Question

1. The combustion of a sample of butane, C4H10 (lighter fluid), produced 2.46 grams of water.

2 C4H10 + 13 O2 -------> 8 CO2 + 10 H2O

(a) How many moles of water formed?

(b) How many moles of butane burned?

(c) How many grams of butane burned?

(d) How much oxygen was used up in moles? In grams?

Answer 1

(a) use the molar mass of water to turn grams into moles of H2O
(b) use the molar ratio from the balanced equation to turn moles of water (from a) into moles of butane burned
(c) use the molar mass of butane to turn moles of butane (from b) into grams of butane
(d) use the molar ratio to turn moles of butane into moles of O2, then use the molar mass of O2 to turn those moles of O2 into grams of O2