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What is the mass of CO2 produced when 100. g of butane, C4H10, is burned with excess oxygen,
according to the following chemical equation? (molar mass of C4H10 is 58.12 g/mol, molar mass of
CO2 is 44.01 g/mol)

2 C4H10 (g) + 13 O2 (g) → 8 CO2 (g) + 10 H20 (l)

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joseaaronlara

Answer:

The answer to your question is: 303g of CO2

Explanation:

Data

mass CO2 = ?

mass C4H10 = 100 g

MW C4H10 = 58.12 g

MW CO2 = 44.01 g

Solve this problem using rules of three

Reaction

                    2 C4H10 (g) + 13 O2 (g) → 8 CO2 (g) + 10 H20 (l)

                    2(58.12)      ------------------ 8(44.01)

                    100g          -------------------    x

mass of CO2 produced = x = (100)(8)(44.01) / (2)(58.12)

                                          x = 35208 / 116.24

                                          x = 302.9 g ≈ 303 g of CO2

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