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Chapter 10: Problem 13

How is the vapor pressure of a liquid related to its boiling point?

Short Answer

Expert verified
The vapor pressure of a liquid is directly related to its boiling point. The lower the vapor pressure of a liquid at a given temperature, the higher the boiling point of the liquid. This is because boiling occurs when the vapor pressure equals the atmospheric pressure, and this state is reached faster for substances with higher vapor pressures, hence they have lower boiling points.

Step by step solution

01

Understanding Vapor Pressure

Vapor pressure is the pressure exerted by a vapor in thermodynamic equilibrium with its condensed phases (solid or liquid) at a given temperature in a closed system. When the liquid molecules gain enough energy to overcome intermolecular forces, they can escape into the vapor phase, creating pressure.
02

Understanding Boiling Point

The boiling point of a liquid is the temperature at which the pressure exerted by the liquid equals the external pressure surrounding the liquid. Therefore, the boiling point is the temperature at which the vapor pressure of the liquid matches the atmospheric pressure on the liquid.
03

Relating Vapor Pressure to Boiling Point

As the temperature increases, more molecules gain enough energy to overcome intermolecular forces and go into the vapor phase, thereby increasing the vapor pressure. When the vapor pressure of the liquid equals the atmospheric pressure, boiling begins. Hence, the lower the vapor pressure of a liquid at a given temperature, the higher the temperature must be raised to reach the boiling point. In other words, substances with higher vapor pressures at a given temperature generally have lower boiling points.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Boiling Point
The boiling point is an essential concept in chemistry and every day life. It refers to the temperature at which a liquid鈥檚 vapor pressure equals the external atmospheric pressure. At this point, the liquid can turn into vapor throughout the substance, not just on the surface.

The boiling point is unique for every liquid and can vary with pressure changes. For example:
  • At higher altitudes, the atmospheric pressure is lower, so liquids boil at lower temperatures.
  • Pressure cookers increase internal pressure, causing water to boil at a higher temperature and cooking food faster.
Understanding the boiling point helps us predict how liquids will behave under different conditions, making it easier to control various scientific and industrial processes.
Intermolecular Forces
Intermolecular forces are the invisible bonds holding molecules together within a substance. They determine how much energy is needed for molecules to escape from a liquid to a vapor phase, which affects vapor pressure and boiling point.

There are different types of intermolecular forces that vary in strength:
  • Dispersion Forces: Present in all molecules, these are the weakest type of forces that result from momentary polarization.
  • Dipole-Dipole Interactions: Occur between polar molecules with permanent dipoles.
  • Hydrogen Bonds: A strong type of dipole-dipole interaction, occurring when hydrogen is bonded to electronegative atoms like oxygen or nitrogen.
Stronger intermolecular forces lead to lower vapor pressures and higher boiling points because more energy is needed to separate the molecules.
Thermodynamic Equilibrium
Thermodynamic equilibrium is a state where all parts of a system are at a steady state with no net changes taking place over time. In the context of vapor pressure and boiling point, it refers to the balance between the liquid phase and vapor phase of a substance.

When a liquid is in a closed container:
  • Some molecules escape from the liquid to become vapor, while some vapor molecules return to the liquid.
  • This dynamic process continues until the rate of evaporation matches the rate of condensation, achieving equilibrium.
At this point, the vapor pressure becomes constant, and it is said to be at equilibrium with its liquid. Understanding this equilibrium helps in predicting how systems will respond to changes in temperature and pressure, fundamental in fields like chemistry and engineering.

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