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2 CH3OH + 3 02 2 CO2 + 4H2O
What is the mass of oxygen (O2) that is required to produce 579 g of carbon dioxide (CO2)?
. Your answer should have three significant figures.

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Answer:

632 g

Explanation:

  • 2CH₃OH + 3O₂ → 2CO₂ + 4H₂O

First we convert 579 g of CO₂ into moles, using its molar mass:

  • 579 g CO₂ ÷ 44 g/mol = 13.16 mol CO₂

Then we convert CO₂ moles into O₂ moles, using the stoichiometric coefficients:

  • 13.16 mol CO₂ * [tex]\frac{3molO_2}{2molCO_2}[/tex] = 19.74 mol O₂

Finally we convert O₂ moles into grams, using its molar mass:

  • 19.74 mol O₂ * 32 g/mol = 632 g

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