mol SiO₂ / 60.09 g SiO₂) x (2 mol H₂O / 1 mol SiO₂) x (18.02 g H₂O / 1 mol H₂O) = 60.01 g H₂O
However, none of the answer choices match this calculation. It is likely that there is either a mistake in the provided choices or a misinterpretation of the question. The closest answer based on the given options would be 'd) 45 g', assuming possible rounding during calculation steps.
The correct answer is that more than 45 grams of water will be produced.