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Chapter 13 Notes – Gases.

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Presentation on theme: "Chapter 13 Notes – Gases."— Presentation transcript:

1 Chapter 13 Notes – Gases

2 Gases are different

3 Properties of Gases The volume of a gas is highly variable
Gases can be compressed Gases can be very “diffuse”, or spread out Solids can only be compressed a little Liquids can not be compressed Gases have low densities Gases have small amounts of mass per unit of volume

4 Behavior of Gases Effusion vs diffusion

5 Kinetic Molecular Theory
Assume: all gases are ideal Is this a correct assumption? Kinetic Molecular Theory (KMT) developed in the 1800’s

6 Kinetic Molecular Theory
Ideal gas particles are so small that their individual volume is zero (compared to the total volume of the gas) They move constantly, rapidly, and randomly, till they collide There are no attractive or repulsive forces between ideal gas molecules Collisions between molecules are 100% elastic

7 KMT (cont’d) Average kinetic energy is proportional to temperature in Kelvin 0 degrees K means what?

8 Kinetic Energy ½ mv2 Energy of motion
What does this mean in the equation above? As mass increases, velocity must decrease As mass decreases, velocity increases A smaller particle moves faster!

9 Variables that describe gases
Average kinetic energy is proportional to temperature The average number of molecules is moving at an average speed, with an average KE Some move higher, and some lower

10 Volume Volume = length x height x width
Can be measured in cm3, mL, L, m3 Gas volumes are often measured by water displacement The amount of water the gas displaces is equal to its volume

11 Pressure Pressure is force per unit area
Pressure = force/unit area For gases, it is a measure of the force when molecules collide with the container. The atmosphere exerts pressure on the earth

12 STP = Std. Temp. and Press. “Standard” temperature and pressure is:
0°C and atm This is the same as: K and kPa (kilopascals) K and 760 mm Hg K and 760 torr

13 Volatile Liquids Liquids that are flammable!!
They have high vapor pressures. They boil at low temperatures They have weak attractive forces They often have strong smells!

14 Vapor pressure The pressure of a vapor over its liquid
Equilibrium VP: when molecules leave the liquid at the same rate as they enter. Boiling: when vapor pressure equals atmospheric pressure, liquids boil.

15 Gas Laws Dalton’s Law of Partial Pressure
The total pressure of a gas is the sum of the pressures of all its parts. Ptot = Pa + Pb + Pc + … + Pz Example:.

16 Gas Laws Charles’ Law Volume is proportional to temperature

17 Gas Laws Boyle’s Law Pressure and volume are inversely proportional

18 The combined gas law Combines Boyle’s and Charles’ Laws:
What variable must we assume is held constant? Example: A helium balloon with a volume of 410 mL is cooled from 27 to –27°C. The pressure is reduced from 110 kPa to 25 kPa. What is the volume of the gas at the lower temperature and pressure?

19 The ideal gas law The ideal gas law relates all 4 variables, P,V,T, and n. PV = nRT What is R? It is a constant: L•kPa/mol•K Or, L•atm/mol•K Which one do I use? Use the one that will cancel out units appropriately.

20 Example: How many liters of hydrogen gas can be produced at 300K and 104kPa if 20g of sodium metal react with water? 2Na + 2H2O  2NaOH + H2

21 Gases and condensation
These two assumptions from KMT aren’t exactly true: Volume of gases is zero No attractive forces between particles At high pressure, gases don’t condense like you think because they DO have volume! And, they do have attractive forces, especially if they are close together.

22 Phase diagrams A graph showing the relationships between solid, liquid, gas, and temperature and pressure Normal boiling point: the temperature at which a substance boils at atm.

23 Things you’ll see on a phase diagram
Sublimation: when a solid goes to a gas Triple Point: temperature and pressure where solid, liquid, and gas all coexist Critical Point: Is it a gas or liquid – who knows? Interactive Phase Diagram

24 Gases: a review A child receives a balloon filled with 2.30 L of helium from a vendor at a fair. The outside temperature is 311K. What will the volume be when she goes home to her air conditioned house at 295K?

25 2. At a deep sea station 200 m below the surface of the pacific ocean, workers live in a highly pressurized environment. How many liters of gas at STP on the surface must be compressed to fill the underwater environment with 2x107 L of gas at 20 atm? Assume constant temperature.

26 Real Gases In the real world, the behavior of gases only conforms to the ideal-gas equation at relatively high temperature and low pressure.

27 Real Gases Even the same gas will show wildly different behavior under high pressure at different temperatures.

28 Deviations from Ideal Behavior
The assumptions made in the kinetic-molecular model (negligible volume of gas molecules themselves, no attractive forces between gas molecules, etc.) break down at high pressure and/or low temperature.

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