why 6.023*10^23 is taken as avogadro number and how it came into existance
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Scientists wanted an easy way to do calculations in Chemistry because it dealt with small quantities like mass of an atom or huge quantities like no of atoms in one gram of Hydrogen. Therefore Mole Concept was introduced.
They first decided to take a standard mass.
It was called Atomic Mass Unit or Amu.
1 Amu is equal to 1/12 of mass of one atom of C(12) Isotope.
Since C has 12 nucleons, it give mass of one nuceon.
Its value is 1.66 x 10 ^ -24 grams
Now if you think of it,
you can get mass of any atom by multiplying no of nucleons to the amu.
Now the scientists wanted to find no of atoms in 12 g Carbon (You will realise why) . So,
Amu x No of nucleons x No Of Atoms = Mass
Amu x 12 x No Of Atoms = 12g
No of Atoms in 12g Carbon 1g/amu
= Avagadro No.
= 6.022 x 10^23
So a collection of 6.022 x 10^23 was called a Mole.
Hope that clear your doubts
They first decided to take a standard mass.
It was called Atomic Mass Unit or Amu.
1 Amu is equal to 1/12 of mass of one atom of C(12) Isotope.
Since C has 12 nucleons, it give mass of one nuceon.
Its value is 1.66 x 10 ^ -24 grams
Now if you think of it,
you can get mass of any atom by multiplying no of nucleons to the amu.
Now the scientists wanted to find no of atoms in 12 g Carbon (You will realise why) . So,
Amu x No of nucleons x No Of Atoms = Mass
Amu x 12 x No Of Atoms = 12g
No of Atoms in 12g Carbon 1g/amu
= Avagadro No.
= 6.022 x 10^23
So a collection of 6.022 x 10^23 was called a Mole.
Hope that clear your doubts
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