1. The Gas Laws
You can predict how pressure, volume, temperature, and number of gas particles are related to each other based on the molecular model of a gas.

2. The Gas Laws The Kinetic Molecular Theory
1.) Gas particles are in constant motion and move in a straight line until they hit another gas particle or the side of the container.
2.) There are not attractive or repulsive forces between the gas particles.
3.) The volume of the actual gas particle is assumed to be zero, since it is insignificant to the volume of the whole sample of gas.

3. The Gas Laws The Kinetic Molecular Theory (cont.)
4.) The temperature is an indirect measure the average kinetic energy of all the gas particles in the sample.
Kinetic Energy = ½ (mass) x (velocity)2
5.) There is no exchange of energy when 2 gas particles collide, the collision is totally elastic.
(Just like when two billiard balls collide.)

4. The Gas Laws Pressure Pressure = Force Applied / Area (P = F / A)
When the gas molecules collide with the inside wall of the container, it exerts a force over an area. Therefore there is always an internal pressure on a gas.

5. The Gas Laws Measuring Pressure
Pressure can be measured using a device called a manometer.

6. The Gas Laws Measuring Pressure
Atmospheric Pressure can be measured using a device called a barometer.

7. 1 atm = 101,300 Pa = 101.3 kPa = 14.7 psi = 760 torr = 760 mm Hg
The Gas Laws
Units for Measuring Pressure
Pascal (Pa) – Metric System unit for pressure
Atmosphere (atm)
Pounds per square inch (psi)
Torricelli (torr)
Millimeter of Mercury (mm Hg)
1 atm = 101,300 Pa = kPa = 14.7 psi = 760 torr = 760 mm Hg

8. 1 atm = 101,300 Pa = 101.3 kPa = 14.7 psi = 760 torr = 760 mm Hg
The Gas Laws
Pressure Conversions
1 atm = 101,300 Pa = kPa = 14.7 psi = 760 torr = 760 mm Hg
Convert 0.75 atm into mm Hg.
Convert 32.0 psi into kPa.

9. The Gas Laws Robert Boyle (1627 – 1691)
An English scientist whose work revolved around trying to discover the relationship between the pressure and volume of a gas.

10. The Gas Laws Boyle’s Law
If the pressure exerted on a gas increases, the volume of the gas will proportionally decrease.
What is the
relationship
between the
pressure exerted on
a gas and its
volume?

11. The Gas Laws Boyle’s Law
The product of the pressure and volume of a gas must always be a constant as long as the temperature and # of moles of gas remain constant.
Pressure x Volume = constant
Pressure(initial) x Volume(initial) = Pressure(final) x Volume (final)
P1V1 = P2V2

12. The Gas Laws Boyle’s Law
Initially, a 3.0 L expandable tank of gas is under a pressure of 13 atm. What would be the volume of the tank if the pressure inside the tank is reduced to 5.0 atm. The temperature and # of moles of gas remain constant.

13. The Gas Laws Jacques Charles (1746 – 1823)
A French scientist, inventor, and avid balloonist.
He was interested in discovering the affect that the temperature had on the volume of a gas.

14. Temperature must be in Kelvins!
The Gas Laws
Charles’ Law
The volume of a gas divided by its Kelvin temperature must remain constant. As long as the pressure and # moles of gas does not change.
Volume = constant
Temperature
Volume(initial) = Volume(final)
Temperature(initial) Temperature(final)
V = V2
T T2
Temperature must be in Kelvins!

15. Charles’ Law This is how absolute zero was determined. Is it possible?
The Gas Laws
Charles’ Law
This is how absolute zero was determined. Is it possible?

16. The Gas Laws Charles’ Law Problem
A balloon has a volume of 1.0 L at 23.0°C. What is the volume of the balloon if the temperature decreases to -10.0°C? Assume that the pressure and # of moles of gas particles remains constant.

17. The Gas Laws
Combined Gas Law (Boyle’s and Charles’ Law)
P1.V1 = P2.V2
T T2
The number of moles of gas must remain constant.

18. The Gas Laws Combined Gas Law (Boyle’s and Charles’ Law)
A 2.0 L balloon initially at Standard Temperature and Pressure (STP) is heated to °C and pressurized to 1.5 atmospheres. Calculate the new volume of the balloon.

19. The Gas Laws Joseph Louis Gay-Lussac (1778 – 1850)
French Chemist and Physicist who discovered th relationship between the pressure and the temperature of a gas.

20. The Gas Laws P1 = P2 T1 T2 Joseph Louis Gay-Lussac (1778 – 1850)
Gay-Lussac’s Law
P1 = P2
T T2
The volume and number of moles of gas must remain constant.

21. The Gas Laws Gay-Lussac’s Law
Initially, a sample of gas has a temperature of 10.0°C. It is then pressurized from 740. mm Hg to 800. mm Hg. What will be the new temperature of the gas if the volume and number of moles of gas remain constant?

