2Gas PropertiesFour properties determine the physical behavior of any gas:Amount of gasGas pressureGas volumeGas temperature
3Gas pressureGas molecules exert a force on the walls of their container when they collide with it
4Gas pressure Gas pressure can support a column of liquid Pliquid = g•h•dg = acceleration due to the force of gravity (constant)h = height of the liquid columnd = density of the liquid
5Standard atmospheric pressure (1 atm) is 760 mm Hg Torricelli barometerIn the closed tube, the liquid falls until the pressure exerted by the column of liquid just balances the pressure exerted by the atmosphere.Patmosphere = Pliquid = ghdPatmosphere liquid heightStandard atmospheric pressure (1 atm) is 760 mm Hg
6Units for pressureIn this course we usually convert to atm
7Gas pressure Pliquid = g•h•d Pressure exerted by a column of liquid is proportional to the height of the column and the density of the liquidContainer shape and volume do not affect pressure
8ExampleA barometer filled with perchloroethylene (d = 1.62 g/cm3) has a liquid height of 6.38 m. What is this pressure in mm Hg (d = 13.6 g/cm3)?P = ghd = g hpce dpce = g hHg dHghpce dpce = hHg dHghHg = hpce d pce = (6.38 m)(1.62 g/cm3) = m dHg g/cm3hHg = 760 mm Hg
9Gas pressureA manometer compares the pressure of a gas in a container to the atmospheric pressure
10Gas Laws: BoyleIn 1662, Robert Boyle discovered the first of the simple gas lawsPV = constantFor a fixed amount of gas at constant temperature, gas pressure and gas volume are inversely proportional
11Examples 6-3A & 6-3BA cylinder contains a gas at 5.25 atm pressure. When the gas is allowed to expand to a final volume of 12.5 L, the pressure drops to 1.85 atm. What was the original volume of the gas?1.50 L of gas at 2.25 atm pressure expands to a final volume of 8.10 L. What is the final gas pressure in mm Hg?
12Gas Laws: CharlesIn 1787, Jacques Charles discovered a relationship between gas volume and gas temperature:• relationship between volumeand temperature is always linear• all gases reach V = 0 at sametemperature, – °Cvolume (mL)• this temperature isABSOLUTE ZEROtemperature (°C)
13A temperature scale for gases: the Kelvin scale A new temperature scale was invented: the Kelvin or absolute temperature scaleK = °CZero Kelvins = absolute zero
14Gas laws: Charles Using the Kelvin scale, Charles’ results is For a fixed amount of gas at constant pressure, gas volume and gas temperature are directly proportionalA similar relationship was found for pressure and temperature:
15Examples 6-4A & 6-4BA gas at 25 °C and atm is heated under a piston. The volume expands from L to 1.65 L. What is the new temperature of the gas, if pressure has remained constant?If an aerosol can contains a gas at 1.82 atm at 22 °C, what will be the gas pressure in the can in an incinerator at 935 °C?
16Standard conditions for gases Certain conditions of pressure and temperature have been chosen as standard conditions for gasesStandard temperature is K (0 °C)Standard pressure is exactly 1 atm (760 mm Hg)These conditions are referred to as STP (standard temperature and pressure)
17Gas laws: AvogadroIn 1811, Avogadro proposed that equal volumes of gases at the same temperature and pressure contain equal numbers of particles.At constant temperature and pressure, gas volume is directly proportional to the number of moles of gasStandard molar volume: at STP, one mole of gas occupies 22.4 L
18Examples 6-6A & 6-6BA small tank of propane is opened and releases 30.0 L of gas at STP. What mass of propane was released?128 g of dry ice sublimes into CO2 gas. What is the volume of this gas at STP?
19Putting it all together: Ideal Gas Equation Combining Boyle’s Law, Charles’ Law, and Avogadro’s Law give one equation that includes all four gas variables:R is the ideal or universal gas constantR = atm L/mol K
20Using the Ideal Gas Equation Ideal gas equation may be expressed two ways:One set of conditions: ideal gas lawTwo sets of conditions: general gas equation
21ExamplesWhat is the volume occupied by 20.2 g NH3 gas at –25 °C and 752 mm Hg?How many moles of He gas are in a 5.00 L tank at 10.5 atm pressure and 30.0 °C?A 1.00 mL sample of N2 gas at 36.2 °C and 2.14 atm is heated to 37.8 °C while the pressure is changed to 1.02 atm. What volume does the gas occupy at this temperature and pressure?
