Title: Evaporation and Boiling Point
1Evaporation and Boiling Point
- Chapter 14. Sections 14.4 and 14.5
2Review
- What is the heat of fusion?
- What is the heat of vaporization?
- What phase change occurs with vaporization?
3Evaporation and Vapor Pressure
- When water goes from being a liquid to a gas,
this is called vaporization - The water molecules have overcome the
intermolecular forces in liquid water and escaped
into gas or vapor form
4Evaporation and Vapor Pressure cont
- When boiling happens heat energy is added to
overcome the intermolecular forces - How about evaporation? There isnt heat energy
being added, but the molecules still overcome the
intermolecular forces? - In evaporation, there are still energy changes
occurring. - You have to remember that heat is only the
AVERAGE kinetic energy of a substance
5Evaporation and Vapor Pressure cont
- Some parts of the water have very low kinetic
energy, however some have a lot. - So the faster moving molecules can escape,
evaporation.
6Evaporation and Vapor Pressure cont
- Now if this process occurs in an insulated
container (no heat can flow in or out) then the
process is endothermic because the average
kinetic energy is being lowered (taken in) - If the container is not being insulated the temp
will remain the same, however the process is
still endothermic because energy is still being
taken in
7Vapor Pressure
- In a sealed container, there may be slight
evaporation at first, but it will soon stabilize - In fact some of the vapor molecules will return
to a liquid state - This is called condensation.
8Vapor Pressure cont
- At the point where no further changes occur in
the amounts of liquid and vapor in a closed
container, because the two processes equally
balance each other, the system is in equilibrium - The amount of a pressure of the gas at
equilibrium is referred to as vapor pressure
9 (a) Measuring vapor of a liquid by using a
simple barometer. (b) The water vapor pushed the
mercury level down. (c) Diethyl ether shows a
higher vapor pressure than water.
10Vapor Pressure cont
- The vapor pressure of certain liquids vary
- Liquid with high vapor pressure are said to be
volatile - The vapor pressure of a liquid at a given temp is
said to be determined by the intermolecular
forces - The stronger the intermolecular forces, the lower
the vapor pressure because it is hard for
molecules to go to the gas phase
11Vapor Pressure cont
- You can predict which molecule will have a high
vapor pressure, by looking at the number of polar
(or O-H) bonds - Example H2O and CH3OH
- H2O has 2 O-H bonds
- CH3OH has 1 O-H bond
- So Water has more polarity and lower vapor
pressure
12Boiling point and vapor pressure
- When you look at boiling water, what do you
notice?
13Boiling point and vapor pressure cont
- When heat energy is added to water, there are
already tiny air bubbles in the water. - The water turns to a vapor inside the air bubbles
14Boiling point and vapor pressure cont
- The bubble can only form when the water molecules
pressure can be equal to or greater than the
atmospheric pressure. - So the vapor pressure of the water must be equal
to the pressure outside of it
15Boiling point and vapor pressure cont
- The lower the atmospheric pressure, the easier it
is for water vapor to form. - Does this tell you why water boils at lower
temperatures at high elevations?
16Boiling point and vapor pressure cont
- http//www.dac.neu.edu/physics/b.maheswaran/phy112
1/data/ch04/anim/anim0405.htm
17Homework
- Read pages 449-453, problems 1-3 on 453 and
problems 28 and 31 on page 464