Boyle's law

Guy-Lussac's law

Avogadro's law

unit

A gas that conforms to the ideal gas equation of state (pV=nRT) at any temperature and pressure

The molecule itself does not occupy volume

No interaction between molecules

conforms to ideal gas behavior when

Generally, it can be approximately considered as an ideal gas under low pressure.

The higher the temperature and the lower the pressure, the closer it is to an ideal gas.

The ratio of the amount of substance B to the total amount of substances in the mixture

The mole fraction of a gas mixture is generally represented by y The mole fraction of a liquid mixture is generally represented by x

The ratio of the mass of substance B to the total mass of the mixture

The ratio of the volume of pure B before mixing to the sum of the volumes of each pure component

Because there is no interaction between ideal gas molecules and the molecules themselves do not occupy volume, the pVT properties of ideal gases have nothing to do with the type of gas. Therefore, some molecules of an ideal gas are replaced by molecules of another ideal gas, forming a mixed ideal gas. , its pVT property does not change, but n in the ideal gas equation of state is the total amount of matter at this time.

The sum of the products of the molar masses of each substance in a mixture and its mole fractions

Applicable conditions: real gas mixtures and ideal gas mixtures.

The total pressure of an ideal mixed gas is equal to the sum of the pressures produced when each component exists alone at T and V of the mixed gas.

Applicable conditions: ideal gas mixture

Physical meaning: In an ideal gas mixture, the partial pressure of a component is equal to the pressure when the component exists alone and has the same temperature and volume as the mixture.

The total volume V of an ideal gas mixture is the sum of the component volumes VB* of each component

Applicable conditions: ideal gas mixture

Physical meaning: The partial volume VB* of substance B in an ideal gas mixture is equal to the volume occupied by pure gas B under the conditions of the temperature and total pressure of the mixture.

It shows that the volume of an ideal gas mixture is additive. At the same temperature and pressure, the total volume after mixing is equal to the sum of the volumes of the components before mixing.

Only two B subscripts can appear

Boyle temperature is a property of matter (gas)

TB is generally 2 - 2.5 times that of Tc

Boyle temperature is high and gases tend to liquefy

Z<1: easy to compress

Z>1: difficult to compress

Z=1: ideal gas

Note: The size of the compression factor only indicates whether it is easy to compress, and has nothing to do with whether it is easy to liquefy.

Saturated vapor pressure is a unique property of pure substances and is determined by its nature

Saturated vapor pressure as a function of temperature

The saturated vapor pressure of a liquid at a constant temperature is the minimum pressure required to liquefy its vapor at that temperature

boiling point

normal boiling point

Relative humidity

1. T < Tc

2. T = Tc

3. T > Tc

The maximum temperature allowed for a gas to liquefy

Saturation vapor pressure at critical temperature The minimum pressure required to liquefy a gas at critical temperature

Volume at critical temperature and pressure

pr=p/pc, Tr=T/Tc, Vr=Vm/Vc

If two contrasting state parameters of different gases are equal to each other, the two gases are in corresponding states. When different gases are in corresponding states, certain physical properties (compression factor, fugacity coefficient, etc.) are the same or have a simple relationship