If I have 6.022xx10^23 individual ""^1H atoms, what MASS do I have?

Jun 8, 2015

Approx, $1 \cdot g$....why?

Explanation:

$\text{If I have 12 eggs, then how many dozen eggs do I have?}$

$\text{If I have 24 eggs, then how many dozen?}$

A $\text{bakers' dozen}$ is 13 rolls, and a $\text{Botany Bay dozen}$ is 25 lashes. If you are following me, I propose that the mole is the $\text{chemists' dozen}$. So, if I have 6.022 x ${10}^{23}$ hydrogen atoms, I have 1 g of hydrogen atoms or 1 mol. Likewise, if I have 2 g hydrogen gas (i.e. hydrogen as the diatomic molecule) I have 1 mol hydrogen gas and 2 mol hydrogen atoms. It is worth getting your head around this, 6.022 x ${10}^{23}$ defines a mole of stuff, it could be atoms or molecules (or something else). The atomic weights given on the periodic table define a mole or Avogadro's number of atoms.

So in effect the mole (or Avogadro's number) defines the link between the micro world of atoms and molecules, with the macro world of grams and kilograms. It is simply a very large number. It is vital that you understand this link, and if I've been unclear, let me know.