Question

Cars run on gasoline, where octane (C8H18) is the principle component. This combustion reaction is responsible for generating enough energy to move a vehicle, or do other work. How much CO2 and H2O (in grams) are produced in the combustion of 1.19 gallons of Octane? (density = 0.703 g/mL

Mass of Carbon Dioxide Formed
g

Mass of Water Formed
g

Answer 1

To calculate the mass of CO2 and H2O produced from 1.19 gallons of Octane, the volume is first converted to grams. Using the balanced equation for the combustion of Octane, the masses of CO2 and H2O produced are calculated through stoichiometry: 22,223.28 grams of CO2 and 17,932.26 grams of H2O are formed.

Step-by-step explanation:

To calculate the mass of CO2 and H2O produced in the combustion of 1.19 gallons of Octane, we first convert the volume of Octane to grams using the provided density (0.703 g/mL). The complete combustion of octane follows the reaction:

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

Knowing the density and the volume of Octane, we find the mass of Octane to be 3146.27 grams (1.19 gallons * 3.78541 Liters/gallon * 1000 mL/Liter * 0.703 g/mL).

Using stoichiometry, we can relate the molar mass of Octane (114.23 g/mol) to the molar masses of CO2 (44.01 g/mol) and H2O (18.015 g/mol). For every 2 moles of Octane that react, 16 moles of CO2 and 18 moles of H2O are produced. This results in the production of 22,223.28 grams of CO2 and 17,932.26 grams H2O.