1. The student will learn:
Gas Unit 1/5
The student will learn:
The five basic assumptions of the Kinetic Molecular Theory.
The difference between an Ideal Gas and a Real Gas
Four items necessary for gas conversions (volume, temperature, moles, molecules)
Calculations of conversion between four different pressure measurements.
atm, mmHg, mmtorr, Kpa

2. Kinetic Molecular Theory
KMT
Kinetic Molecular Theory
1. Gases consist of particles far apart.
Collisions between particles are elastic elastic meaning = no net loss of KE
Gas particles are in constant, rapid, random motion
No forces of attraction or repulsion between gas particles.
Average KE of a gas depends on Temperature of gas.

3. One inch 50 feet 6 miles 1 yard 2mile
If the molecules of air that surrounds us could be magnified until they were as big as tennis balls, the average distance between the molecules would be:
One inch
50 feet
6 miles
1 yard
2mile

4. (Noble gases) closest thing to it
Ideal Gases: an imaginary gas that
perfectly fits all assumptions of KMT.
(Noble gases) closest thing to it
Real Gases: does not behave completely
to the laws and theories of the KMT.

5. Need to know 4 items for understanding Gases
Volume: liters and milliliters
Temperature: Kelvin K K = oC
convert 42oC =
126oC=
212oC=
Zero degrees Kelvin = absolute zero
coldest temperature
never reachable

6. What is -10OC on the Kelvin scale?
None of these

7. STP === standard temperature pressure
Need to know 4 items for understanding Gases
Volume: Temperature:
# of moles or molecules
avogadro’s number x 1023 molecules per mole
22.4 liters per mole @ STP
STP === standard temperature pressure
OoC or 273K, atm

8. S.T.P. means…. -273K and 1atm OOC and 1atm 25Oc and 760mmHg
Zero Kelvin and 760mmHg

9. Pressure: atm atmosphere of pressure
1 atm = 760 mm Hg = 760 torr = kpa
Sea level pressure = 1 atm or 760mm Hg or kpa
STP === standard temperature pressure
OoC or 273K, 1atm
Average pressure in Denver Colorado is 0.083atm.
Exress in mm Hg and kpa

10. 752 mmHg to atm. 3 atm to torr 780mmHg to kPa 320 kPa to atm

11. 799 torr to atmospheric pressure 799 torr to kPa 1. 78 atm to kPa 85
799 torr to atmospheric pressure 799 torr to kPa 1.78 atm to kPa 85.4 kPa to mmHg

12. 1.83 atm to mmHg 790mmHg to kPa 123.85 kPa to atm 745mmHg to torr

13. The student will learn:
Gas Unit 1/5
The student will learn:
The five basic assumptions of the Kinetic Molecular Theory.
The difference between an Ideal Gas and a Real Gas
Four items necessary for gas conversions (volume, temperature, moles, molecules)
Calculations of conversion between four different pressure measurements.
atm, mmHg, mmtorr, Kpa

14. Gas Unit 2/5
The student will learn:
1. Concepts concerning Boyles Law, Charles Law, Gay-Lussac Law.
2. Calculations of gas problems using the Combined Gas Law.
PV = PV
T T

15. Boyles Law: keeping temperature same P1V1 = P2V2
Pressure down = volume up
Pressure up = volume down
Inversely porportioned
When cap comes off …pressure down
= volume up
Down to bottom of ocean…pressure up
= volume down

16. Charles Law:
Pressure-Volume Inversely proportional.

17. Double Remain the same Decrease by 1/3 Decrease by ½ Triple
Doubling the initial pressure of one liter of a gas causes the volume of the gas to :
Double
Remain the same
Decrease by 1/3
Decrease by ½
Triple

18. V1 T1 V2 T2 Charles Law: keeping pressure same =
temperature up volume up
temperature down volume down
Balloon in freezer vs balloon next to heat
Car tires in summer vs. tires in winter V1 T1 V2 T2
Versly propoational

19. Throw hair spray can in fire
Gay-Lussac’s law : keeping volume same
Temperature up = pressure up
Temperature down = pressure down
Throw hair spray can in fire
P1 = P2
T T2

20. Combined Gas Laws: all 3 put together P1V1 = P2V2 T1 T2
Worksheet 11.0
1)A scuba diver at the beach has his 24 L air tank sitting outside in a temperature of 30 degree Celsius and the tank pressure registers at 12atm. As he dives down into the ocean the temperature of the water and tank drop to 10 degrees Celsius. What is the new pressure of the scuba tanks?

21. 2. A gas has a volume of 22 liters, a pressure of 3. 5 atm and a
2. A gas has a volume of 22 liters, a pressure of 3.5 atm and a temperature of 278K. If I raise the temperature to 350K and lower the pressure to 1.5 atm. What is the new volume of the gas?

22. 3. A balloon has a volume of 28L at the beach with standard pressure
3. A balloon has a volume of 28L at the beach with standard pressure. As the balloon rises the volume changes to 30L and its temperature decreased to 15Oc . The presssure is recorded by the instrument panel to be 0.75atm at the height of its rise. What was the temperature at the beach?

23. 4. If I have 15L of oxygen gas held at a pressure 55atm and a temperature of 800K, what will the volume of the gas if I decrease the pressure to 45atm and decrease the temperature to 775K?

24. A student was assigned to calculate the unknown volume of gas held at temperature of 75K in a container with a pressure of 60 atm. If increasing the temperature to 225 K and decreasing the pressure to 15 atm causes the volume of the gas to be 32 liters, how many liters of unknown gas did the student calculate?

25. 6. An aerosol can of hair spray holds 0. 25 liters of spray at STP
6. An aerosol can of hair spray holds 0.25 liters of spray at STP. Then a crazy chemistry student throws the can into a campfire, which is 1400 degrees Celsius. How much pressure may be generated? What will determine if the can explodes?
Ws.11.0

26. Gas Unit 2/5
The student will learn:
1. Concepts concerning Boyles Law, Charles Law, Gay-Lussac Law.
2. Calculations of gas problems using the Combined Gas Law.
PV = PV
T T