Compression and Expansion of Gases
The relationship between pressure and density when compressing - or expanding - a gas depends on the nature of the process. The process can be
- isentropic (adiabatic)
Isothermal Compression/Expansion Processes
If compression or expansion of gas takes place under constant temperature conditions - the process is said to be isothermal. The isothermal process can be expressed with the Ideal Gas Law as
p / ρ = constant (1)
p = absolute pressure (Pa, N/m2)
ρ = density (kg/m3)
The isothermal process can also be expressed as
pV = constant (1a)
p1V1 = p2V2 (1b)
V = gas volume (m3, ft3...)
suffix1 denotes initial conditions and suffix2 denotes final conditions
Isentropic (or adiabatic) Compression/Expansion Processes
If compression or expansion of gas takes place with no flow of heat energy either into or out of the gas - the process is said to be isentropic or adiabatic. The isentropic (adiabatic) process can be expressed with the Ideal Gas Law as
p / ρk = constant (2)
k = cp / cv - the ratio of specific heats - the ratio of specific heat at constant pressure - cp - to the specific heat at constant volume - cv
The isentropic or adiabatic process can also be expressed as
pVk = constant (2a)
p1V1k = p2V2k (2b)
Polytropic Compression/Expansion Process
An ideal isothermal process must occur very slowly to keep the gas temperature constant. An ideal adiabatic process must occur very rapidly without any flow of energy in or out of the system. In practice most expansion and compression processes are somewhere in between, or said to be polytropic.
The polytropic process can be expressed as
pVn = constant (3a)
p1V1n = p2V2n (3b)
n = polytropic index or exponent (ranging 1 to 1.4)
• Fluid Mechanics
The study of fluids - liquids and gases. Involving velocity, pressure, density and temperature as functions of space and time.
Gases - Specific Heats and Individual Gas Constants
Specific heat at constant volume, specific heat at constant pressure, specific heat ratio and individual gas constant - R - common gases as argon, air, ether, nitrogen and many more.
The Ideal Gas Law
The relationship between volume, pressure, temperature and quantity of a gas, including definition of gas density.