22Ideal Gas Equation and molar mass Solving for molar mass (M)
23ExampleA glass vessel weighs g when clean, dry, and evacuated. When filled with an unknown gas at 772 mm Hg and 22.4 °C, the vessel weighs g. What is the molar mass of the gas?1.27 g of an oxide of nitrogen (believed to be either NO or N2O) occupies 1.07 L at 25 °C and 737 mm Hg. Which oxide is it?
25Gas densityGas density depends directly on pressure and inversely on temperatureGas density is directly proportional to molar mass
26ExamplesWhat is the density of helium gas at 298 K and atm? Why can we say He is lighter than air?Hint: what is the average molar mass of air, which is 78.08% N2, 20.95% O2, 0.93% Ar, and 0.036% CO2?At what temperature will the density of O2 gas be 1.00 g/L if the pressure is kept at 745 mm Hg?
27Mixtures of Gases Ideal gas law applies to pure gases and to mixtures In a gas mixture, each gas occupies the entire container volume, at its own pressureThe pressure contributed by a gas in a mixture is the partial pressure of that gasPtotal = PA + PB (Dalton’s Law of Partial Pressures)
28Mixtures of GasesWhen a gas is collected over water, it is always “wet” (mixed with water vapor).Ptotal = Pbarometric = Pgas + Pwater vaporExample: If 35.5 mL of H2 are collected over water at 26 °C and a barometric pressure of 755 mm Hg, what is the pressure of the H2 gas? The water vapor pressure at 26 °C is 25.2 mm Hg.
29Gas mixturesThe mole fraction represents the contribution of each gas to the total number of moles.XA = mole fraction of A
30Gas mixturesThe mole fraction represents the contribution of each gas to the total number of moles.XA = mole fraction of AThe pressure fraction is equal to the mole fraction
31Gas mixtures The volume composition of a gas mixture is Avogadro’s hypothesis: at constant T & P, gas V is proportional to moles of gasThe volume percent gives the mole fraction
32Gas Mixtures For gas mixtures, mole fraction equals pressure fraction Each gas occupiesthe entire container.The volume fraction describesthe % composition by volume.mole fractionequalspressure fractionvolume fraction
33ExamplesWhat is the total gas pressure in a mixture of 1.0 g H2, 5.00 g He, and 12.5 g Ne, in a 5.0 L container at 55 °C?A mixture of mol CO2 and mol H2O gas are held at 30.0 °C and 2.50 atm. What is the partial pressure of each gas in the mixture?Air is 78.08% N2, 20.95% O2, 0.93% Ar, and 0.036% CO2 by volume. What is the partial pressure of each gas at a barometric pressure of 748 mm Hg?
34Gases in Chemical Reactions To convert gas volume into moles for stoichiometry, use the ideal gas equation:If both substances in the problem are gases, at the same T and P, gas volume ratios = mole ratios.P2 = P1 and T2 = T1
35ExamplesHow many grams of NaN3 will produce 20.2 L N2 at 30.0 °C and 776 mm Hg? NaN3 (s) 2 Na(l) N2 (g)What volume of O2 is consumed per liter of NO formed, at constant temperature and pressure: 4 NH3 (g) O2 (g) 4 NO (g) + 6 H2O (g)
36A Model for Gas Behavior Gas laws describe what gases do, but not why.Kinetic Molecular Theory of Gases (KMT) is the model that explains gas behavior.developed by Maxwell & Boltzmann in the mid-1800sbased on the concept of an ideal or perfect gas
37Ideal gasComposed of tiny particles in constant, random, straight-line motionGas molecules are point masses, so gas volume is just the empty space between the moleculesMolecules collide with each other and with the walls of their containerThe molecules are completely independent of each other, with no attractive or repulsive forces between them.Individual molecules may gain or lose energy during collisions, but the total energy of the gas sample depends only on the absolute temperature.
