- Define vapor pressure.
- Describe the relationship between the intermolecular forces in a liquid and its vapor pressure.
- Describe the relationship between the vapor pressure of a liquid and temperature.
What causes this toy to move?
The drinking duck is a toy that many kids (and adults) enjoy playing with. You can see the drinking duck in action in the video at the link below:
The motion of the duck illustrates a physical principle called vapor pressure. As the vapor pressure changes, the liquid in the duck moves up and down, causing the duck to move.
When a partially filled container of liquid is sealed with a stopper, some liquid molecules at the surface evaporate into the vapor phase . However, the vapor molecules cannot escape from the container and so after a certain amount of time, the space above the liquid reaches a point where it cannot hold any more vapor molecules. Now some of the vapor molecules condense back into a liquid. The system reaches the point where the rate of evaporation is equal to the rate of condensation (see Figure below ). This is called a dynamic equilibrium between the liquid and vapor phases.
Equilibrium between liquid phase and vapor phase.
A dynamic equilibrium can be illustrated by an equation with a double arrow, meaning that the reaction is occurring in both directions and at the same rate.
The forward direction represents the evaporation process, while the reverse direction represents the condensation process.
Because they cannot escape the container, the vapor molecules above the surface of the liquid exert a pressure on the walls of the container. The vapor pressure is a measure of the presure (force per unit area) exerted by a gas above a liquid in a sealed container. Vapor pressure is a property of a liquid based on the strength of its intermolecular forces. A liquid with weak intermolecular forces evaporates more easily and has a high vapor pressure. A liquid with stronger intermolecular forces does not evaporate easily and thus has a lower vapor pressure. For example, diethyl ether is a nonpolar liquid with weak dispersion forces. Its vapor pressure at 20°C is 58.96 kPa. Water is a polar liquid whose molecules are attracted to one another by relatively strong hydrogen bonding. The vapor pressure of water at 20°C is only 2.33 kPa, far less than that of diethyl ether.
Vapor Pressure and Temperature
Vapor pressure is dependent upon temperature. When the liquid in a closed container is heated, more molecules escape the liquid phase and evaporate. The greater number of vapor molecules strike the container walls more frequently, resulting in an increase in pressure. The Table below shows the temperature dependence of the vapor pressure of three liquids.
Notice that the temperature dependence of the vapor pressure is not linear. From 0°C to 80°C, the vapor pressure of water increases by 46.73 kPa, while it increases by 53.99 kPa in only a span of twenty degrees from 80°C to 100°C.
- Vapor pressure is a measure of the pressure exerted by a gas above a liquid in a sealed container.
- Strong intermolecular forces produce a lower rate of evaporation and a lower vapor pressure.
- Weak intermolecular forces produce a higher rate of evaporation and a higher vapor pressure.
- As the temperature increases, the vapor pressure increases.
Use the link below to answer the following questions:
- What material has the highest vapor pressure at 25°C?
- What material has the lowest vapor pressure at 25°C?
- What device is used to measure vapor pressure?
- Does the surface area of the liquid affect the vapor pressure?
- Define vapor pressure.
- How do intermolecular forces affect vapor pressure?
- How does temperature affect vapor pressure?
- liquid phase: A substance in the liquid state of matter.
- vapor phase: A substance in the gaseous state of matter.
- vapor pressure: A measure of the force exerted by a gas above a liquid in a sealed container.