Chapter 14

Chapter 14

Thermodynamics Basics
1. Transfer of energy between systems of particles
2. Conservation of Energy is key
3. Changes in energy affects its properties
Systems
1. Particles exchange energy via collisions
2. Systems can exchange energy with other systems
3. Example: Balloon filled with Oxygen molecules
4. Properties
  1. Macroscopic
    1. Temperature
    2. Heat
    3. When comparing 2 systems, macroscopic properties as a whole will be the same
  2. Microscopic
    1. position
    2. velocity
    3. When comparing 2 systems, they may not be the same on the microscopic level
Temperature
1. Associated with "hotness" and "coldness"
2. Energy is transferred from the "hotter" system to the "colder" system
  1. Thermal equilibrium is reached when both systems have the same temperature
3. Conversions
  1. Tk = Tc + 273.15
  2. Tf = (9/5)Tc+32
  3. Tc = 5/9 (Tf-32)
4. Scales
  1. Farenheit
    1. Water freezes at 32 degrees F
    2. Water boils at 212 degrees F
  2. Celsius
    1. Water freezes at 0 degrees C
    2. Water boils at 100 degrees C
  3. Kelvin
    1. Water freezes at 273.15 K
    2. Water boils at 373.15 K
5. Lower limit is 0K, absolute zero
Heat/Heat Energy
1. Energy that flows between systems
2. Principle of Conservation of Energy
  1. the amount of energy that "leaves" system 1 must be = to the amount of energy "entering" system 2
3. Transfer depends on temp difference
4. Units of Heat
  1. SI unit = Joules
  2. 1 calorie = 4.186 J
  3. 1 Calorie = 1000 calories
Zeroth Law
1. If 2 systems (A & B) are in thermal equilibrium, and systems B & C are also in equilibrium, then A & C are in equilibrium
2. Temp is the only property of a system that will determine heat flow between it and another system

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