AP Phys B Test Review Thermodynamics 4/30/2008
Overview Thermodynamics
• Heat, Temperature, Energy • Thermal Expansion • Ideal Gas Law • PV Diagrams • Laws of Thermodynamics
Internal Energy and Heat Internal
Energy: consists of the kinetic and potential energy of the molecular components of a system (i.e. molecular translation, rotation, vibration and bonds). Heat: The transfer of energy between systems as a result of a temperature difference.
Temperature Macroscopic:
How “how” or “cold”
something is
• Microscopic: related to the motion of the atoms of a system
Measured
in Celsius (relative) or Kelvin (absolute) scales.
• Absolute zero.
Thermal Expansion of Solids
When a “linear” object’s temperature increases, it’s physical dimensions will typically increase.
∆ L = αL 0 ∆ T •
Coefficient of linear expansion
For a truly 3-d object, there is a volume expansion with increasing temperature
∆V = βV 0∆T
Ideal Gas Law PV=nRT
(wimpy chemistry version) PV=Nk T (buff physics version) B
• K : Boltsmann constant B
‘nuff
said.
Kinetic Theory of Gases
The number of molecules is large, and the average separation between gas molecules is large The molecules obey Newton’s Laws of Motion The molecules undergo completely elastic collisions with each other and with the walls
•
No other interactions
All the gas molecules are identical Note: this allows us to interpret the ideal gas law in terms of microscopic objects!
Kinetic Theory of gases
Pressure is proportional to the number of molecules per unit volume and their average translational kinetic energy Temperature of a gas is a direct measure of the average kinetic energy of the molecules of the gas.
•
For a monatomic gas, the internal energy is:
3 U = NkBT 2
Specific Heat
The specific heat of a substance is the amount of heat energy it takes to cause in increase or decrease in temperature.
Q = m c∆T • •
c = specific heat, different for every substance Calorimetry: measuring specific heat by using heat transfer.
Latent Heat
Latent Heat is defined as the amount of energy it takes to induce a phase change in a substance.
Q = m L •
L = latent heat, varies with phase and substance.
Latent Heat and Specific Heat
Temperature Conduction Thermal
conduction
• Contact • Radiative • Convection
Zeroth Law of Thermodynamics If
objects A and B are separately in thermal equilibrium with a third object C, then A and B are in thermal equilibrium with one another.
• Two objects in thermal equilibrium with each other are at the same temperature.
First Law of Thermodynamics
The change in the internal energy of a system is equal to the heat added to the system minus the work done by the system on its environment
∆U = Q − W • •
If work is done on the system, W is negative. A piston is a good example of this.
Thermodynamic Processes
Isothermal: Constant temperature
•
Isobaric: constant pressure
•
P = constant
Isovolumetric: constant volume
•
PV = constant
V = constant
Adiabatic: No heat flows into or out of the system
•
Q=0
Thermodynamic Processes Isothermal
Process
Isobaric and Isovolumetric Processes
Adiabatic Processes
Thermodynamic Processes
Work done is given by the following:
W = P∆V • • • •
Isothermal, ∆U=0, and Q=-W Isobaric: W=P∆V, Q= ∆U+ P∆V Isovolumetric, W=0 and ∆U=Q Adiabatic, Q=0 so ∆U=W
Second Law of Thermodynamics
In any closed system, the total entropy must be increasing.
Q ∆S = T
Heat can flow spontaneously from a hot object to a cold object, but not vice versa
Heat Engines Mechanical
Energy obtained from thermal energy when heat is allowed to flow from a hot reservoir to a cold reservoir.
• First law is critically important here.
Heat Engines
Efficiency of a heat engine is defined as
Q H − Q L Q L W e = = = 1 − Q H Q H Q H
For the Carnot cycle (see next slide)
TH − TL TL e = = 1 − TH TH
Carnot Cycle The
most efficient process theoretically possible (not realistic). No device will have an efficiency equal to or greater than a Carnot engine.
Third Law of Thermodynamics It
is impossible to achieve absolute zero in a real physical system.