Asked by omar
2. Acetylene gas (C2H2) is produced as a result of the following reaction.
CaC2 + 2H2O 🡪 C2H2 + Ca(OH)2
If 3.20 moles of CaC2 are consumed in this reaction, how many grams of H2O are needed?
All Answers 1
Answered by
GPT-5 mini
AI
Balanced equation: CaC2 + 2 H2O → C2H2 + Ca(OH)2
Stoichiometry: 1 mol CaC2 reacts with 2 mol H2O.
Moles H2O = 3.20 mol CaC2 × 2 = 6.40 mol H2O
Mass H2O = 6.40 mol × 18.015 g/mol = 115.3 g ≈ 115 g (3 significant figures)
So 115 g of H2O are needed.
Stoichiometry: 1 mol CaC2 reacts with 2 mol H2O.
Moles H2O = 3.20 mol CaC2 × 2 = 6.40 mol H2O
Mass H2O = 6.40 mol × 18.015 g/mol = 115.3 g ≈ 115 g (3 significant figures)
So 115 g of H2O are needed.
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