Avogadro’s Law Hypothesis, Formula and Examples

What is Avogadro’s Law?

portrait-of-Amedeo-Avogadro
Amedeo Avogadro – founder of Avogadro’s Law Credit/Wikimedia Commons

Avogadro’s Law or Avogadro’s Hypothesis is an Ideal Gas Law that basically defines that how the volume of a gas is directly proportional to the amount of substance (moles) of gas used when pressure and temperature are held constant.

In other words, at constant temperature and pressure, of course, an equal volume of all the gases will have the same number of molecules.

This phenomenon is known as Avogadro’s Principle; named after Italian Chemist, Physicist, and Scientist Amedeo Avogadro who first hypothesized this law in 1811.

In fact, when Avogadro’s Law is substituted with Combined Gas Law (i.e the combination of Boyle’s Law, Charles’s Law, and Gay-Lussac’s Law) develops into an Ideal Gas Law. Moreover, Avogadro’s Law can be deduced from the Kinetic Molecular Theory Of Gas.

Take a look at Top 6 Real-Life Gay Lussac Law Examples

 

General Consequences and Facts About Avogadro’s Hypothesis

Not to mention, there are some general consequences and easy to remember facts about Avogadro’s Law, which you definitely want to keep in mind:

  • If the amount of substance (moles) is increased, the volume will increase. And, vice-versa.
  • Like all the other Ideal Gas Law, this Law also describes the behavior of an Ideal Gas. Yet, it can also be applied to real gases at normal temperatures and low pressure.
  • In real practice, real gases show a small deviation from the ideal gas behavior. Yet, it is still a useful tool for scientists.
  • The molar volume i.e one mole of an ideal gas occupies 22.4 Liters at STP ( i.e at  0°C and 1 atm pressure).
  • The Avogadro Number or Avogadro Constant is the number of elementary entities (atoms, molecules, or other particles) present in 1 mole of a substance; represented by NA. Mathematically, it is equal to 6.022×1023.
  • This Avogadro Number remains the same for every element; whether the lightest one i.e Hydrogen or the heaviest one i.e Uranium.

Check out, Top 6 Applications of Charles Law

 

Avogadro’s Law Formula

Mathematically, Avogadro’s Law Formula is expressed as:
 
{displaystyle {frac {V}{n}}=k,}
 
where,
 
V = Volume of the gas
n = Number of particles
k = Propotionality Constant
 
 
On the other hand, let us compare the same substance under two different conditions, then Avogadro’s gas law formula can be stated as:
 
avogadro's-law
 
where,
P1 and P2 = Pressure of the different gas
T1 and T2 = Temperature of different gas (in Kelvin)
V1 and V2 = Volume of different gas
n1 and n2 = No. of particles
 
 
The above equation shows that”an increase in the volume of a gas will be an increase in the amount of substance (moles) in proportion; and vice-versa.

 

Recommended, Top 6 Applications of Boyle’s Law

 

Avogadro’s Law Example Problem

  1. A 5 L sample at 27 °C and 3 atm contain 0.600 mol of gas. If we add 0.300 mol of gas at the same pressure and temperature. Then, what will be the final total volume of the gas?
ANS = as we know, according to Avogadro’s law equation:
 
V1 / n1 = V2 / n2
 
Where,
V1 = 5 L
n1 = 0.600 mol
n2 = 0.600 + 0.300 = 0.900 mol
V2 =?
 
now putting all the values in above equation we get,
 
5 / 0.600 = V2 / 0.900
 
on solving,
 
Hence, the final volume of the gas V2 = 7.5 Litre.

I am a mechanical engineer by profession. Just because of my love for fundamental physics, I switched my carrier, and therefore I just completed my postgraduate degree in physics. Right now I am a loner (as like ever) and a Physics blogger too. My sole future goal is to do a Ph.D. in theoretical physics, especially in the field of cosmology. Because in my view, every part of physics comes within the range of cosmology. And I love traveling, especially the Sole one.

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