(1) Compute the number of moles (n) of octane in 1 liter. The mass of that liter is 700 g, because of the 0.70 g/ml density.
(2) Using the balanced reaction for oxidation, calculate how many moles of O2 are needed to burn n moles of C8H18. That number is 12.5.
C8H18 + 12.5 O2 = 8CO2 + 9H2O
(3) The number of moles of air needed will be 12.5 n/0.22 = 56.8 n
(4) One mole of any gas occupies 24.2 liters at 20 C and 1 atm.
Put the pieces together for the final answer.
How many liters of air (78 percent N2, 22 percent O2 by volume) at 20 degrees Celsius and 1.00 atm are needed for the complete combustion of 1.0 L of octane, C8H18, a typical gasoline component that has a density of 0.70 g/mL?
4 answers
V = 4316 L
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