Basic definition
Gas is a state of matter. Gas is fluid like liquid: it can flow and deform. Unlike liquids, gases can be compressed. If there is no restriction (container or force field), the gas can diffuse and its volume is not restricted. The atoms or molecules of a gaseous substance can move freely with each other. The kinetic energy of atoms or molecules of gaseous substances is relatively high.
The gas form can be affected by its volume, temperature and pressure. These elements constitute a number of gas laws, and the three can influence each other:
Boyle’s Law
At a certain temperature, when the volume of gas increases, its The pressure must be small. This can be expressed by the following formula: pv=K
here
V refers to the volume of gas P refers to the pressure k as a constant
Charlie’s law
When the pressure remains constant, the gas volume is proportional to its temperature. That is, as the temperature of the gas increases, its volume also increases. Its mathematical expression is:
1.V1/T1=V2/T2
2. For the thermodynamic temperature scale, V/T=C (C is a fixed value), indicating The volume of an ideal gas with a constant mass and pressure is proportional to the thermodynamic temperature.
Ideal gas
Ideal gas is an imaginary gas. Its characteristics are:
There is no force between gas molecules. The gas molecules themselves do not occupy the volume. Complete elastic collision occurs between the gas molecules and the container wall. The real gas is in the state of lower pressure and higher temperature, and its properties are closer to ideal gas. . The gas closest to the ideal gas is helium.