3 Kinetic Molecular Theory Postulate #1Gases consist of tiny particles (atoms or molecules)Postulate #2These particles are so small, compared with the distances between them, that the volume (size) of the individual particles can be assumed to be negligible (zero).Gases are COMPRESSIBLE
4 Kinetic Molecular Theory Postulate #3The particles are in constant random motion, colliding with the walls of the container. These collisions with the walls cause the pressure exerted by the gas.
5 Kinetic Molecular Theory Postulate #4The particles are assumed not to attract or to repel each other.Postulate #5The average kinetic energy of the gas particles is directly proportional to the Kelvin temperature of the gas.
6 Pressure What is pressure? How is it measured? mmHg (or Torr) Atmospheres (atm)Pascals (used in physics:1 pascal = 1 newton per square meter)4. psiEquivalences:1 atm = 760 mmHg1 atm = 101,325 Pa = kPa1 atm = 14.7 psi
7 Pressure Pressure of air is measured with a BAROMETER (developed by Torricelli in 1643)
8 Pressure Calculation What is 475 mm Hg expressed in atm? 475 mm Hg =0.625 atm760 mm Hg
9 “The Law of Partial Pressure” Dalton’s Law“The Law of Partial Pressure”The total pressure of a mixture of gases is the sum of the partial pressures of the gases in the mixture.Ptotal = PA + PB + PC
10 Temperature Scales Celsius Kelvin 100 ˚C 0 ˚C 100˚C 373 K 273 K 100 K Boiling point of water100 ˚C0 ˚C100˚C373 K273 K100 KFreezing point of waterNotice that 1 kelvin = 1 degree Celsius
11 Calculations Using Temperature ALL gas calculations require temperature in KelvinT (K) = T(˚C)Body temp = 37 ˚C = 310 KLiquid nitrogen = ˚C = 77 K
12 Relationships How are temperature and volume related? How are volume and pressure related?How are pressure and temperature related?
13 Reminders Homework: Gases WS 1 Reminders: Extra Credit Due 5/11 Test Corrections due 5/1
15 Warm UpWhen you increase the temperature in a container, do the particles of gas move faster or slower? Would this increase or decrease the pressure?What would happen if you put a balloon in the freezer?What would happen if you put a balloon in the oven?Is it possible to compress a gas?
16 DemoPut a few drops of water in a can. Heat the can until the water boils. What is happening to the gas inside?Now flip the can over into cold water. Predict what do you predict will happen?
17 On a Larger ScaleThe most common (and commonly collapsed) railcar is the DOT 111A100 class or commonly called a "general purpose" tank car. These cars are rated to a test pressure of 100 psig and a minimum burst pressure of 500 psig. Minimum carbon steel plate thickness is 7/16 inch. For a 23,000 gallon car, the tank length is about 55 feet. For comparison purposes the "heaviest" pressure car commonly used is a 105J500, rated to a test pressure of 500 psig and a minimum burst of 1250 psig. They are made of 1 inch thick, high-strength steel plate.
20 PV=nRT P = pressure ( atm or kPa ) V= volume ( L ) The Gas LawPV=nRTP = pressure ( atm or kPa )V= volume ( L )n= number of moles (mol)T= temperature (K)
21 R – The Proportionality Constant Value depends on units8.314L (kPa)mol (K)0.0821L (atm)OrR is the proportionality constantBasically once scientists got the gas laws figured out, they put them all together but realized that the variables behaved according to this proportionality constant.Your value of R, like anything else, will vary depending on the units.Can’t add apples to oranges – If you have 3 apples and 5 oranges how many apples do you have? Because you can’t add apples to oranges. So to add them together you would need to convert to fruit for both and then add them together.
22 The Gas Law – Problem PV = nRT P = 1454.95 kPa P = 1500 kPa If 7.0 moles of an ideal gas has a volume of 12.0 L with a temperature of 300. K, what is the pressure in kPa?PV = nRTP (12.0 L)=(7.0 mol)(300 K)8.314L (kPa)mol (K)Using the Ideal Gas Law work through this problem with your neighbor.P = kPaP = 1500 kPa
23 The Gas Law – Problem 9.95 atm PV = nRT If 4.00 moles of a gas has a volume of 10.0 L with a temperature of 303. K, what is the pressure in atm?PV = nRTP (10.0 L)=(4.00 mol)(303 K)0.0821L (kPa)mol (K)Using the Ideal Gas Law work through this problem with your neighbor.9.95 atm
24 Combined Gas LawLet’s say we have a balloon full of O2 gas AND we change some conditions. Would there be anything similar between the two gases?
