An experimental fuel is a mixture of 83.30% ethanol and 16.70% gasoline by volume. Calculate how...
An experimental fuel is a mixture of 83.30% ethanol and 16.70% gasoline by volume. Calculate how much energy in the form of heat is available from 100 mL of this mixture and compare it with the amount from pure gasoline. Assume the densities of ethanol and gasoline are 0.789 and 0.737 g/mL, respectively, and that n-nonane is an appropriate model hydrocarbon for gasoline.
Heat from experimental fuel mixture
Heat from pure gasoline
Homework Answers
Dear student
heats of combustion of ethanol and nonane as 1360kJ/mole and 6125 kJ/mole, respectively.
fuel is a mixture of 83.30% ethanol and 16.70% gasoline by volume
heat released by fuel = volume x density / molar mass x ΔH
Ethanol: 83.30mL x [0.789g/mL] x [1mole/46g] x [1360kJ/mole] =
1943kJ
nonane: 16.70mL x [0.737g/mL] x [1mole/128g] x [6125kJ/mole =
589KJ
Total 2532 kJ / 100mL fuel.
compared with 100mL nonane
100mL x [0.737g/mL] x [1mole/128g] x [6125kJ/mole] = 3526kJ
The ethanol mix has 2532/3526x 100 = 71.8% of the energy of pure
nonane.
Regards
Team HomeworkLib
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Ln (relative rate) and 1/T in K^-1 is calculated by hand*
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