# How much will 1.2 * 10^46 atoms of carbon weigh?

Mar 30, 2018

$2.4 \cdot {10}^{23} \setminus \text{g}$

#### Explanation:

A carbon atom has an average mass of $12.0107 \setminus \text{amu}$. Also, one mole of carbon atoms have a mass of $12.0107 \setminus \text{g}$.

Recall that one mole of atoms is $6.02 \cdot {10}^{23}$ atoms.

So here, we got:

(1.2*10^46color(red)cancelcolor(black)"atoms")/(6.02*10^23color(red)cancelcolor(black)"atoms""/mol")~~2*10^22 \ "mol"

And so, the total mass will be

$2 \cdot {10}^{22} \textcolor{red}{\cancel{\textcolor{b l a c k}{\text{mol"*(12.0107 \ "g")/(color(red)cancelcolor(black)"mol")=2.4*10^23 \ "g}}}}$