Problem PageQuestion A major component of gasoline is octane. When octane is burned in air, it chemically reacts with oxygen gas to produce carbon dioxide and water. What mass of oxygen gas is consumed by the reaction of 6.1 g of octane

grams of oxygen = 21.40 g

Explanation:

octane → C8H18

The chemical reaction needs to be represented with a chemical equation before solving. The equation also need to be balanced.

C8H18 + O2 → CO2 + H2O

Balanced equation

2C8H18 + 25O2 → 16CO2 + 18H2O

Molar mass of octane = 12 * 8 + 18 = 96 + 18 = 114 g

Mass of octane in the chemical equation = 2 (114) = 228 g

molar mass of oxygen = 32 g

mass of oxygen in the chemical equation = 25 * 32 = 800 g

if 228 g of octane react with 800 g of oxygen

6.1 g of octane will require? grams of oxygen

cross multiply

grams of oxygen = 6.1 * 800/228

grams of oxygen = 4880 / 228

grams of oxygen = 21.4035087719

grams of oxygen = 21.40 g