Question

Which of the following affects the vapor pressure of a liquid? (a) Volume of the liquid, \((\mathbf{b})\) surface area, \((\mathbf{c})\) intermolecular attractive forces, \((\mathbf{d})\) temperature, \((\mathbf{e})\) density of the liquid.

Short answer

Vapor pressure is affected by intermolecular forces and temperature.

Step-by-step solution

Understanding Vapor Pressure

Vapor pressure is the pressure exerted by the vapor of a liquid when it is in equilibrium with its liquid phase. It is highly dependent on the kinetic energy of the molecules, as only molecules with sufficient kinetic energy can escape into the vapor phase.

Effect of Intermolecular Forces

Intermolecular attractive forces directly impact vapor pressure. Strong intermolecular forces mean molecules are held more tightly and it is harder for them to escape into the vapor phase, leading to lower vapor pressure. Therefore, intermolecular forces affect vapor pressure.

Impact of Temperature

Temperature affects the kinetic energy of molecules. An increase in temperature means an increase in kinetic energy, allowing more molecules to escape into the vapor phase. Thus, vapor pressure increases with temperature.

Analyzing Other Factors

The volume of the liquid, surface area, and density do not affect the inherent vapor pressure. Vapor pressure is a property at equilibrium, primarily determined by temperature and intermolecular forces, not by the amount or configuration of the liquid.

Conclusion

Given the analysis, vapor pressure is affected by (c) intermolecular attractive forces and (d) temperature due to their direct relation to the ability of molecules to escape into the vapor phase.

Key concepts

Intermolecular Forces

Intermolecular forces play a crucial role in determining the vapor pressure of a liquid. These are the forces of attraction between molecules, and they can vary greatly depending on the nature of the liquid. For instance, liquids with strong hydrogen bonds, like water, exhibit significant intermolecular forces.

When intermolecular forces are strong, the molecules in a liquid are held tightly together. This makes it more challenging for molecules to escape from the liquid phase to the vapor phase. As a result, liquids with stronger intermolecular forces possess lower vapor pressures at a given temperature. On the other hand, liquids with weaker intermolecular forces, such as ether, have molecules that can escape more readily, resulting in higher vapor pressure.

Some common types of intermolecular forces include:

• Dispersion forces (also known as London forces)
• Dipole-dipole interactions
• Hydrogen bonds

Understanding these forces helps in predicting and explaining the behavior of different liquids in relation to their vapor pressures.

Temperature Effects

Temperature has a profound impact on the vapor pressure of a liquid. As the temperature increases, the kinetic energy of the molecules also rises. This increment in kinetic energy means that a greater number of molecules now possess enough energy to overcome intermolecular forces and escape into the vapor phase.

Increasing the temperature of a liquid will always result in an increase in vapor pressure. This happens because:

• Higher temperatures lead to more energetic collisions among molecules.
• More molecules reach the necessary energy threshold to transition into the vapor phase.

A useful practical understanding of this is noticing how liquids evaporate faster on a hot day compared to a cold one. This illustrates the concept that the higher the temperature, the higher the vapor pressure, as more molecules are moving rapidly and escaping from the surface of the liquid.

Kinetic Energy of Molecules

Kinetic energy is a fundamental concept when discussing the behavior of molecules in a liquid. Each molecule within a liquid has a certain amount of kinetic energy, which influences its ability to transition from the liquid phase to the vapor phase.

The kinetic energy of molecules is dependent on:

• The temperature of the liquid
• The mass of the molecules

Molecules must have sufficient kinetic energy to overcome the attractive forces keeping them in the liquid phase. If a molecule achieves this energy, it can escape and become part of the vapor above the liquid.

As a result, when analyzing vapor pressure, the kinetic energy of the molecules provides insights into how readily molecules can escape from the liquid. Liquids with molecules that frequently achieve high kinetic energy have higher vapor pressures, as more molecules are continually making the transition to the gas phase.