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MindMap Gallery Gases, solids and liquids
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Gases, solids and liquids
This is a mind map about gases, solids and liquids, including 1. Temperature and temperature scale, 2. Gases, 4. Liquids, 3. Solids, crystals and amorphous crystals, etc.
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Gases, solids and liquids
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Gases, solids and liquids
1. Temperature and temperature scale
State parameters and equilibrium state
thermodynamic system
To study the thermal properties of gases in a container, the research object is a system composed of a large number of molecules in the container
state parameters
definition
Some physical quantities are needed to determine the state of the system
example
Geometric parameter volume V
Determine the spatial scope of the system
Mechanical parameter pressure p
Determine the role of forces between the outside world and the system or between parts within the system
Thermal parameter temperature T
Determine how hot or cold the system is
equilibrium state
In the absence of external influences, as long as a long enough time passes, the state parameters of each part of the system can reach a stable state. This state is called an equilibrium state.
Thermal balance and temperature
Thermal equilibrium
The two systems should be in contact to transfer heat, and the state parameters of the two systems will affect each other and change respectively.
After a period of time, the respective state parameters no longer change, indicating that the two systems have reached equilibrium.
thermal equilibrium law
If two systems are each in thermal equilibrium with a third system, then the two systems must also be in thermal equilibrium with each other.
temperature
When two systems are in thermal equilibrium, they must have some common thermal properties
The physical quantity that characterizes this "common thermal property"
Thermometer and temperature scale
temperature scale
To describe temperature quantitatively, there must be a method
thermodynamic temperature
The temperature represented by the thermodynamic temperature scale
symbol
T
unit
Kelvin (open) K
2. Gas
Isothermal changes in gases
Isothermal changes in gases
The relationship between the pressure and volume of a certain mass of gas when the temperature remains constant
Boyle-Marriott's law
When the temperature of a certain mass of a certain gas remains constant, the pressure p is inversely proportional to the volume V
formula
pV=C (C is a constant)
p1V1=p2V2
Isobaric changes in gases
Isobaric changes in gases
The process by which the volume of a certain mass of a certain gas changes with temperature when the pressure remains constant.
Gay-Lussac's law
When the pressure of a certain mass of a certain gas remains constant, its volume V is directly proportional to the thermodynamic temperature T.
formula
V=CT
V1/T1=V2/T2
isovolumetric change of gas
isovolumetric change of gas
The process by which the pressure of a certain mass of a certain gas changes with temperature when the volume remains constant.
Charlie's Law
For a certain mass of a certain gas, when the volume remains constant, the pressure p is proportional to the thermodynamic temperature T
formula
p=CT
p1/T1=p2/T2
ideal gas
Gas Requirements for Experimental Gas Laws
The pressure is not too high
The pressure does not exceed several times the atmospheric pressure
The temperature is not too low
The temperature is not lower than tens of degrees Celsius below zero
ideal gas
Molecular size and interaction force can be ignored, and the kinetic energy loss of gas molecules colliding with the wall can also be ignored.
Follow the experimental laws of gases at any temperature and pressure
Microscopic Interpretation of Experimental Laws of Gases
Boyle's Law
For an ideal gas of a certain mass, when the temperature remains constant, the average kinetic energy of the molecules is constant. In this case, when the volume decreases, the number density of molecules increases, and the number of molecules that collide with the wall of the device per unit time and unit area increases, and the pressure of the gas increases. .
Gay-Lussac's law
When the temperature of a certain ideal gas of a certain mass increases, the average kinetic energy of the molecules increases; only when the volume of the gas increases simultaneously and the number density of the molecules decreases can the pressure remain unchanged.
Charlie's Law
For a certain mass of an ideal gas, when the volume remains constant, the number density of molecules remains constant. In this case, when the temperature increases, the average kinetic energy of the molecules increases, and the pressure of the gas increases.
Equation of state of ideal gas
4.Liquid
surface tension of liquid
In the surface layer, the molecules are relatively sparse, the distance r between molecules is slightly larger than r0, and the force between molecules appears as gravity.
It exists in all directions within the liquid surface layer. The direction of the force is always tangent to the liquid surface and perpendicular to the interface.
Infiltration and non-infiltration
infiltration
reason
The interaction between a liquid and the solid it comes into contact with is stronger than the interaction between liquid molecules
Phenomenon
A liquid that wets a solid and adheres to its surface
No infiltration
reason
The interaction between the liquid and the solid it came into contact with is weaker than the interaction between the liquid molecules
Phenomenon
A liquid will not wet a solid and will not adhere to the surface of the solid.
capillarity
The phenomenon of rising liquid in a thin tube of wetting liquid and the falling phenomenon of non-wetting liquid in a straw
application
To preserve underground water, we must loosen the soil on the ground and destroy the capillaries of the soil.
liquid crystal
constitute
Organic molecules are mostly rod-shaped, with the rod length being more than 5 times the diameter of the rod.
nature
fluidity of liquid
fixed arrangement of crystal molecules
Liquid crystals with molecular alignment have optical anisotropy
application
Life science field, etc.
3.Solid
Crystalline and amorphous
Can be converted into each other
crystal
example
Quartz, mica, alum, salt, copper sulfate, monosodium glutamate, snowflakes, etc.
Natural and regular geometric shapes
Has a fixed melting point
Anisotropic
Amorphous
example
Glass, wind wax, rosin, asphalt, rubber, etc.
irregular appearance
no fixed melting point
Homosexuality
Polycrystalline
example
Candy sticks stuck together
irregular appearance
Has a fixed melting point
isotropic
crystal microstructure
diamond crystal structure