Gases are fluids that have no shape or volume of their own, their shape and size will depend on the container where they are stored.
This is because gas molecules are separated from each other.
Index
At gas laws were created by three different physicists and chemists. This happened in the 17th and 19th century; are they:
In these laws, the properties of volume, pressure and temperature of gases were studied.
Ideal gases or perfect gases are models that were designed to facilitate the study of gases. the three gas laws show the behavior of perfect gases has constant properties, while two others are constant.
Characteristics of ideal gases:
The law created by physicist and chemist Robert Boyle shows an isothermal transformation.
Where the temperature of the gases remains constant, while the gas volume and pressure are proportional but inversely.
P.V = K or P = K/V
P = sample pressure
V = volume
K = temperature constant (depending on the nature of the gas, temperature and mass)
This law created by also French physicist and chemist Joseph Louis Gay – Lussac showing a isobaric transformation of gases when gas pressure is constant, temperature and volume are proportional:
V = K.T or K = V/T
V = gas volume
T = temperature
K = pressure constant (isobaric)
See also: wind energy
Created by the French physicist and chemist Jacques Alexandre César Charles, it presents an isometric or isochoric transformation of perfect gases.
Here the gas volume is constant and the pressure and temperature are proportional:
P = K.T or K = P/T
P = pressure
T = temperature
K = volume constant (depending on the nature, volume and mass of the gas)
I recommend: Newton's Laws
The Claperyron equation was devised by the French chemist and physicist Benoit Paul Émile Clapeyron. This study unites the three properties of gases: temperature, pressure and volume:
PV = n. RT
P = pressure
V = volume
no = number of moles
R = universal constant of perfect gases = 8.31 J/mol. K
T = temperature
This equation is used for gases that have a constant mass, which would be number of moles, and variation of some of the quantities that are pressure, temperature and volume:
K = P.V/T or P1.V1/T1 = P2.V2/T2
P = pressure
V = volume
T = temperature
K = molar constant
P1 = initial pressure
V1 = initial volume
T1 = initial temperature
P2 = final pressure
V2 = final volume
T2 = final temperature
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