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Chapter 10 Kinetic Theory of Matter

Chapter 10 Kinetic Theory of Matter. Objectives. 10.1 Compare characteristics of a solid, liquid, and gas. 10.1 Relate the properties of a solid, liquid, and gas to the kinetic theory of matter 10.1 Distinguish among an amorphous material, liquid crystal, and plasma. Objectives.

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Chapter 10 Kinetic Theory of Matter

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  1. Chapter 10 Kinetic Theory of Matter

  2. Objectives • 10.1Compare characteristics of a solid, liquid, and gas. • 10.1 Relate the properties of a solid, liquid, and gas to the kinetic theory of matter • 10.1 Distinguish among an amorphous material, liquid crystal, and plasma

  3. Objectives • 10.2Interpret changes in temperature and changes of state of a substance in terms of the kinetic theory of matter • 10.2 Relate Kelvin and Celsius scale • 10.2 Analyze the effects of temperature and pressure on state changes • 10.2 Identify and understand types of intermolecular forces (LDF, Dipole-Dipole, Induced dipole) for molecules

  4. Solid Liquid Gas Revisited • Solid: Fixed atomic position • Liquid/Gas: No fixed atomic position • Solid/Liquid: Atoms and molecules hold onto one another • Ideal Gas: No attraction at all for each other

  5. Same Temperature means Same Kinetic Energy • All matter is in random and constant motion. • Not all matter or molecules within the same state of matter move at the same speed • The heavier a molecule is, the smaller its speed • Heavier gases diffuse slower than light gases • Heavier solid atoms jiggle less than lighter solids

  6. Other States of Matter • Liquid Crystals • When some solids melt, they don’t melt in all dimensions, remain a solid in at least one dimension. Some keep their shape in one of the three dimensions. These can then be manipulated by electric charge

  7. Other States of Matter • Amorphous Materials • Have an incomplete, or random crystal lattice. • Examples include peanut butter, glass (when heated), cotton candy, pudding • Distinction can be difficult, many everyday objects you would consider solid could be classified in this way • If it is a mixture of solids/liquids (hard to tell), it is amorphous

  8. Other States of Matter • Plasmas • Ionized gas • Most common in universe, not on earth • Occurs in stars

  9. Temperature and Particle Motion

  10. Same Temperature, Different Gases

  11. Temperature Scales • Three Scales: Kelvins, Celsius, Fahrenheit • Kelvins Absolute Temperature Scale, it has a value of 0 at absolute 0 • Important to use an absolute temperature scale in many calculations otherwise you would find negative volumes of air as well as other unfortunate mistypes in the calculator • Absolute Zero: All molecules have zero kinetic energy

  12. Temperature Scales • Celsius  Has same slope as Kelvins, just starts below it 273 degrees. • Water freezes at 0 C and boils at 100 C, convenient • Fahrenheit  The American scale, based on ability to detect temperature change • Equation above is black, but should be green

  13. Quick Questions • If the temperature of the room is at equilibrium, which state of matter in this room has the most kinetic average per particle? • Can an individual molecule touch absolute zero? Defend your rationale. • 373 Kelvin is what temperature Celsius?

  14. Diffusion/Effusion • Diffusion • Process of gas molecules spreading out due to random motion • Effusion • Process of gas molecules escaping through a tiny opening (why balloons go flat) • What goes flat faster: Helium or Normal filled balloon?

  15. Distillation • Technique used to separate mixtures based on difference in boiling points • Example: If water and another liquid are mixed, if you boil them, the one with a lower boiling point evaporates first until it is all gone before temperature rises again

  16. Temperature is an Average • Therefore, some molecules are able to evaporate or melt before the temperature reaches that point • Some water evaporates (boils) before 100 C

  17. Changes of States • Solid to Liquid  Melting • Solid to Gas  Sublimation • Dry Ice and Moth Balls • Liquid to Gas  Evaporation • Gas to Liquid  Condensation • Gas to Solid  Deposition • Frost • Liquid to Solid  Freezing

  18. Vapor Pressure • How much of a liquid evaporates? • That is vapor pressure • The liquid molecules which turn to gas exert a pressure (as a gas does). • The warmer it gets, the more that evaporates, the larger the pressure • Polar molecules = Lower Vapor pressures • Have a difficult time escaping from one another

  19. Vapor Pressure • As the temperature increases (for the liquid), the vapor pressure increases as more and more of the liquid can evaporate

  20. How much heat to evaporate? • Heat of Vaporization: Energy required to make a substance evaporate • Also energy released when condensing • Heat of Fusion: Energy required to make a substance melt • Also energy released when freezing

  21. Lots of energy to evaporate • Why we feel cold after being in the pool

  22. Some Math • How much energy will it take to melt 1.0 gram of ice? Heat of fusion for water is 334 J/g • If you have 200 grams of water that the ice melts in, what is the temperature change of the water? The specific heat of water is 4.18 J/g

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