Final answer:
Ethanol evaporates slower than acetone due to its stronger intermolecular forces.
Step-by-step explanation:
When comparing the rate of evaporation between ethanol and acetone, it is important to consider the intermolecular forces present in each substance. In ethanol, the molecules are capable of forming hydrogen bonds, which are relatively strong intermolecular attractions. On the other hand, acetone molecules cannot form hydrogen bonds.
Due to the presence of hydrogen bonding in ethanol, its overall intermolecular forces are stronger than those in acetone. As a result, fewer molecules of ethanol escape from the liquid at any given temperature, leading to a lower rate of evaporation than acetone.
Furthermore, ethanol has a higher boiling point than acetone, indicating that its molecules require more energy to break the intermolecular interactions and enter the gas phase. This suggests that acetone evaporates faster than ethanol at the same temperature.