2A Gas Uniformly fills any container. Mixes completely with any other gasExerts pressure on its surroundings.
3Simple barometer invented by Evangelista Torricelli
4Pressure is equal to force/unit area SI units = Newton/meter2 = 1 Pascal (Pa)1 standard atmosphere = 101,325 Pa1 standard atmosphere = 1 atm =760 mm Hg = 760 torr
5Pressure Unit Conversions The pressure of a tire is measured to be 28 psi. What would the pressure in atmospheres, torr, and pascals.(28 psi)(1.000 atm/14.69 psi) = 1.9 atm(28 psi)(1.000 atm/14.69 psi)( torr/1.000atm) = 1.4 x 103 torr(28 psi)(1.000 atm/14.69 psi)(101,325 Pa/1.000 atm) = 1.9 x 105 Pa
9Boyle’s Law* (Pressure)( Volume) = Constant (T = constant) P1V1 = P2V2 (T = constant)V 1/P (T = constant)(*Holds precisely only at very low pressures.)
10Boyle’s Law Calculations A 1.5-L sample of gaseous CCl2F2 has a pressure of 56 torr. If the pressure is changed to 150 torr, will the volume of the gas increase or decrease? What will the new volume be?DecreaseP1 = 56 torrP2 = 150 torrV1 = 1.5 LV2 = ?V1P1 = V2P2V2 = V1P1/P2V2 = (1.5 L)(56 torr)/(150 torr)V2 = 0.56 L
11Boyle’s Law Calculations In an automobile engine the initial cylinder volume is L. After the piston moves up, the volume is L. The mixture is atm, what is the final pressure?P1 = 1.00 atmP2 = ?V1 = LV2 = LV1P1 = V2P2P2 = V1P1/V2P2 = (0.725 L)(1.00 atm)/(0.075 L)P2 = 9.7 atmIs this answer reasonable?
12A gas that strictly obeys Boyle’s Law is called an ideal gas.
13Plot of PV vs. P for several gases at pressures below 1 atm.
18Charles’s Law Calculations Consider a gas with a a volume of L at 35 oC and 1 atm pressure. What is the temperature (in Co) of the gas when its volume is L at 1 atm pressure?V1 = LV2 = LT1 = 35 oC = 308 KT2 = ?V1/V2 = T1/T2T2 = T1 V2/V1T2 = (308 K)(0.535 L)/(0.675 L)T2 = 244 K -273T2 = - 29 oC
19At constant temperature and pressure, increasing the moles of a gas increases its volume.
20Avogadro’s LawFor a gas at constant temperature and pressure, the volume is directly proportional to the number of moles of gas (at low pressures).V = ana = proportionality constantV = volume of the gasn = number of moles of gas
22AVOGADRO’S LAWA 12.2 L sample containing 0.50 mol of oxygen gas, O2, at a pressure of 1.00 atm and a temperature of 25 oC is converted to ozone, O3, at the same temperature and pressure, what will be the volume of the ozone? 3 O2(g) ---> 2 O3(g)(0.50 mol O2)(2 mol O3/3 mol O2) = 0.33 mol O3V1 = 12.2 LV2 = ?n1 = 0.50 moln2 = 0.33 molV1/V2 = n1/n2V2 = V1 n2/n1V2 = (12.2 L)(0.33 mol)/(0.50 mol)V2 = 8.1 L
24COMBINED GAS LAWWhat will be the new volume of a gas under the following conditions?V1 = 3.48 LV2 = ?P1 = atmP2 = atmT1 = - 15 oC + 273= 258 KT2 = 36 oC + 273T2= 309 KV1/ V2 = P2 T1/ P1 T2V2 = V1P1T2/P2T1V2 = (309 K)(0.454 atm)(3.48 L)(258 K)(0.616 atm)V2 = 3.07 L
25Pressure exerted by a gas increases as temperature increases provided volume remains constant.
26P1 / P2 = T1 / T2 If the volume of a gas is held constant, then V1 / V2 = 1.Therefore:P1 / P2 = T1 / T2
27Ideal Gas Law An equation of state for a gas. “state” is the condition of the gas at a given time.PV = nRT
28IDEAL GAS 1. Molecules are infinitely far apart. 2. Zero attractive forces exist between the molecules.3. Molecules are infinitely small--zero molecular volume.What is an example of an ideal gas?
29REAL GAS 1. Molecules are relatively far apart compared to their size. 2. Very small attractive forces exist between molecules.3. The volume of the molecule is small compared to the distance between molecules.What is an example of a real gas?
