mole vs molecule – Difference between mole and molecule
Keywords covered in this post are are mole or mol, molecule, gram mole, g mol, gram mol, molar mass . While studying the chapter on gas laws you must have come across the term ‘mole’ or ‘mol‘. You may have seen gram-mol as well in that chapter. I find many students confused with mole (or mol) and molecule. Here we will discuss and explain the concept of mole or mol with some examples. This will help you to understand the difference between mole and molecule.
One mole (also abbreviated as mol) is the amount of substance that contains a specific number of particles ( 6.023 X 1023). These particles may be atoms or molecules or ions etc.
So if we say 1 mol of Oxygen gas, then that means an amount of Oxygen sample which contains 6.023 X 1023 number of Oxygen molecules. Similarly 1 mol of atomic Carbon contains 6.023 X 1023 number of Carbon atoms.
This specific number (6.023 X 1023 ) is called Avogadro number.
Gram mole: representation of molar mass in gram
1 gram mole of Oxygen gas: In this case we have to count the molecular mass of Oxygen( O2 = 2X16)and add the gram unit with it to get the mass of 1 gram mole Oxygen. So 1 gram mole Oxygen gas means 32 grams of Oxygen gas.
Now 1 gram mole atomic Carbon: In this case we have to get the atomic mass of Carbon(C = 1X12) and again add the gram unit with it. So 1 gram mole atomic Carbon means 12 gram Carbon.
Similarly 1 gram mole water(H2O) means 2X1+16 that is 18 gram of water molecules.
So we can say that 32 grams of Oxygen gas will contain Avogadro number of Oxygen molecules. Similarly 12 grams of atomic Carbon contains Avogadro number of Carbon atoms.And 18 gram of water molecules will contain Avogadro number of water molecules. Remember that (6.023 X 1023 ) is called Avogadro number.
Will provide more examples in the next post.