Chapter 10, Problem 16CI

Ethanol, ${\text{C}}_{\text{2}}{\text{H}}_{\text{6}}\text{O}$ , is obtained from renewable crops such as corn, which use the Sun as their source of energy. In the United States, automobiles can now use a fuel known as E85 that contains 85.0% ethanol and 15.0% gasoline by volume. Ethanol has a melting point of -115 °C, a boiling point of 78 °C, a heat of fusion of 109 J/g, and a heat of vaporization of 841 J/g. Liquid ethanol has a density of 0.796 g/mL and a specific heat of 2.46 J/g °C. (8.3, 8.5, 9.2, 9.3, 10.4, 10.5)
a. Draw a heating curve for ethanol from $\text{-150 °C to 100 °C}\text{.}$
b. When 20.0 g of ethanol at -62 °C is heated and completely vaporized at 78 °C, how much energy, in kilojoules, is required?
c. If a 15.0-gal gas tank is filled with E85, how many liters of ethanol are in the gas tank?
d. Write the balanced chemical equation for the complete combustion of ethanol.
e. How many kilograms of ${\text{ CO}}_{\text{2}}$ are produced by the complete combustion of the ethanol in a full 15.0-gal gas tank?
f. What would be the strongest intermolecular force between liquid ethanol molecules?