Concept explainers
Assume that a car burns pure octane.
C8H18 (d = 0.703 g/cm3)
(a) Write the balanced equation for burning octane in air. forming CO2 and H2O.
(b) If the car has a fuel efficiency of 32 miles per gallon of octane, what volume of CO2 at 25 °C and 1.0 atm is generated when the car goes on a 10.0-mile trip? (The volume of 1 mol CO2(g) at 25 °C and 1 atm is 24.5 L.)
(a)
Interpretation:
A balanced chemical equation for burning of octane has to be stated.
Concept Introduction:
The performance of an engine or fuel is measured in terms of octane number or octane rating. The processes that are used to increase the octane number of a fuel are known as catalytic cracking and catalytic reforming. Catalytic reforming converts the straight chain hydrocarbon into the branched hydrocarbon.
Answer to Problem 97QRT
A balanced chemical equation for burning of octane is shown below.
Explanation of Solution
The chemical reaction for combustion of octane is as follows.
In the above equation, the number of atoms on reactant and product side is not balanced. In order to balance them, a coefficient of
Therefore, the balanced chemical reaction for combustion of octane is shown below.
(b)
Interpretation:
The volume of
Concept Introduction:
Refer to part (a).
Answer to Problem 97QRT
The volume of
Explanation of Solution
The amount of fuel that is octane required to travel
The relation between gallon and liters is as follows.
Conversion of
The density of octane is
The relation between volume and mass is shown below.
Substitute the density and volume of octane in the above equation.
The molar mass of octane is
Substitute the mass and molar mass of octane in the above equation.
From the balanced chemical equation for combustion of octane, it is known that one mole of octane gives
Therefore, the number of moles of
The volume of
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