Question

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

Short answer

The factors that affect the vapor pressure of a liquid are (c) intermolecular attractive forces and (d) temperature. Stronger intermolecular forces result in lower vapor pressure, while weaker intermolecular forces lead to higher vapor pressure. Additionally, the vapor pressure increases as temperature increases. The volume of the liquid, surface area, and density do not directly affect the vapor pressure.

Step-by-step solution

Option (a): Volume of the liquid

The volume of the liquid does not affect its vapor pressure. Vapor pressure depends on the equilibrium between the liquid and vapor phases, which is determined by intermolecular forces and temperature, irrespective of the volume of the liquid.

Option (b): Surface area

The surface area of a liquid does not directly affect its vapor pressure. However, surface area may influence the rate of evaporation of the liquid. But since vapor pressure is a property of the liquid-vapor equilibrium, it does not depend on the surface area.

Option (c): Intermolecular attractive forces

Intermolecular attractive forces play a crucial role in determining the vapor pressure of a liquid. Stronger intermolecular forces make it more difficult for the molecules to escape the liquid and enter the vapor phase, resulting in lower vapor pressure. On the contrary, weaker intermolecular forces lead to higher vapor pressure.

Option (d): Temperature

Temperature affects the vapor pressure of a liquid. As temperature increases, the kinetic energy of the liquid molecules increases, making it easier for them to escape into the vapor phase. Consequently, the vapor pressure of the liquid increases with increasing temperature.

Option (e): Density of the liquid

The density of the liquid does not directly affect its vapor pressure. However, it may be indirectly related to vapor pressure, as liquids with higher densities often have stronger intermolecular forces. But the density itself does not influence the vapor pressure.

Final Answer

Based on our analysis, the factors that affect the vapor pressure of a liquid are (c) intermolecular attractive forces and (d) temperature.

Key concepts

Understanding Intermolecular Forces

Intermolecular forces are the invisible glue that holds the molecules of a liquid together. These forces affect how tightly or loosely the molecules are packed. There are different kinds of intermolecular forces, including hydrogen bonds, dipole-dipole interactions, and dispersion forces, each having its own strength and characteristics.

• **Hydrogen bonds** are the strongest among these forces. They occur when hydrogen is bonded to electronegative atoms like oxygen or nitrogen.
• **Dipole-dipole interactions** happen in molecules that have a permanent electric dipole. These are generally weaker than hydrogen bonds but stronger than dispersion forces.
• **Dispersion forces** are the weakest and occur in all molecules, mainly influencing non-polar substances.

The strength of these intermolecular forces significantly influences a liquid's vapor pressure. When intermolecular forces are strong, molecules find it harder to escape into the vapor phase, resulting in a lower vapor pressure. Conversely, weaker forces allow molecules to easily move into the vapor phase, increasing vapor pressure.

Temperature Effects on Vapor Pressure

Temperature is a driving force that plays a pivotal role in vapor pressure. When you heat a liquid, its molecules gain kinetic energy. With more energy, molecules move around more and eventually find it easier to break free into the vapor phase. This increase in movement with rising temperature leads to higher vapor pressure.

• Every liquid has a unique vapor pressure curve, where temperature and vapor pressure are directly related. Higher temperature equals higher vapor pressure.
• At a certain temperature, known as the boiling point, vapor pressure equals atmospheric pressure, causing the liquid to boil.

This principle is crucial for understanding phenomena like boiling and evaporation. Thermometers, pressure cookers, and even some cooking techniques rely heavily on the interplay between temperature and vapor pressure.

Liquid-Vapor Equilibrium Explained

Liquid-vapor equilibrium occurs when the rate of evaporation of a liquid equals the rate of condensation. In this balanced state, the vapor pressure remains constant. This equilibrium does not depend on how much liquid is present or the container's size. Rather, it is influenced by the nature of the liquid and external conditions.

• The equilibrium is dynamic, meaning that although the rates are equal, molecules constantly move between the liquid and vapor phases.
• Factors influencing liquid-vapor equilibrium include temperature and intermolecular forces, both crucial in determining the vapor pressure.

Understanding liquid-vapor equilibrium helps explain why certain liquid behaviors, such as evaporation and boiling, occur. It's a foundational concept in physical chemistry, vital for fields like chemical engineering, meteorology, and environmental science.