Question

The combustion of hexyne, C₆H₁₀, is represented by the given equation: C6H10 + O₂ --> CO₂ + H₂O. If 376 grams of C₆H₁₀ is available and all C₆H₁₀ will be fully consumed, how many grams of CO₂ will be produced for complete combustion, assuming no excess O₂ is supplied? Write your final answer in two decimal places. Use the following mass numbers: C - 12 g/mol, H - 1 g/mol, O - 16 g/mol.

Answer 1

To find the mass of CO₂ produced during the combustion of hexyne, we can use stoichiometry and the molar mass of C₆H₁₀. Using the balanced equation, we can convert the mass of C₆H₁₀ to moles and then use the stoichiometric ratio to find the mass of CO₂ produced. Approximately 219.5 grams of CO₂ will be produced when 376 grams of C₆H₁₀ is completely burned.

Step-by-step explanation:

To determine the amount of CO₂ produced from the combustion of hexyne, we first need to find the molar mass of C₆H₁₀.

Molar mass of C₆H₁₀ = 6(12 g/mol) + 10(1 g/mol) = 82 g/mol

Next, we can use the balanced equation to set up a stoichiometric ratio:

1 mol C₆H₁₀ produces 1 mol CO₂

Using this ratio, we can convert the mass of C₆H₁₀ to moles and then use the stoichiometry to find the mass of CO₂ produced:

376 g C₆H₁₀ * (1 mol C₆H₁₀/82 g) * (1 mol CO₂/1 mol C₆H₁₀) * (44 g CO₂/1 mol CO₂) ≈ 219.5 g CO₂

Therefore, approximately 219.5 grams of CO₂ will be produced during the complete combustion of 376 grams of C₆H₁₀.