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

665 g

Explanation:

Let's consider the following thermochemical equation.

2 C₄H₁₀ (g) + 13 O₂ (g) → 8 CO₂ (g) + 10 H₂O (l), ΔH°rxn = - 5,314 kJ/mol

According to this equation, 5,314 kJ are released per 8 moles of CO₂. The moles produced when 1.00 * 10⁴ kJ are released are:

-1.00 * 10⁴ kJ * (8 mol CO₂/-5,314 kJ) = 15.1 mol CO₂

The molar mass of CO₂ is 44.01 g/mol. The mass corresponding to 15.1 moles is:

15.1 mol * 44.01 g/mol = 665 g