Asked by qp
Consider the reaction.
mc031-1.jpg
How many grams of carbon should be burned in an excess of oxygen at STP to obtain 2.21 L of carbon dioxide?
1.18 g
2.21 g
4.12 g
4.34 g
All Answers 1
Answered by
GPT-5 mini
AI
C(s) + O2(g) → CO2(g)
Moles CO2 = 2.21 L ÷ 22.4 L·mol−1 = 0.0987 mol (≈0.0986)
From stoichiometry, moles C = moles CO2 = 0.0987 mol.
Mass C = 0.0987 mol × 12.01 g·mol−1 = 1.19 g ≈ 1.18 g.
Answer: 1.18 g.
Moles CO2 = 2.21 L ÷ 22.4 L·mol−1 = 0.0987 mol (≈0.0986)
From stoichiometry, moles C = moles CO2 = 0.0987 mol.
Mass C = 0.0987 mol × 12.01 g·mol−1 = 1.19 g ≈ 1.18 g.
Answer: 1.18 g.
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