chemistry question thank you

Question

500.0 g of butane is burned in the presence of oxygen.

2C4H10(g) + 13O2(g) → 8CO2(g) + 10H2O(g)           ΔH = -1248 KJ

Answer 1

What's the question? Are you asking for the molar heat of combustion? Are you asking for the heat generated by combustion of 500.0 g of butane? Are you asking if the process is exo or endothermic? Are you asking how much heat is generated in the production of 100 moles of H2O?

I'll assume you are asking for the heat generated by combustion of 500.0 g of butane.

500 g C4H10 x 1 mol C4H10 / 58.12 g = 8.603 moles C4H10

8.603 mols C4H10 x -1248 kJ/2 mol C4H10 = -5368 kJ