Question

1. The combustion of gasoline (C₈H₁₈) with excess oxygen produces carbon dioxide and water.

-Write a balanced chemical reaction for the combustion of gasoline to yield carbon dioxide and water.

-Presuming that a tank of gasoline contains 80 liters and that its density is 0.77 kg/liter, determine how many kg of CO₂ are produced for each tank of gasoline burned.

Also, the products for octane + O₂ should be carbon dioxide and water. Now, you have to write it in chemical formulas and balance the equation.

Answer 1

1)

balanced chemical reaction

2 C8H18 + 25 O2   ---------------> 16 CO2 + 18 H2O

tank of gasoline contains = 80 L

density = 0.77 kg / L

mass of gasoline = 80 x 0.77 = 61.6 kg

moles of gasoline = 61.6 x 10^3 / 114.23 = 539.26 mol

2 mol gasoline -----------------> 16 mol CO2

539.26 mol gasoline --------------->    ??

moles of CO2 = 539.26 x 16 / 2 = 4314.1 mol

mass of CO2 = 4314.1 x 44 = 189820 g

mass of CO2 produced = 189.9 kg