# How do you find the number of molecules equal to 1.46 moles of CaCl_2?

Mar 20, 2017

There are $8.7892 \times {10}^{23}$ molecules in $1.46$ mols of $C a C {l}_{\text{2}}$.

#### Explanation:

The formula we are using to convert is $n = \frac{N}{N} _ \text{A}$.
=> Where $n$ is the amount of moles, in mols.
=> Where $N$ is the number of molecules.
=> Where ${N}_{\text{A}}$ is Avogadro's Number. It is a constant number of $6.02 \times {10}^{23} \text{molecules"/"mol}$.

All we have to do is rearrange our equation to give us the amount of molecules, and plug in our numbers.

$n = \frac{N}{N} _ \text{A}$

$N = n \cdot {N}_{\text{A}}$

Now we plug in our variables.

$N = n \cdot {N}_{\text{A}}$

$= 1.46 \cdot \left(6.02 \times {10}^{23}\right)$

$= 8.7892 \times {10}^{23}$

Therefore, there are $8.7892 \times {10}^{23}$ molecules in $1.46$ mols of $C a C {l}_{\text{2}}$.

Hope this helps :)