38Molecular collisions and pressure Force of molecular collisions depends oncollision frequencymolecule kinetic energy, ekek depends on molecule mass m and molecule speed umolecules move at various speeds in all directions
39Molecular speed Molecules move at various speeds Imagine 3 cars going 40 mph, 50 mph, and 60 mphMean speed = u = ( ) ÷ 3 = 50 mphMean square speed (average of speeds squared) u2 = ( ) ÷ 3 = m2/hr2Root mean square speed urms = √2567 m2/hr2 = mph
41The basic equation of KMT Combining collision frequency, molecule kinetic energy, and the distribution of molecule speeds gives the basic equation of KMTP = gas pressure and V = gas volumeN = number of moleculesm = molecule massu2 = mean square molecule speed (average of speeds squared)
42Combine the Equations of KMT and Ideal Gas If n = 1,N = NAandPV = RTAvogadro’s number
43Combine the Equations of KMT and Ideal Gas NA x m (Avogadro’s number x mass of one molecule)= mass of one mole of molecules (molar mass M)
44Combine the Equations of KMT and Ideal Gas We can calculate the root mean square speedfrom temperature and molar mass
45Calculating root mean square speed To calculate root mean square speed from temperature and molar mass:Units must agree!Speed is in m/s, soR must be J/mol KM must be in kg per mole, because Joule = kg m2 / s2Speed is inversely related to molar mass: light molecules are faster, heavy molecules are slower
46Example 6-17AWhich has the greater root mean square speed at 25 °C, NH3 gas or HCl gas? Calculate urms for the one with greater speed.
47Interpreting temperature Combine the KMT and ideal gas equations againAgain assume n=1, so N = NA and PV = RT
48Interpreting temperature Absolute (Kelvin) temperature is directly proportional to average molecular kinetic energyAt T = 0, ek = 0
49Diffusion and Effusion Diffusion (a) is migration or mixing due to random molecular motionEffusion (b) is escape of gas molecules through a tiny hole
50Rates of diffusion/effusion The rate of diffusion or effusion is directly proportional to molecular speed:The rates of diffusion/effusion of two different gases are inversely proportional to the square roots of their molar masses (Graham’s Law)
51Using Graham’s LawGraham’s Law applies to relative rates, speeds, amounts of gas effused in a given time, or distances traveled in a given time.
52Using Graham’s Law with times Graham’s law can be confusing when applied to timesrate = amount of gas (n)time (t)
53Use common sense with Graham’s Law When you compare two gases, the lighter gasescapes at a greater ratehas a greater root mean square speedcan effuse a larger amount in a given timecan travel farther in a given timeneeds less time for a given amount to escape or travelMake sure your answer reflects this reality!
54Examples2.2 x 10–4 mol N2 effuses through a tiny hole in 105 seconds. How much O2 effuses through the same hole in the same time?How long would it take for 2.2 x 10–4 mol H2 to effuse through the same hole as the 2.2 x 10–4 mol N2, which effused in 105 seconds?
55ExamplesA sample of Kr gas escapes through a tiny hole in 87.3 sec. Under the same conditions, the same amount of unknown gas effuses in sec. What is the molar mass of the unknown gas?How long would it take for the same amount of ethane gas to effuse, under the same conditions as the Kr gas in problem A?
56Reality Check Ideal gas molecules Real gas molecules constant, random, same straight-line motionpoint masses are NOT points – molecules have volume; Vreal gas > Videal gasindependent of each other are NOT independent – molecules are attracted to each other, so Preal gas < Pideal gasgain / lose energy during same (some energy may be collisions, but total energy absorbed in molecular depends only on T (ek) )
57Real gas corrections For a real gas, a corrects for attractions between gas molecules, which tend to decrease the force and/or frequency of collisions (so Preal < Pideal)b corrects for the actual volume of each gas molecule, which increases the amount of space the gas occupies (so Vreal > Videal)The values of a and b depend on the type of gas
58An equation for real gases: the van der Waals equation Add correction to Preal to make it equal to Pideal,because intermolecular attractions decrease real pressureSubtract correction to Vreal to make it equal to Videal,because molecular volume increases real volume
59When do I need the van der Waals equation? Deviations from ideality become significant whenmolecules are close together (high pressure)molecules are slow (low temperature)At low pressure and high temperature, real gases tend to behave ideallyAt high pressure and low temperature, real gases do not tend to behave ideally}non-idealconditions
60Example 6-20ACalculate the pressure exerted by 1.00 mol CO2 when confined to a volume of 2.00 L at 273 K. aCO2 = 3.59 L2atm/mol2 and bCO2 = L/mol. Which shows a greater departure from ideality, CO2 or Cl2 (aCl2 = 6.49 and bCl2 =0.0562, same units)?