22. The Gas Laws The Ideal Gas Law
The only gas law that incorporates moles into it.
PV = nRT
P = Pressure (atm or kPa)
V = Volume (L)
n = # of moles of gas particles
R = The Gas Law Constant ( L.atm)
mol.K
T = Temperature (K)

23. The Gas Laws The Ideal Gas Law
What volume would grams of CO2 occupy at 0.00°C and 1.00 atmosphere?

24. The Gas Laws The Ideal Gas Law
What is pressure of 10.0 grams of NH3 in a 5.0 L tank at 50.0°C?

25. The Gas Laws
Using the Ideal Gas Law to Relate Molar Mass and Density of Gas;
We can rearrange the Ideal Gas Law to get the following equation -
P.V = nRT ==== n = P
V RT

26. The Gas Laws
Using the Ideal Gas Law to Relate Molar Mass and Density of Gas;
If we multiply both sides of the Ideal Gas Law by molar mass, we have the following –
(molar mass) n = P (molar mass)
V RT
Mass = P (molar mass)
Volume RT

27. The Gas Laws
Using the Ideal Gas Law to Relate Molar Mass and Density of Gas;
Mass = P (molar mass)
Volume RT
Density = P (molar mass) RT

28. The Gas Laws
Using the Ideal Gas Law to Relate Molar Mass and Density of Gas;
Density = P (molar mass) RT
Calculate the density of nitrogen gas at a pressure of 1.5 atm and a temperature of -10.0°C.

29. The Gas Laws
Using the Ideal Gas Law to Relate Molar Mass and Density of Gas;
Density = P (molar mass) RT
Calculate the molar mass of a gas that has a density of g / L when it is at a pressure of 800. kPa and 25.0°C.

30. The Gas Laws Using the Ideal Gas Law with Gas Stoichiometry;
How many grams of hydrogen gas is needed to fill a L vessel with ammonia gas at 1.2 atm at a temperature of -25.0°C?
N2(g) + 3H2(g)  2NH3(g)

31. The Gas Laws Using the Ideal Gas Law with Gas Stoichiometry;
Automobile airbags are inflated with nitrogen gas using the following chemical reaction;
2NaN3(s)  2Na(s) + 3N2(g)
How many grams of NaN3 must decompose in order to fill a 40.0 L airbag with nitrogen gas at 30.0°C and 1.0 atm?

32. John Dalton (1766-1844) What did he not do?
The Gas Laws
John Dalton ( )
What did he not do?

33. 0.05atm trace gases = 1.0 atm (atmospheric pressure)
The Gas Laws
Dalton’s Law of Partial Pressures
The partial pressure (pgas X) of a gas is the pressure that the gas exerts when it is part of a mixture of gases.
Right now, the room that we are sitting in contains nitrogen gas, oxygen gas, water vapor, and trace amount of other gases.
0.21 atm O atm N atm CO2 +
0.05atm trace gases = 1.0 atm (atmospheric pressure)

34. p gas 1 + p gas 2 + p gas 3 + ……… = P total
The Gas Laws
Dalton’s Law of Partial Pressures
The total pressure of a mixture of gases is equal to the sum of all of the partial pressures of the gases that make up the gas mixture.
p gas 1 + p gas 2 + p gas 3 + ……… = P total

35. The Gas Laws Graham’s Law of Effusion
Grahams Law Describes the relative speed (velocity) at which gas particles will move, or diffuse.

36. The Gas Laws Graham’s Law of Effusion
Effusion – The movement of a gas molecule through a small hole so its velocity may be measured.
Diffusion – The movement of gas particles from an area of high concentration to an area of low concentration.

37. Graham’s Law of Effusion What is diffusion?
The Gas Laws
Graham’s Law of Effusion
What is diffusion?

38. The Gas Laws Graham’s Law of Effusion
A heavier gas particle will travel slower than a lighter gas particle.
KE = ½ mass x velocity2
If the kinetic energy is the same for a heavy and a light gas particle, then the velocity of the heavier one will be less than the velocity of the lighter one.

39. NH3(g) + HCl(g)  NH4Cl(s)
The Gas Laws
Graham’s Law of Effusion
Ammonia and hydrogen chloride gas will form the white precipitate ammonium chloride;
NH3(g) + HCl(g)  NH4Cl(s)

40. NH3(g) + HCl(g)  NH4Cl(s)
The Gas Laws
Graham’s Law of Effusion
Ammonia and hydrogen chloride gas will form the white precipitate ammonium chloride;
NH3(g) + HCl(g)  NH4Cl(s)
Which end contains the
ammonia?

41. The Gas Laws Graham’s Law of Effusion
Which molecule will diffuse faster, H2 or O2? How many times faster will the ‘faster’ molecule diffuse compared to the slower one?