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

1 Answer
Nov 29, 2016

Answer:

You compare #CuCl_2# with #CuCl_2*2H_2O#?

Explanation:

If you have a mole each of #"copper(II) chloride"# and #"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 #"copper(II) chloride"# differs from one mole of #"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 #"copper(II) chloride"# is #134.45*g#, and that of #"copper(II) chloride dihydrate"#, #170.45*g#.