Question

What mass of carbon dioxide will be produced when 10.6 g of butane (C₄H₁₀) burns in an excess of oxygen forming CO₂ and H₂O?

a) 16.4 g
b) 22.8 g
c) 31.2 g
d) 42.7 g

Answer 1

The mass of carbon dioxide produced when 10.6 g of butane burns is approximately 186.08 g.

Step-by-step explanation:

First, we need to balance the chemical equation for the combustion of butane:

C4H10 + 13/2 O2 → 4 CO2 + 5 H2O

From the balanced equation, we can see that for every 1 mole of butane burned, 4 moles of CO2 are produced. Given that the molar mass of CO2 is 44 g/mol, we can calculate the mass of CO2 produced using the formula:

Mass of CO2 = Moles of CO2 × Molar mass of CO2

Mass of CO2 = (10.6 g C4H10) × (4 mol CO2 / 1 mol C4H10) × (44 g / mol CO2) = 186.08 g

Therefore, the mass of carbon dioxide produced when 10.6 g of butane burns is approximately 186.08 g.