25 Combined Gas Law – Problem You have 3.0 moles of a solution at 300. K and 15 atm in a 2.0 L container. If the container is heated to 350. K and the volume decreased to 1.0 L, what will the new pressure be?P115 atmP2wantV12.0 LV21.0 Ln13.0 molesn2R1constantR2T1300. KT2350. KWork through this problem with your neighbor.What did everyone get?35 atm, correctLet’s see how you got that:All work is on the powerpoint (click mouse)
26 Combined Gas Law – Problemc P1V1=n1R1T1P2V2n2R2T2If we know that R1 = R2 and the mass is constant thenP1V1=T1P2V2T2Replace with numbers(15 atm)(2.0 L)=(300. K)P2(1.0L)(350. K)
27 Combined Gas Law – Problem (15 atm)(2.0 L)=(300. K)P2(1.0 L)(350. K)(15 atm)(2.0 L)(350. K)=P2(1.0L)(300. K)P2 = 35 atm
28 P1V1 = P2V2 Pressure & Volume At constant Temperature Pressure and Volume vary inversely.Why?More collisions More pressureP1V1 = P2V2P1V1=n1R1T1P2V2n2R2T2Smaller volume means particles have shorter distance to go to hit the sides of the container.
29 P & V – Example Problem 1.0 atm = P2 If you start with L of a gas at 7.0 atm and you move the gas to a container with 3.5 L available, how much pressure will the gas exert?P1 (V1) = P2 (V2)7.0 atm (0.500 L) = P2 (3.5 L)Work through this problem with your neighbor.What did everyone get?1.0 atm, correctLet’s see how you got that:All work is on the powerpoint (click mouse)7.0 atm (0.500 L)=P23.5 L1.0 atm = P2
30 V1 = V2 T1 T2 Temperature & Volume At constant Pressure Volume & Temperature vary directly.Why?More collisions More VolumeP1V1=n1R1T1P2V2n2R2T2Heating a gas will make it expand.ROOT BEER DEMOAlso relate back to gases expanding to take up all space available.V1=V2T1T2
31 T & V – Example ProblemIf a gas is in a balloon with a volume of 12.0 L and at a temperature of 300. K, what will the volume be if you place the balloon in a freezer at 250. K?V1=V2T1T212.0 L300. K250. K12.0 L (250. K)10.0 LWork through this problem with your neighbor.What did everyone get?10.0 L, correctLet’s see how you got that:All work is on the powerpoint (click mouse)
32 S.T.P.Standard Temperature and PressureThese are conditions that are universalStandard Temperature:0ºC or KStandard Pressure:1atm or kPa
33 S.T.P. – Example Problem PV = nRT V= 22.4 L What is the volume of 1 mole of a gas at STP?P1 atmVwantn1 moleR(L)(atm)/(K)(mole)T273 KPV = nRT(1atm)V = (1 mole)( [Latm/Kmole])(273K)V= 22.4 L
34 Practice ProblemsThe pressure of a sample of gas is 5.00 atm and the volume is 30.0 L. If the volume is changed to 50.0 L, what is the new pressure?
35 Practice ProblemsA sample of gas has a volume of 50.0 L at a temperature of 300.K. What temperature would be needed for this sample to have a volume of 60.0 L if its pressure remains constant?
36 Practice ProblemsA 3.68g sample of a certain diatomic gas occupies a volume of 3.00 L at 1.00 atm and a temperature of 45°C. Identify this gas.
50 Warm UpA sample of gas is in a 13.0 L container with 1.26 atm of pressure on it at 23.5 ˚C. How many moles of gas are in the sample?If the gas in the problem above is released from its container into a 56.0 L container but the temperature remains constant, what will the new pressure be?
51 DemosHow does atmospheric pressure affect gas particles?
52 RemindersHomework: Study for your test Reminders: Extra Credit Due 5/11 Gases Test 5/7 or 5/8