Question

Gasoline is a mixture of compounds. A gasoline sample was found to be 2.851% (by mass) octane (C₈H₁₈). 482.6 g of gasoline is combusted to produce gaseous carbon dioxide and gaseous water.
Write out the balanced combustion reaction of octane with oxygen gas to form carbon dioxide and water. Submit an image of the balanced reaction.
Show all work.

Answer 1

Answer:

See below.

Explanation:

The mass of octane in the sample of gasoline is 0.02851 * 482.6 =  13.759 g of octane.

The balanced equation is:

2C8H18(l)  +  25O2(g) ---->  16CO2(g)  +   18H2O(g)

From the equation, using  atomic masses:

228.29 g of  octane forms 704 g of CO2 and 324.3 g of H2O

So the mass of CO2 formed from the combustion of 13.759 g of octane = (704 * 13.759) / 228.29

= 42.43 g of CO2.

Amount of water = 324.3 * 13.759) / 228.29

= 19.55 g of H2O.