Complete combustion of butane ( C ₄ H ₁₀ ) yields carbon dioxide and water. The mass of CO ₂ (in g) produced upon the complete combustion of 116 ~g of butane is : [Given molar masses in g mol ⁻¹: C =12, H =1, O =16 ]

Step-by-step solution

The balanced chemical equation for the combustion of butane is: C ₄ H ₁₀ + 13 2 O ₂ 4 CO ₂ + 5 H ₂ O Molar mass of butane ( C ₄ H ₁₀ ) = 4 12 + 10 1 = 58 ~g mol ⁻¹ Moles of butane given = 116 58 = 2 ~mol From the stoichiometry of the balanced equation, 1 ~mol of butane produces 4 ~mol of CO ₂ . Therefore, 2 ~mol of butane will produce 2 4 = 8 ~mol of CO ₂ . Molar mass of CO ₂ = 12 + 2 16 = 44 ~g mol ⁻¹ Mass of CO ₂ produced = 8 44 = 352 ~g Answer: 352