# What would be the mass of 4.5xx10^26 carbon atoms?

May 18, 2017

Well, the mass of $6.022 \times {10}^{23}$ carbon atoms is $12.011 \cdot g$.

#### Explanation:

How do we know this? Well, $6.022 \times {10}^{23}$ individual ""^12C atoms has a mass of $12.00 \cdot g$ precisely, and we use this number as a bridge between the sub-micro world of atoms and molecules to the macro world of grams, and litres, that which we can quantitatively measure.

And so.........

"Mass of carbon"=(4.5xx10^26*"carbon atoms"xx12.011*g)/(6.022xx10^23*"carbon atoms")

$\cong 9 \cdot k g$ carbon...........

May 18, 2017

We will convert to mols.

#### Explanation:

1 mol of $C$ has 6.02xx10^23 atoms (Avogadro's number).

So the number you mention contains:

$\frac{4.5 \times {10}^{26}}{6.02 \times {10}^{23}} = 0.748 \times {10}^{3} m o l$

Since 1 mol of $C$ has a mass of $12.01 g$

Total mass $= 12.01 \times 0.748 \times {10}^{3} = 8.98 \times {10}^{3} g \approx 9.0 k g$