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The Kinetic-Molecular Theory of Matter

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Title: The Kinetic-Molecular Theory of Matter


1
The Kinetic-Molecular Theory of Matter
  • Objective 2.05

2
Ideal Gases
  • An imaginary gas that perfectly fits all the
    assumptions about kinetic molecular theory
  • Kinetic Molecular Theory of Gases (KMT)
  • explains the properties of gases

3
Kinetic-Molecular Theory of Gases
  • Assumptions about Ideal Gases
  • particles are spread far apart
  • mostly empty space
  • Collisions are elastic collisions
  • Particles are in continuous, random motion
  • no forces of attraction or repulsion
  • average kinetic-energy temperature

4
However.
  • Real Gases
  • Do not follow KMT completely
  • But we can use the KMT to describe them
  • How they differ
  • Occupy space
  • Particles ARE attracted to each other (to some
    degree)
  • Nonpolar gases deviate less than polar gases

5
Nature of gases explained by KMT
  • Expansion
  • Fluidity
  • Low Density
  • Compressibility
  • Diffusion

6
Units of pressure
  • Mm of Hg
  • Torr
  • Atmospheres (atm)
  • Kilopascals (kPa)
  • Pressure Unit Conversions
  • 1 atm 760 mmHg 760 torr 101.3 kPa

7
Units of Temperature
  • Celsius (C)
  • Kelvin (K)
  • K C 273

8
Standard temperature and pressure(STP)
  • 1 atmOR
  • 760 mm Hg
  • 760 torr
  • 101.3 kPa
  • 273 K (0 C)

9
The Gas Laws
  • Combined Gas Law
  • P1V1 P2V2
  • T1 T2
  • Used to determine pressure, temperature or volume
    of a gas

10
Examples of Gas Problems using Combined Gas Law
  • Pg. 315 Sample Problem 10-2
  • Pg. 318 Sample Problem 10-3
  • Pg. 320 Sample Problem 10-4
  • Pg. 321 Sample Problem 10-5
  • Remember T must be in Kelvin!
  • Remember P units must be all the same!
  • Whichever unit is constant cancels out!!!

11
The Gas Laws
  • Boyles Law
  • Charles Law
  • Gay Lussacs Law

12
Ideal Gas Law
  • Mathematical relationship among pressure, volume,
    temperature, and the number of moles of a gas
  • PVnRT (given on Reference Guide)
  • Pressure (P)
  • Volume (V)
  • Number of moles (n)
  • Ideal gas constant (get from table on sheets)
  • Temperature (T)

13
Examples of Ideal Gas Problems
  • Pg. 342 Sample Problem 11-3
  • Pg. 343 Sample Problem 11-4
  • Pg. 344 Sample Problems 11-5

14
Daltons Law of Partial Pressures
  • The total pressure of a mixture of gases is equal
    to the sum of the partial pressures of the
    component gases
  • PTP1P2P3 (given on reference guide)
  • Alsofor gas collected over water
  • PT Pgas PH2O

15
Example of Partial Pressures Problem
  • Pg. 324 Sample Problem 10-6
  • To get water pressure use
  • Water Vapor Pressure Table Appendix A pg 899

16
Avogadros Law for Gases
  • Gases of the same volume, at the same temp and
    pressure, have the same number of molecules!
  • n/V n/V
  • A mole ratio in an equation can become a VOLUME
    ratio when all compounds are gases

17
Example of Avogadros Law
  • H2 (g) Cl2 (g) ? 2HCl (g)
  • Mole Ratio 1 mol1mol2mol
  • Volume Ratio 1L 1L 2L

18
Molar Volume of A Gas
  • At STP
  • 1 mole of any gas 22.4 L
  • New Branch on Mole Map
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