Since the question stated that the mileage is directly proportional to the heat of combustion of the fuel, we can make a direct comparison of the energy they produce per liter.
We don't have the ΔH°rxn for both combustion reactions of the 2 types of fuels so we have to compute that manually using ΔH°f values.
Ethanol, C2H5OH, is used as a fuel for motor vehicles, particularly in Brazil.
Assuming that an automobile’s mileage is directly proportional to the heat of combustion of the fuel, calculate how much farther an automobile could be expected to travel on 1 L of gasoline than on 1 L of ethanol. Assume that gasoline has the heat of combustion and the density of n–octane, C8H18 (ΔH°f = −208.4 kJ/mol; density = 0.7025 g/mL).
Frequently Asked Questions
What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Enthalpy of Formation concept. You can view video lessons to learn Enthalpy of Formation. Or if you need more Enthalpy of Formation practice, you can also practice Enthalpy of Formation practice problems.
What professor is this problem relevant for?
Based on our data, we think this problem is relevant for Professor Jackson's class at KU.
What textbook is this problem found in?
Our data indicates that this problem or a close variation was asked in Chemistry - OpenStax 2015th Edition. You can also practice Chemistry - OpenStax 2015th Edition practice problems.