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Notes on Gases: Chapter 11

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1 Notes on Gases: Chapter 11
Section 1: Properties of Gases Section 2: Gas Laws Section 3: Gas Stoichiometry Chemistry - Vaughn

2 Kinetic Molecular Theory:
Gas Properties Kinetic Molecular Theory: Gases consist of large numbers of particles that are far apart. When particles collide, they do not lose energy (aka elastic collisions). Gas particles are in continuous, rapid, random motion. There are no forces of attraction between gas particles. The temperature of a gas depends on the average kinetic energy of the gas.

3 More Properties… Expansion: -No definite shape or volume.
Gases naturally expand to fill their containers. Fluidity: Gas particles glide past one another causing them to “flow” like liquids. (Liquids and gases are FLUIDS.)

4 More Properties… Low Density:
Particles are so far apart compared to solids and liquids the density is really low…therefore, gases float! Compressibility: Gas particles can be squeezed closer together (causing the volume to decrease and the pressure to increase).

5 More Properties… Diffusion:
Natural mixing of gas particles caused by random motion. Ex. – Perfume in a room. Effusion: Process of gas particles passing through a tiny opening. Ex. – Hole in a bike tire.

6

7 Graham’s Law of Effusion
Therefore, (smaller gas) effuses _____ times faster than (bigger gas). = 4.00 Therefore, hydrogen effuses 4.00 times faster than oxygen.

8 What is Pressure? Pressure (P) is the force applied over a surface area. P = force area Pressure…Collisions against the container. More collisions means higher pressure. Barometers are used to measure atmospheric pressure. Measured in… Millimeters of mercury (mm Hg) Atmospheres (atm) Torricelli (torr) *invented the barometer* Pascal (Pa) or kilopascal (kPa)

9 Units for Pressure Units for Temperature 1 atm = 760 mm Hg
(All calculations must be in atm!!!) Atmospheric pressure at sea level: 1 atm = 760 mm Hg = 760 torr = kPa = in. Hg = 14.7 psi Units for Temperature (All calculations must be in Kelvin!!!) Converting from Kelvin  Celsius K – 273 = C Converting from Celsius  Kelvin C = K

10 Pressure Conversions Examples: Convert the following pressures:
109 kPa = ________ atm atm = ________ mm Hg 0.62 atm = ________ in. Hg 758.7 psi = _______ atm 758.7 mmHg = _______ torr 453.1 torr = ________ kPa 201.1 kPa = _______ psi 708 mmHg = _______ in. Hg

11 Pressure Conversions Examples: Convert the following pressures:
109 kPa = ________ atm atm atm = ________ mm Hg mm Hg 0.62 atm = ________ in. Hg 19 in. Hg 758.7 psi = _______ atm atm 758.7 mmHg = _______ torr torr 453.1 torr = ________ kPa kPa 201.1 kPa = _______ psi psi 708 mmHg = _______ in. Hg in. Hg

12 Standard Temperature and Pressure
Oftentimes, chemists want to use the same conditions for several experiments…so a standard temperature and pressure was agreed upon. STP = 273K and 1 atm (0ºC)

13 The Gas Laws Boyle’s Law (Pressure-Volume)
Charles’s Law (Temperature-Volume) Gay-Lussac’s Law (Temperature-Pressure) Combined Gas Law (P-T-V) Ideal Gas Law (P-T-V-Moles)

14 Boyle’s Law (Pressure-Volume)
P1V1 = P2V2 If pressure increases, volume will ________. If pressure decreases, volume will ________. This relationship is ________.

15 Boyle’s Law (Pressure-Volume)
P1V1 = P2V2 If pressure increases, volume will decrease. If pressure decreases, volume will increase. This relationship is inverse. Lungs Video Marshmallows Video

16 Charles’s Law (Temperature-Volume)
V1 = V2 T1 T2 If temperature increases, volume will _______. If temperature decreases, volume will _______. This relationship is ________.

17 Charles’s Law (Temperature-Volume)
V1 = V2 T1 T2 If temperature increases, volume will increase. If temperature decreases, volume will decrease. This relationship is direct. Liquid Nitrogen + Balloon 55-Gallon Can

18 Gay-Lussac’s Law (Temperature-Pressure)
P1 = P2 T1 T2 If temperature increases, pressure will ______. If temperature decreases, pressure will ______. This relationship is ________.

19 Gay-Lussac’s Law (Temperature-Pressure)
P1 = P2 T1 T2 If temperature increases, pressure will increase. If temperature decreases, pressure will decrease. This relationship is direct. Fountain Egg + Bottle

20 Wouldn’t it be easier if we only had one formula?
COMBINED GAS LAW P1 V1 = P2 V2 T T2 If one of these variables is constant, block it out and use the equation that is left. If temperature is constant (no T) = Boyle’s Law If pressure is constant (no P) = Charles’s Law If volume is constant (no V) = Gay-Lussac’s Law

21 T1 T2 Boyle’s Law : P1V1 = P2V2 Charles’s Law : V1 = V2 T1 T2
Summary of Formulas Boyle’s Law : P1V1 = P2V2 Charles’s Law : V1 = V2 T1 T2 Gay-Lussac’s Law : P1 = P2 Combined Gas Law : P1 V1 = P2 V2 T T2

22 P1 V1 = P2 V2 T1 T2 COMBINED GAS LAW
PRACTICE – 1 of 4 COMBINED GAS LAW P1 V1 = P2 V2 T T2 Q1: A sample of Neon gas occupies a volume of 752mL at 25.0ºC. What volume will the gas occupy at 50.0ºC if the pressure remains constant? What law will we use?

