This is a mind map about gases. It mainly talks about knowledge points related to gases. Gases are one of the four basic states of matter (the other three are solid, liquid, and plasma).
Microscopic model of gas molecular motion (particle, uniform, elastic collision)
Statistical concepts of pressure and temperature
Pressure Statistical Concept - Root Mean Square Rate
Temperature: the zeroth law of thermodynamics; the translational kinetic energy of molecules is parallel to temperature, the intensity of random movement of a large number of molecules
empirical laws
B-M: constant temperature, quantitative gas pV=C
C-G-L: Constant pressure, quantitative gas Vt=C'T
A: Same temperature, same pressure, same volume, various gases N1=N2
Ideal gas equation of state: high temperature and low pressure; kB=R/L Boltzmann constant
Partial pressure law, partial volume law
Quantitative relationship between Et and T
M rate distribution
Distribution function
Statistical averages of rates: root mean square rate, most probable rate, mathematical mean rate
Distribution of molecular translational kinetic energy
M-like rate distribution formula; two-dimensional space E2/E1 (ratio of molecules with energy higher than E2 to molecules with energy higher than E1
Molecular collision frequency and mean free path
z', z: collision between molecules, related to the reaction rate; z'': collision between molecules and the wall, related to the pressure
Molecular gap flow va/va=(Ma/Mb)1/2
real gas
Compression factor: TB Boyle temperature, the slope of the isotherm is 0, and gases above this temperature are not easily compressible
Van der Waals equation: correction of internal pressure and molecule’s own volume, TB=a/Rb
Critical state: The first-order and second-order partial derivatives of Van's gas p with respect to v are both 0