Physics Test (B1-B4) Flashcards
What are the 3 types of systems?
Isolated, Open, and Closed
Isolated System
Cannot exchange thermal, energy, work or matter with its surroundings.
Open Stsrem
Can exchange thermal energy, work and matter with its surroundings.
Closed System
Can exchange thermal energy or work with its surroundings but not matter.
What kind of energy is the internal energy of an Ideal Gas?
It is all kinetic energy
The First Law of Thermodynamics
States that the change in internal energy of a system is equal to the heat added to the system minus the work done by the system.
Q symbol
Heat
U symbol
Internal Energy
Isothermal Process
Temperature remains constant
ΔU=o
Q=W
Isovolumetric Process
Volume is constant. No Work done on or by gas.
W=0
Q=ΔU
Adiabatic Process
No thermal energy is exchanged between the gas and its surroundings.
Q=0
ΔU=-W
Isobaric Process
Pressure is constant
Q=ΔU+W
Isotherms
Lines where temperature is constant along a pV diagram.
Thermodynamic Cycle
A sequence of processes which vary the pressure, volume, and temperature of a gas.
How do you find work done by a system with a thermodynamic cycle?
The enclosed area on the pV diagram equates to the work done.
Heat Engine
Converts thermal energy into mechanical energy
Thermal Efficiency η equals?
Useful Work Output / Energy Input
Entropy
A measurement of the disorder of a system. The more particles in a system move the greater the disorder.
What is Entropy’s Symbol?
S (Units: J/K)
The Second Law of Thermodynamics
At constant temperature, all thermodynamic processes are irreversible. The entropy of the universe increases with time.
Carnot Cycle
A theoretical concept for the most efficient cycle of a heat engine.
What are the 4 parts of a Carnot Cycle?
- Isothermal Expansion
-Adiabatic Expansion
-Isothermal Compression
-Adiabatic Compression
Microstate
A possible combination of microscopic properties for a thermodynamic system
Temperature
Measurement of the average Kinetic Energy per particle in a material
Thermal Equilibrium
They have if they have the same temperature
Internal Energy
Total kinetic energy of particles in a substance plus the potential energy stored in the bonds between the particles.
Specific Heat Capacity
A measurement of how many Joules of heat is required to change the temperature of 1kg of mass by 1 degree Celsius or Kelvin.
Freezing Point
0 Celsius
Boiling point
100 Celsius
Calculate Kelvin from Celsius
T=0 Celsius + 273 = Kelvin
Absolute Zero
Almost all molecular movement has stopped.
Boltzmann Constant
Links microscopic particle energies to macroscopic temperature measurements.
Thermal Conduction
KE transferred between particles
Thermal Convection
Differences in densities of liquids and gases result in their movement.
Thermal Radiation
Electromagnetic radiation is emitted by surfaces.
Thermal Conductivity (k)
Constant that represents substance’s ability to conduct thermal energy.
Black Body
Surface that absorbs all of the Infared and light
Luminosity
Total power of electromagnetic radiation emitted by a star (SI Unit: W)
Wiens Displacement Law
Related absolute temp and wavelength emitted with max power by a black body at that temp.
Calorimeter
apparatus designed for experiments investigating thermal energy transfers.
Latent Heat
Thermal energy that is transferred at constant temperature during any change of physical phase.
Solar Constan
Intensity of the suns radiation
Albedo
scatter or reflected power (total scattered power/total incident power)
Scattering
Irregular reflections of waves or particles because of matter.
Emissivity
Power radiated by an object divided by the power radiated by a black body of the same surface area and Temperature.
What are the Greenhouse gasses?
CO2, Methane (Ch4), H20, Nitrous Oxide (N20)
Pressure (P)
Force acting normally per unit area (Force/Area)
Amount of Substance (n)
n=Na (avogandros constant)/N (number of molecules)
Boyles Law
Pressure of a fixed amount of gas is inversely proportional to volume. PV=PV
Pressure law
For fixed amount of gas with constant volume.
P/T=P/T
Charles Law
V/T=V/T
What happens to gas under extreme conditions?
Real gas doesn’t function like normal
Ideal Gas
- No IMFs (so No PE)
- All collisions perfectly elastic
- volume of particles is negligible compared to volume of container.
- contains a large # of particles
- particles are moving at randoms speeds and directions
