# How do you calculate the moles of copper(II) chloride from the moles of copper(II) chloride dihydrate?

You compare $C u C {l}_{2}$ with $C u C {l}_{2} \cdot 2 {H}_{2} O$?
If you have a mole each of $\text{copper(II) chloride}$ and $\text{copper(II) chloride dihydrate}$, then, CLEARLY, you have the same quantities, the same numbers, of copper and chlorine atoms. If you don't appreciate this, tell us, and someone here will help you.
One mole of $\text{copper(II) chloride}$ differs from one mole of $\text{copper(II) chloride dihydrate}$ in that the latter has 2 moles of water tacked on. The dihydrate is a pale, sky blue solid; the anhydrous form is a beige solid.
The mass of one mole of $\text{copper(II) chloride}$ is $134.45 \cdot g$, and that of $\text{copper(II) chloride dihydrate}$, $170.45 \cdot g$.