MindMap Gallery kinetic theory of gases
The kinetic theory of gases reveals the microscopic nature of macroscopic thermal phenomena and laws of gases by finding the relationship between macroscopic quantities and microscopic quantities. From the perspective of molecular motion, statistical methods are used to study the macroscopic properties and change patterns of thermal motion of gas molecules.
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This is a mind map about bacteria, and its main contents include: overview, morphology, types, structure, reproduction, distribution, application, and expansion. The summary is comprehensive and meticulous, suitable as review materials.
This is a mind map about plant asexual reproduction, and its main contents include: concept, spore reproduction, vegetative reproduction, tissue culture, and buds. The summary is comprehensive and meticulous, suitable as review materials.
This is a mind map about the reproductive development of animals, and its main contents include: insects, frogs, birds, sexual reproduction, and asexual reproduction. The summary is comprehensive and meticulous, suitable as review materials.
kinetic theory of gases
Basic concepts of molecular motion
Macroscopic objects are composed of a large number of particles (molecules, atoms, etc.). The molecules in the object are constantly undergoing disordered thermal motion.
Avogadro's number
There are interactions between molecules
The subtle nature of temperature
A sign of the intensity of thermal motion of molecules inside an object
equipartition theorem of energy
For an ideal gas with coverage D in equilibrium, the average kinetic energy of each degree of freedom of the molecule is equal and equal to kT/2
The average auxiliary energy of a molecule with i degrees of freedom is ikT/2
internal energy of ideal gas
The internal energy of an ideal gas is the sum of all forms of kinetic energy of all molecules and the potential energy between atoms within the molecules. For a given ideal gas, its internal energy depends only on temperature.
If vibration energy is not considered, the internal energy of an ideal gas with mass m is
ideal gas pressure formula
The pressure of a gas is caused by a large number of molecules constantly exerting force on the wall when they collide with the wall. It is a statistical average quantity.
Maxwell's law of rate distribution
Rate distribution function of molecules of an ideal gas in equilibrium
Ratio of the number of molecules distributed over a rate interval
Three statistical averages of molecular speed
average rate
square root rate
most probable rate
Boltzmann distribution rate
Molecules in a potential field always preferentially occupy states with lower potential energy.
The pressure of gas in the gravity field decreases exponentially with height
mean free path
The average distance a molecule moves between two consecutive collisions is called the mean free path
The principle of entropy increase
Boltzmann's principle
Ω is the total microstate number of the system
All processes that occur in an isolated system that is not affected by external energy proceed from a macro state with a small probability (a small number of micro states) to a macro state with a high probability (a large number of micro states).
The entropy of an isolated system never decreases