Avogadro’s Constant

Mole carbon relationship

Avogadro's Constant and Mole relationship

The mole is used in measurements similar to the “dozens”.

  • The reason why we use moles in chemistry is because of the vast number of molecules and atoms involved in the calculations.
  • The number is huge and unimaginable, a bit like the number of stars in the galaxy.
  • Using the mole unit helps simplify calculations.
  • So instead of having to write 6.02 × 10^23 number of particles or atoms, you could write 1 mole of particles or atoms instead.

1 mole of atoms

How many atoms in 1 mole

The Mole Shop

The mole sop - avogadro's number

The mole shop showing Avogadro's number

Mole to represent a very large number

Avogadro's constant and the mole

The mole is equal to 602 thousand billion billion!

Avogadro Mole in a limousine
1 mole = 602,000,000,000,000,000,000,000.

AMADEO AVOGADRO

Avogadro Amedeo
By From a drawing by C. Sentier, executed in Torino at Litografia Doyen in 1856. (Edgar Fahs Smith collection) [Public domain], via Wikimedia Commons

Amadeo Avogadro was an Italian physicist who was honored for his contribution for his molecular hypothesis in the gas law. The concept of the mole was introduced long after his death.

 

The mole is a representation of the number which happens to be the same number of atoms found in 12 grams of carbon.

The AVOGRADRO CONSTANT is a very important number in physics and chemistry and you will see it pops up frequently. It’s important to memorize this number (6.022 x 1023) so you can easily recall it for your calculations.

 

 

Mole to Mole Comparison

It is important to know that 1 mole represents the same number but not the same mass.

items total number of items

in 1 mole

total mass in

1 mole

H
6.022 x 1023 H atoms
1.008 g
H2
6.022 x 1023 H2 molecules
2.016 g
H2O
6.022 x 1023 H2O molecules
18.016 g

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