Question

Please help! I’ll thank you :)

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)

Answer 1

The answer to your question is: 303g of CO2

Step-by-step 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