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Kinetic Theory of Matter

Kinetic Theory of Matter. MARCH 21 st 2013. Energy Types. Electrical / Magnetic (light, magnetic fields) Chemical (food, batteries) Thermal (heat) Nuclear (fission, fusion) Kinetic (motion) Potential (resting, stored up).

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Kinetic Theory of Matter

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  1. Kinetic Theory of Matter MARCH 21st 2013

  2. Energy Types • Electrical / Magnetic (light, magnetic fields) • Chemical (food, batteries) • Thermal (heat) • Nuclear (fission, fusion) • Kinetic (motion) • Potential (resting, stored up)

  3. Kinetic Energy is entire objects travelling in a particular direction. Thermal Energy measures how each and every atom is wiggling or bouncing randomly all the time. KE vs. TE

  4. Temperature vs. Energy Distribution Temperature measures the AVERAGE kinetic energy. Molecules will follow a distribution surrounding the average related to a STANDARD DEVIATION.

  5. States of Matter Match the diagram above with the description below. *Plasma has enough Thermal Energy to separate electrons from the nucleus. **Atoms have insignificant volume and undergo elastic collisions.

  6. Solids • Packed tightly together. • Held in place by chemical bonds. • ‘Vibrate’ in place. • May be crystalline in structure. • May take multiple forms (allotropes)

  7. Liquids • Tend to stick to similar molecules (Surface tension due to intermolecular forces). • ‘Wiggle’ and move around so long as touching other molecules. • Have a vapor pressure which is positively correlated to temperature. • Vapor pressures are the equilibrium between liquid and gas within a closed system at a certain temperature.

  8. Gases • Moves freely with or without contact from other atoms. • ‘Bounces’ around in-between walls of container. • Molecules are moving the fastest. • Collisions w/ container cause pressure. • Atmospheric pressure is defined as: • 1 atm • 760mm Hg • 101.3 kPa • Plasma is a special gas where e- get removed from their orbits and go free. Examples: lightning, fluorescent lights, stars • Subject to forces from electric and magnetic fields. Plasma

  9. Phase Changes Less Energy More Energy Colder Hotter Sublimating Melting Evaporating Ionizing Boiling Vaporization Solid Liquid Gas Plasma Freezing Condensing De-Ionizing Fusion De-sublimating

  10. Phase Diagram

  11. Vapor Pressures

  12. Heat Transfer • Radiation: The hot object ‘glows’ (visibly or invisibly) and energy leaves as light, or photons. • Example: campfire, toaster oven, microwave, laser • 2) Conduction: High-speed atoms (hot) hit touching atoms like bumper cars, and transfer their momentum and thermal energy directly. • Example: ice-cubes, stove -> skillet -> food, hot pavement -> feet • 3) Convection: High-speed atoms spread out and mix with cooler atoms, increasing the overall average energy. • Examples: HVAC, hot and cold water spigots, hair dryer

  13. Physics of Heating Latent Heat (L) is the amount of energy required to cause a phase change. Equation: Q = m L Units: Q = heat in Joules, m = mass in grams, L = Latent heat in J/g Specific Heat Capacity (C) defines how much temperature is affected by heating within a particular phase. Equation: Q = m C ∆T Units: same, C = specific heat capacity in J/(g *K)

  14. Starter Gas Laws Charles’ Law V1 / T1 = V2 / T2 when P stays the same Boyle’s Law P1 V1 = P2 V2 when T stays the same Gay-Lussac’s Law P1 / T1 = P2 / T2 when V stays the same

  15. Ideal Gas Law P V = n R T P = pressure V = volume n = number of moles (groups of 6.02 * 1023 atoms or molecules) R = 8.31 L*kPa/(mol *K) called the universal gas constant T = temperature in Kelvin Measure in kPa for pressure, Liters for volume, moles for n, and Kelvin for temperature.

  16. Guided Practice Problems • If I have a jar of air at 293 *K which has a pressure of 10 Pascals, and I place it in boiling water and let it reach thermal equilibrium, what will the new pressure be (assuming it does not expand)? • If I have a balloon at sea level, which I carry up a mountain until it is twice the size, what do I know about the air pressure at that elevation on the mountain? • A motor piston has a pressure of 100,000 Pa on both sides before the fuel ignites. Then the fuel temperature on one side goes from 293* K to 373* K. • What does the pressure on the hot side do? • What is the net pressure on the piston? • If the piston has an area of .1 m2, what is the force? • 4) How much volume will 4g of H2 occupy at 400*K and 1.5 atm?

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