The Kinetic-Molecular Theory of Matter
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Transcript of The Kinetic-Molecular Theory of Matter
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The Kinetic-Molecular The Kinetic-Molecular Theory of MatterTheory of Matter
Objective 2.05Objective 2.05
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Ideal GasesIdeal Gases
►An An imaginaryimaginary gas that perfectly fits all gas that perfectly fits all the assumptions about kinetic the assumptions about kinetic molecular theorymolecular theory
►Kinetic Molecular Theory of Gases Kinetic Molecular Theory of Gases (KMT)(KMT) explains the properties of gasesexplains the properties of gases
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Kinetic-Molecular Theory of Kinetic-Molecular Theory of GasesGases
►Assumptions about Ideal GasesAssumptions about Ideal Gases particles are spread far apartparticles are spread far apart mostly empty spacemostly empty space Collisions are elastic collisions Collisions are elastic collisions Particles are in continuous, random Particles are in continuous, random
motionmotion no forces of attraction or repulsion no forces of attraction or repulsion average kinetic-energy = temperatureaverage kinetic-energy = temperature
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However…….However…….
►Real Gases Real Gases Do not follow KMT completelyDo not follow KMT completely But we can use the KMT to describe themBut we can use the KMT to describe them How they differ:How they differ:
►Occupy spaceOccupy space►Particles ARE attracted to each other (to some Particles ARE attracted to each other (to some
degree)degree)►Nonpolar gases deviate less than polar gasesNonpolar gases deviate less than polar gases
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Nature of gases explained by Nature of gases explained by KMTKMT
► ExpansionExpansion► FluidityFluidity► Low DensityLow Density► CompressibilityCompressibility►Diffusion Diffusion
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Units of pressureUnits of pressure
►Mm of HgMm of Hg►TorrTorr►Atmospheres (atm)Atmospheres (atm)►Kilopascals (kPa)Kilopascals (kPa)
►Pressure Unit ConversionsPressure Unit Conversions 1 atm = 760 mmHg = 760 torr = 101.3 1 atm = 760 mmHg = 760 torr = 101.3
kPakPa
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Units of TemperatureUnits of Temperature
►Celsius (˚C)Celsius (˚C)►Kelvin (K)Kelvin (K)
K = ˚C + 273K = ˚C + 273
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Standard temperature and Standard temperature and pressurepressure
(STP)(STP)►1 atm…OR1 atm…OR
760 mm Hg760 mm Hg 760 torr760 torr 101.3 kPa101.3 kPa
►273 K (0273 K (0° C)° C)
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The Gas LawsThe Gas Laws
►Combined Gas LawCombined Gas Law
PP11VV1 1 = P= P22VV22
TT11 T T22
Used to determine pressure, Used to determine pressure, temperature or volume of a gas temperature or volume of a gas
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Examples of Gas Problems using Examples of Gas Problems using Combined Gas LawCombined Gas Law
►Pg. 315 Sample Problem 10-2Pg. 315 Sample Problem 10-2►Pg. 318 Sample Problem 10-3Pg. 318 Sample Problem 10-3►Pg. 320 Sample Problem 10-4Pg. 320 Sample Problem 10-4►Pg. 321 Sample Problem 10-5Pg. 321 Sample Problem 10-5
►Remember T must be in Kelvin!Remember T must be in Kelvin!►Remember P units must be all the same!Remember P units must be all the same!►Whichever unit is constant cancels out!!!Whichever unit is constant cancels out!!!
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The Gas LawsThe Gas Laws
►Boyles Law:Boyles Law:
►Charles Law: Charles Law:
►Gay Lussac’s LawGay Lussac’s Law
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Ideal Gas LawIdeal Gas Law
►Mathematical relationship among Mathematical relationship among pressure, volume, temperature, and pressure, volume, temperature, and the the number of molesnumber of moles of a gas of a gas
►PV=nRTPV=nRT (given on Reference Guide)(given on Reference Guide)
Pressure (P)Pressure (P) Volume (V)Volume (V) Number of moles (n)Number of moles (n) Ideal gas constant (get from table on Ideal gas constant (get from table on
sheets)sheets) Temperature (T) Temperature (T)
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Examples of Ideal Gas Examples of Ideal Gas ProblemsProblems
►Pg. 342 Sample Problem 11-3Pg. 342 Sample Problem 11-3►Pg. 343 Sample Problem 11-4Pg. 343 Sample Problem 11-4►Pg. 344 Sample Problems 11-5Pg. 344 Sample Problems 11-5
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Dalton’s Law of Partial Dalton’s Law of Partial PressuresPressures
►The total pressure of a mixture of The total pressure of a mixture of gases is equal to the sum of the partial gases is equal to the sum of the partial pressures of the component gasespressures of the component gases
►PPTT=P=P11+P+P22+P+P33+… +… (given on reference guide)(given on reference guide)
►Also…for gas collected over waterAlso…for gas collected over water PPT T = P= Pgasgas + P + PH2OH2O
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Example of Partial Pressures Example of Partial Pressures ProblemProblem
►Pg. 324 Sample Problem 10-6Pg. 324 Sample Problem 10-6
►To get water pressure use To get water pressure use ►Water Vapor Pressure Table Appendix A pg Water Vapor Pressure Table Appendix A pg
899899
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Avogadro’s Law for GasesAvogadro’s Law for Gases
►Gases of the same volume, at the Gases of the same volume, at the same temp and pressure, have the same temp and pressure, have the same number of molecules!same number of molecules!
►n/V = n/Vn/V = n/V►A mole ratio in an equation can A mole ratio in an equation can
become a VOLUME ratio when all become a VOLUME ratio when all compounds are gasescompounds are gases
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Example of Avogadro’s LawExample of Avogadro’s Law
HH22 (g)(g) + Cl + Cl22 (g)(g) 2HCl 2HCl (g)(g)
Mole Ratio: 1 mol:1mol:2molMole Ratio: 1 mol:1mol:2mol
Volume Ratio: 1L : 1L :2LVolume Ratio: 1L : 1L :2L
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Molar Volume of A GasMolar Volume of A Gas
►At STPAt STP
1 mole of any gas = 22.4 L1 mole of any gas = 22.4 L
New Branch on Mole MapNew Branch on Mole Map