61Examples 6-18 & 6-19A2.2 x 10–4 mole of N2 gas effuses through a pinhole in 105 s. How much O2 effuses through the same hole in that amount of time?How long would it take for 2.2 x 10–4 mol H2 to effuse through the same hole?A sample of Kr gas escapes through a pinhole in 87.3 s. Gas X requires s for the same amount to escape. What is the molar mass of X?
62Exercise 28A gas is collected over water when the barometric pressure is mm Hg, but the water level inside the container of gas is 4.5 cm higher than outside. What is the total pressure of the gas inside the container, in mm Hg?
63Exercise 29A 35.8-L cylinder of Ar gas is connected to an evacuated 1875-L tank. If the temperature is held constant and the final pressure is 721 mm Hg, what must have been the original gas pressure in the cylinder, in atm?
64Exercise 31A fixed amount of gas held at a constant volume of 275 mL exerts a pressure of 798 mm Hg at 23.4 °C. At what temperature in °C will the pressure of the gas become exactly 1.00 atm?
65Exercise 33 A 27.6 mL sample of PH3 gas is obtained at STP. a. What is the mass of this gas, in mg?b. How many molecules of PH3 are present?
66Exercise 37A 12.8 L cylinder contains 35.8 g O2 at 46 °C. What is the pressure of this gas, in atm?
67Exercise 42A 10.0 g-sample of a gas has a volume of 5.25 L at 25 °C and 762 mm Hg. If to this constant volume is added 2.5 g of the same gas, and the temperature raised to 62 °C, what is the new gas pressure?
68Exercise 44A g sample of a gaseous compound occupies 428 mL at 24.3 °C and 742 mm Hg. The compound consists of 15.5% C, 23.0% Cl , and 61.5% F, by mass. What is its molecular formula?
69Exercise 49In order for a gas-filled balloon to rise in air, the density of the gas in the balloon must be less than that of air.a. Consider air to have a molar mass of g/mol. Determine the density of air at 25 °C and 1 atm, in g/L.b. Show by calculation that a balloon filled with carbon dioxide at 25 °C and 1 atm would not be expected to rise in air at 25 °C.
70Exercise 56A 3.57-g sample of a KCl-KClO3 mixture is decomposed by heating and produces 119 mL O2 measured at 22.4 °C and 738 mm Hg. What is the mass percent of KClO3 in the mixture? KClO3 (s) KCl (s) + O2 (g)Hint: the KCl is unchanged
71Exercise 61A mixture of 4.0 g H2 and 10.0 g He gases in a 4.3 L flask is maintained at 0 °C.a. What is the total pressure in the container?b. What is the partial pressure of each gas?
72Exercise 64A typical producer gas has this composition by volume: 8.0% CO2, 23.2% CO, 17.7% H2, 1.1% CH4, and 50.5% N2.a. What is the density of this gas mixture at 23 °C and 763 mm Hg, in g/L?b. What is the partial pressure of CO in this mixture at STP?
73Exercise 68A g sample of He gas is found to occupy a volume of L when collected over hexane at 25.0 °C and mm Hg barometric pressure. Determine the vapor pressure of hexane at 25 °C from these data.
74Exercise 75If mol N2O gas effuses through an orifice in a certain period of time, how much NO2 gas would effuse in the same time under the same conditions?
75Exercise 76A sample of N2 gas effuses through a tiny hole in 38 s. What must be the molar mass of a gas that requires 64 s to effuse under identical conditions?
76Exercise 79Use the van der Waals equation to calculate the pressure exerted by 1.50 mol SO2 gas when it is confined to a volume of 5.00 L at 298 K. For SO2, a = 6.71 L2 atm/mol2 and b = L/mol. Compare this real pressure to what you would predict assuming SO2 to be an ideal gas.
77Exercise 87A 3.05-g sample of solid NH4NO3 is placed in an evacuated 2.18-L flask and heated to 250 °C. What is the total gas pressure in atm in the flask at 250 °C after the solid has completely decomposed: NH4NO3 (s) N2O (g) H2O (g)
78Exercise 92What is the apparent molar mass of air, given that it is 78.08% N2, 20.95% O2, 0.93% Ar, and 0.036% CO2 by volume?