Introduction to universal gas law
Gases were the first of the phases is used to measure the quantitative measurements.In the second half of the seventeenth century,Boyle did experiments with the behaviour of gases with respect to change in volume He inferred that the pressure and the volume are inversely proportional to each other at constant temperature.The same can be represented as under
P =1/V at constant temperature
P=k/V
Where k is proportionality constant.
PV=K
This is called as Boyle's law.
The scientific reason behind this relationship is that as the voume increases,the moleculees of the gas thereby reduce the number of collisions on the walls of the container,and hence exert less pressure.The vice mversa too holds true.
Charles law
Charles gave the relationship between pressure and temperature at constant volume.He prooved that the pressure of a gas is directly proportionl to the temperature.
P T
P=kT
Where k is proportionality constant.
This is called as Charle's law. These were later used to find the universal gas constant.
Universal Gas Law Equation
In the course of time ,attempts were made to further corelate both these relationships.PV=k Boyle's law.
P/T=k Charle's law.
From the above it can be derived that
PV/T=k
If the same relationship is applied to other sets,then
P1V1/T1=k =P2V2/T2
This was called as Universal gas law equation as it gave universal relationship of pressure,temperature and volume.
Significance of Universal Gas Law Equation
Universal gas law helps to find out any missing information in the equation.If pressure,temperature at two points and the volume at one point is known,then the volume at second point could be found out. e.g.If the pressure,temperature at two points and the volume at one point is 1atm ,2atm,200 K,300K and 2 L,then the volume at second point would be
P1V1/T1=k =P2V2/T2
1 x 2/200= 2 x V2/300
V2=1 x 2 x300/200 x 2
=1.5 L
Avagadro's Law:
Avagadro's law is an elementary law that relate the quantity of gas with the volume of the gas. The law states " Equal volume of all gases under identical conditions of temperature and pressure contain equal number of molecules". Therefore, the number of molecules in a specific volume of gas is independent of the size or mass of the gas molecules. MathematicallyV = n k
where, V = the volume of the gas,
n = amount of substance of the gas (number of moles)
k = Proportionality constant.
One mole of an ideal gas occupies 22.414 litres at standard temperature and pressure.
Here is an example that represent the use of Avagadro's law (avogadro's law problem):
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