23 P1 V1 = P2 V2 T1 T2 COMBINED GAS LAW
PRACTICE – 2 of 4 COMBINED GAS LAW P1 V1 = P2 V2 T T2 Q2: A sample of oxygen gas has a volume of 150.mL when its pressure is 0.947atm. What will the volume of the gas be if the pressure increases to 0.987atm? (Temperature remains constant.) What law will we use?

24 P1 V1 = P2 V2 T1 T2 COMBINED GAS LAW
PRACTICE – 3 of 4 COMBINED GAS LAW P1 V1 = P2 V2 T T2 Q3: The gas in an aerosol can is at a pressure of 3.00atm at 25.0ºC. Directions on the can warn the user not to keep the can in a place when the temperature exceeds 52.0ºC. What would the pressure in the can be at 52.0ºC? (Assume volume remains constant.) What law will we use?

25 P1 V1 = P2 V2 T1 T2 COMBINED GAS LAW
PRACTICE – 4 of 4 COMBINED GAS LAW P1 V1 = P2 V2 T T2 Q4: A helium-filled balloon has a volume of 50.0L at 25.0ºC and 1.03atm. What volume will it have at 0.855atm and 10.0ºC? What law will we use?

26 The Ideal Gas Law A law relates pressure, volume, temperature, and the number of moles of a gas. PV = nRT P = pressure (in atm) V = volume (in L) n = number of moles (in moles) R = Ideal Gas Constant ( always) T = temperature (in Kelvin)

27 The Ideal Gas Law PV = nRT Always L Always mol Always weird Always K
Pressure (P) Volume (V) Moles (n) Constant Value (R) Constant Units Temperature (T) atm L mol 0.0821 K kPa 8.314 mm Hg 62.4 Always L Always mol Always weird Always K

28 PRACTICE – 1 of 3 Ideal Gas Law PV = nRT Q1: What is the pressure (in atm) exerted by a mol sample of nitrogen gas in a 10.0L container at 298K?

29 PRACTICE – 2 of 3 Ideal Gas Law PV = nRT Q2: What is the volume (in liters) of moles of oxygen gas at 20.0ºC and atm of pressure?

30 PRACTICE – 3 of 3 Ideal Gas Law PV = nRT Q3: How many moles of chlorine (Cl2) is contained in a 10.0L tank at 27.0ºC and 3.50atm of pressure?

31 Final Summary of Formulas
Boyle’s Law : P1V1 = P2V2 Charles’s Law : V1 = V2 T1 T2 Gay-Lussac’s Law : P1 = P2 Combined Gas Law : P1 V1 = P2 V2 T T2 Ideal Gas Law : PV = nRT

32 Gas Stoichiometry Same rules as Reaction Stoichiometry…
We are simply adding one value – Standard Molar Volume. The volume occupied by one mole of gas at STP (Standard Temperature and Pressure). standard molar volume = 22.4 L/mol of gas.

33 (Remember the value 22.4L/mol.)
PRACTICE – 1 of 4 Gas Stoichiometry Q1: A chemical reaction produces mol of oxygen gas. What volume (in liters) is occupied by the gas at STP? (Remember the value 22.4L/mol.)

34 (Remember the value 22.4L/mol.)
Notes on Gases PRACTICE – 2 of 4 Gas Stoichiometry Q2: A chemical reaction produced 98.0 mL of sulfur dioxide gas (SO2) at STP. What was the mass in grams of the gas produced? (Remember the value 22.4L/mol.) Chemistry - Vaughn

35 Gas Stoichiometry CaCO3  CaO + CO2
PRACTICE – 3 of 4 Gas Stoichiometry CaCO3  CaO + CO2 Q3: How many grams of calcium carbonate must be decomposed to produce 5.00L of carbon dioxide gas at STP? (Use PV=nRT)

36 WO3 (s) + 3H2 (g)  W(s) + H2O(l)
PRACTICE – 4 of 4 Gas Stoichiometry WO3 (s) + 3H2 (g)  W(s) + H2O(l) Q4: How many liters of hydrogen gas at 35.0ºC and atm are needed to react completely with 875 g of tungsten oxide? (PV=nRT)

37 2C2H2 (g) + 5O2 (g)  2H2O(g) + 4CO2(g)
CHALLENGE 2C2H2 (g) + 5O2 (g)  2H2O(g) + 4CO2(g) 425.0cm3 of acetylene fully combusts with oxygen according to the reaction above. If the reaction occurs at 25.0ºC and 375kPa, what mass of steam in kilograms will be produced? What will be the density of the steam if it occupies 75kL of space?

38 YouTube Videos – GAS HELP
1. Gas Stoichiometry #1 2. Gas Stoichiometry #2 3. Molar Volume Explanation 4. How to Collect a Gas Experimentally 5. Ideal Gas Law Example 6. Diffusion of Gas Demos 7. Effusion of Heavy Gas (Sulfur hexafluoride) 8. Effusion of Light Gas (Hydrogen) 9. Kinetic Molecular Theory of Gases 10. Properties of Gases

39 Review Topics for the Test
Properties of Gases a) Kinetic Molecular Theory (5 parts) b) Fluidity, Expansion c) Compressibility, Density d) Effusion/Diffusion e) Units for Temperature and Pressure f) STP

40 Review Topics for the Test
II. Gas Laws Boyle’s Law : P1V1 = P2V2 Charles’s Law : V1 = V2 T1 T2 Gay-Lussac’s Law : P1 = P2 Combined Gas Law : P1 V1 = P2 V2 T T2 Ideal Gas Law : PV = nRT

41 Review Topics for the Test
III. Gas Stoichiometry Converting from moles  Liters Converting from Liters  moles Converting from grams  Liters Converting from Liters  grams Using a balanced equation to predict grams or Liters by using PV=nRT

42 Remember: - Scientific Calculator - Pencil - Scratch paper - 3x5 Note Card (front/back)

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