Gas Laws

Boyle-Mariotte: At constant temperature, the volume of a given mass of an ideal gas is inversely proportional to the pressure to which it is subjected; consequently, the product of pressure and its volume is constant.
P₁V₁ = P₂V₂

APPLICATION EXAMPLE:

In an experiment an ideal gas with 25 m³ volume and pressure of 1.5 atm, it was subjected to a pressure of 4 atm, keeping it at a constant temperature. What volume will it occupy?
Since the temperature remains constant and we know the P₁, P₂ and V₁, we have to:

V₂= P₁V₁/ P₂

V₂= (1.5 atm) (25 m³) / 4 atm = 9.37 m³

Charles: At constant pressure, the volume of a given mass of an ideal gas increases by 1/273 relative to its volume at 0 ° C for every ° C its temperature rises. Similarly, it contracts by 1/273 with respect to its volume at 0 ° C for every degree ° C that its temperature drops, provided that the pressure remains constant, that is:

V_total= V₀(1 + 1 / 273T) = V₀/273(273+T)=k₁T

p = constant
k₁= constant

From this it follows that: k₁= k₂

V₁/ k₁T₁= V₂/ k₂T₂ therefore V₁/ T₁= V₂/ T₂

Gay-Lussac: At constant volume, the pressure of a given mass of an ideal gas increases 1/273 with respect to its pressure at 0 ° C for every ° C that increases or decreases its temperature, as long as its volume remains constant.

P_total= P₀(1 + 1 / 273T) = P₀/273(273+T)=P₀/273(273+T)k₁T

V = constant
From this it follows that: k₁= k₂

P₁/ K₁T₁= P₂/ K₂T₂ therefore P₁/ T₁= P₂/ T₂