1. Gas Properties and Behavior
Chemistry

2. Properties of Gases - KMT
1. Mostly empty space 2. Particles are always moving (fast) 3. Volume depends on temp and pressure 4. Shape depends on the container (earth??) 5. Kinetic energy of particles determines speed. (temp)

3. Gas Pressure
Pressure: the force acting on a unit area of a surface (example: force per square centimeter)
Atmospheric pressure: 14.7psi (pounds per square inch) at sea level; also called: 1 atm
Kinetic Theory: all matter is composed of particles in constant, random motion.
Gas pressure is caused by the gas particles hitting the sides of the container.(collisions)

4. Pressure
Defined: Force per unit area Occurs when particles collide with walls of container. -more collisions = more pressure

5. Kinetic Energy, Speed, and Temp.
KE is energy of motion
Temperature is a measure of average KE
Both are linked to the speed of the particles
TEMP KINETIC ENERGY
(SPEED)

6. Atmospheric pressure
Air pressure or barometric pressure (comes from the weight of the air)

7. Barometric pressure
Higher at sea level than on top of mountains. Why????

8. Ideal gases
A gas that is described by the kinetic molecular theory (model) (particles have no attractions and can be compressed to zero). Real gases will condense to a liquid and particles have some (small) volume.

9. Kinetic Molecular Theory - Gases
Group of statements that describe physical characteristics of gases.
1. made of very tiny atoms
2. move constantly, straight lines, random
3. very far apart (particle volume is almost zero)
4. collisions cause pressure and conserve energy.
5. No attractions between particles.

10. Pressure
Measured with a barometer or pressure gauge. Units are: mmHg (Torr) (common) or psi (USA only) Pascal (official SI unit) but is really tiny or kilopascal (more likely) or Atmosphere (my favorite)

12. Pressure Conversions Standard (Equivalent) Pressure: at sea level
1.0 atm = 760 mmHg = 14.7 psi = kPa
Problem: Tire pressure gauge reads 35psi. What is the equivalent in kilopascals?
(35psi) x kPa = 240 kPa
14.7 psi

13. Make conversions Change 2.0 atm to kPa 2.0 atm x 101.3 kPa = 202.6 kPa
Given x conversion factor = new value
2.0 atm x kPa = kPa
1.0 atm

14. Temperature Fahrenheit – common, not scientific
Celcius – used everywhere, except USA, based on water MP = 0°C BP = 100°C
Absolute zero = -273°C
Kelvin – (Absolute temperature) used for all gas law calculations
absolute zero 0°K = no motion of atoms
No negative temp.
K = C + 273

15. Kelvin Temperature Scale
Absolute Zero = zero kinetic energy; particles are not moving at all. Absolute zero has never been reached.
Kelvin Scale: directly proportional to kinetic energy of particles.
Celsius Kelvin
100oC 373
0oC 273
-273oC

16. STP Standard Temperature and Pressure 1 atm pressure and 273 K
Used to compare measured gases in diff. experiments.
1 atm pressure and 273 K
Molar Volume (22.4 L/mol)
At STP 1.0 mole of any gas occupies 22.4 L

17. The Gas Laws Statements which predict gas behaviors Math relationships
Mostly common sense.
Know relationships and graph

18. Daltons law of partial pressure.
In a mixture of gases, the total pressure equals the sum of all the individual gases.
P1 + P2 + P3…… =PTotal

19. Boyles law
Pressure and volume are inversely proportional (when the temp. stays the same)
P1 x V1 = P2 x V2
If the pressure doubles the volume is cut in half.

20. Boyle’s Law Cont. Graph resembles a curve.
Kinetic theory explanation: compressing the air (making the volume smaller) creates less space for the particles to travel = more hits = greater pressure.
Expand the volume & the particles must travel farther to hit the sides of the container = less hits = lower pressure.

21. Charles Law
Volume and Temperature(Kelvin) are directly proportional (pressure is constant)
V1 = V2
T T2
If the temperature doubles, the volume doubles
Temperature must be in Kelvins to compare.

22. Charles’s Law cont. Graph is a straight line
Kinetic Theory Explanation: When the gas particles are heated, they speed up (increase kinetic energy) = more hits on the sides of the expandable container (balloon) = greater volume.
When the gas particle are cooled, they slow down= fewer hits = less volume

23. Gay Lussac Law
Pressure and Temperature(Kelvin) are directly proportional (volume is constant)
P1 = P2
T T2
If the Temperature doubles, the pressure doubles
Temperature must be in Kelvins for calc.

24. Temperature & Gas Pressure
High temperature makes particles speed up = more hits on the sides of the container = greater pressure.
Cold temperature makes particles slow down = fewer hits = lower pressure

25. Combined Gas Law Boyles, Charles, and Gay Lussac Laws all together…..
P1V1 = P2V2
T T2
Keep track of the units - temp. must be in Kelvins, P and V must have the same units on both sides.

26. The Ideal Gas Law
Relationship between pressure, temp. volume and number of moles (particles).
Can be used to find info about any gas.
PV = nRT
P is pressure(atm or kPa) V is volume (L)
n is number of moles(mol) T is temperature (K)
and R is the ideal gas constant