The combustion of butane produces heat according to the equation 2C₄H₁₀(g) + 13O₂(g) $\rarr$ 8CO₂(g) + 10H₂O(l) $\Delta$ H°_rxn= -5,314 kJ/mol
How many grams of CO₂ are produced per 1.00 *10⁴ kJ of heat released?

Question

The combustion of butane produces heat according to the equation 2C₄H₁₀(g) + 13O₂(g)

\rarr

8CO₂(g) + 10H₂O(l)

\Delta

H°_rxn= -5,314 kJ/mol
How many grams of CO₂ are produced per 1.00 *10⁴ kJ of heat released?

Quizplus · Accepted Answer

The reaction releases 5,314 kJ per 2 moles of butane, producing 8 moles of CO2. For 10,000 kJ, the moles of CO2 produced is (10,000 kJ / 5,314 kJ) * 8 moles. The molar mass of CO2 is 44.0 g/mol, so the mass is (10,000 / 5,314) * 8 * 44.0 g = 662 g.

The Combustion of Butane Produces Heat According to the Equation →\rarr→

The Combustion of Butane Produces Heat According to the Equation $\rarr$