30Ideal Gas Law PV = nRT Holds closely at P < 1 atm R = proportionality constant= L atm molP = pressure in atmV = volume in litersn = molesT = temperature in KelvinsHolds closely at P < 1 atm
31Ideal Gas Law Calculations A 1.5 mol sample of radon gas has a volume of 21.0 L at 33 oC. What is the pressure of the gas?p = ?V = 21.0 Ln = 1.5 molT = 33 oC + 273T = 306 KR = Latm/molKpV = nRTp = nRT/Vp = (1.5mol)( Latm/molK)(306K)(21.0L)p = 1.8 atm
32Ideal Gas Law Calculations A sample of hydrogen gas, H2, has a volume of 8.56 L at a temperature of O oC and a pressure of 1.5 atm. Calculate the number of moles of hydrogen present.p = 1.5 atmV = 8.56 LR = Latm/molKn = ?T = O oC + 273T = 273KpV = nRTn = pV/RTn = (1.5 atm)(8.56L)( Latm/molK)(273K)n = 0.57 mol
33Standard Temperature and Pressure “STP”P = 1 atmosphereT = CThe molar volume of an ideal gas is liters at STP
35Molar Volume pV = nRT V = nRT/p V = (1.00 mol)( Latm/molK)(273K)(1.00 atm)V = 22.4 L
36Gas Stoichiometry Not at STP (Continued) p = 1.00 atmV = ?n = 1.28 x 10-1 molR = Latm/molKT = 25 oC = 298 KpV = nRTV = nRT/pV = (1.28 x 10-1mol)( Latm/molK)(298K)(1.00 atm)V = 3.13 L O2
37Gases at STPA sample of nitrogen gas has a volume of 1.75 L at STP. How many moles of N2 are present?(1.75L N2)(1.000 mol/22.4 L) = 7.81 x 10-2 mol N2
38Gas Stoichiometry at STP Quicklime, CaO, is produced by heating calcium carbonate, CaCO3. Calculate the volume of CO2 produced at STP from the decomposition of 152 g of CaCO3. CaCO3(s) ---> CaO(s) + CO2(g)(152g CaCO3)(1 mol/100.1g)(1mol CO2/1mol CaCO3) (22.4L/1mol) = 34.1L CO2Note: This method only works when the gas is at STP!!!!!
39Volume-VolumeIf 25.0 L of hydrogen reacts with an excess of nitrogen gas, how much ammonia gas will be produced? All gases are measured at the same temperature and pressure.2N2(g) + 3H2(g) ----> 2NH3(g)(25.0 L H2)(2 mol NH3/3 mol H2) = 16.7 L NH3
40MOLAR MASS OF A GAS n = m/M n = number of moles m = mass M = molar mass
41MOLAR MASS OF A GASP = mRT/VMorP = DRT/Mtherefore:M = DRT/P
42Molar Mass Calculations M = ? d = 1.95 g/LT = 27 oC p = 1.50 atmT = 300. K R = Latm/mol KM = dRT/pM = (1.95g/L)( Latm/molK)(300.K)(1.5atm)M = 32.0 g/mol
43Dalton’s Law of Partial Pressures For a mixture of gases in a container,PTotal = P1 + P2 + P
44Dalton’s Law of Partial Pressures Calculations A mixture of nitrogen gas at a pressure of atm, oxygen at 2.55 atm, and carbon dioxide at .33 atm would have what total pressure?PTotal = P1 + P2 + P3PTotal = atm atm atmPtotal = 4.13 atm
45Water Vapor Pressure 2KClO3(s) ----> 2KCl(s) + 3O2(g) When a sample of potassium chlorate is decomposed and the oxygen produced collected by water displacement, the oxygen has a volume of L at a temperature of 22 oC. The combined pressure of the oxygen and water vapor is 754 torr (water vapor pressure at 22 oC is 21 torr). How many moles of oxygen are produced?Pox = Ptotal - PHOHPox = 754 torr - 21 torrpox = 733 torr
46MOLE FRACTION-- the ratio of the number of moles of a given component in a mixture to the total number of moles of the mixture.1 = n1/ ntotal1 = V1/ Vtotal1 = P1 / Ptotal (volume & temperature constant)
47Kinetic Molecular Theory 1. Volume of individual particles is zero.2. Collisions of particles with container walls cause pressure exerted by gas.3. Particles exert no forces on each other.4. Average kinetic energy Kelvin temperature of a gas.
48Plot of relative number of oxygen molecules with a given velocity at STP (Boltzmann Distribution).
49Plot of relative number of nitrogen molecules with a given velocity at three different temperatures.
50The Meaning of Temperature Kelvin temperature is an index of the random motions of gas particles (higher T means greater motion.)
51Diffusion: describes the mixing of gases Diffusion: describes the mixing of gases. The rate of diffusion is the rate of gas mixing.Effusion: describes the passage of gas into an evacuated chamber.