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. Intermolecular attractive forces play a role in determining the tendency of a liquid's molecules to escape into the vapor phase, while temperature influences the kinetic energy of the molecules, affecting the vapor pressure.

Step-by-step solution

Understand the problem

Firstly, it is important to recognize that we are looking for the factors that affect the vapor pressure of a liquid. Vapor pressure refers to the equilibrium pressure exerted by a vapor in contact with its liquid or solid condensed phase.

Analyzing the factors individually

Now, let's analyze each of the given factors one by one: (a) Volume of the liquid: The vapor pressure does not depend on the volume of the liquid. It is an intrinsic property of the substance, given by the temperature. (b) Surface area: The vapor pressure also does not depend on the surface area of the liquid. The rate of evaporation from the surface may indeed differ with surface area, but the vapor pressure is independent of the surface area. (c) Intermolecular attractive forces: This is an important factor that affects vapor pressure. When the intermolecular forces are strong, the tendency of a liquid's molecules to escape into the vapor phase is reduced because the molecules are "held" more tightly to each other. This leads to a lower vapor pressure. (d) Temperature: This is another crucial factor that affects the vapor pressure of a liquid. As the temperature increases, the kinetic energy of the molecules increases, and more molecules escape into the vapor phase. This results in higher vapor pressure. (e) Density of the liquid: The vapor pressure does not depend on the density of the liquid, because it depends on the intermolecular forces within the liquid and the temperature, not on how closely packed the molecules are.

Determine which factors affect vapor pressure

Based on the analysis of each factor, we can conclude that the factors which affect the vapor pressure of a liquid are: - Intermolecular attractive forces (c) - Temperature (d) So, the answer is (c) intermolecular attractive forces, and (d) temperature.

Key concepts

Intermolecular Forces

Intermolecular forces play a crucial role in determining the vapor pressure of a liquid. These are the forces that act between the molecules in a liquid. They include forces such as hydrogen bonding, dipole-dipole interactions, and London dispersion forces.
When the intermolecular forces are strong, the molecules within the liquid are held together more tightly. This means it's harder for the molecules to escape into the vapor phase, which results in a lower vapor pressure.
Think of it like friends holding hands tightly—they’re less likely to drift apart. In contrast, with weak intermolecular forces, molecules can easily escape, leading to a higher vapor pressure.

• Strong intermolecular forces = Low vapor pressure
• Weak intermolecular forces = High vapor pressure

Understanding these interactions helps us predict how a liquid will behave under different conditions.

Temperature Effects on Vapor Pressure

Temperature has a direct and significant effect on the vapor pressure of a liquid. As the temperature increases, the energy of the liquid's molecules also increases. This added energy helps more molecules overcome intermolecular forces and enter the vapor phase.
In simpler terms, think of temperature as giving molecules a little boost or push. As the molecules gain energy, they move faster, breaking free more easily from the liquid surface. Thus, higher temperatures lead to a higher vapor pressure.
The relationship between temperature and vapor pressure is usually exponential. This means a small increase in temperature can result in a large increase in vapor pressure.

• Higher temperature = Higher vapor pressure
• Direct correlation between temperature increase and vapor pressure

It's essential to note that this effect is the same regardless of the liquid type, although different liquids will respond differently based on their specific intermolecular forces.

Intrinsic Properties of Liquids

Vapor pressure is an intrinsic property of a liquid, meaning it is inherent to the liquid and not dependent on external factors like volume or surface area. An intrinsic property describes characteristics that are essential to the identity of a substance.
For vapor pressure, this means that regardless of how much liquid you have or the size of the surface area, the vapor pressure remains constant at a given temperature.
These intrinsic properties arise from the molecular composition of the liquid. Liquids with different molecular structures and intermolecular forces exhibit different vapor pressures at the same temperature.

• Independent of external factors like volume or surface area
• Dependent on molecular structure and intermolecular forces

This intrinsic nature is what allows chemists to predict how a liquid will behave under certain conditions, knowing its molecular makeup and temperature.