1. How many moles of water were in your sample of copper chloride hydrate? (2*1.

Question

1. How many moles of water were in your sample of copper chloride hydrate?

(2*1.008) + 16 = 18.02g/mol mass of H2O 0.2g water * (1m/18.02g) = 0.011099m reduced to 0.01 moles of water

2. How many moles of copper were in your sample of copper chloride?

0.4g * (1m/63.55g) = 0.006294 moles of copper reduced to 0.006 moles

3. How many moles of chlorine were in your sample of copper chloride?

0.006 moles of copper * 2 for chlorine = 0.0012588 moles reduced to 0.001 moles of chlorine

4. Write the proper chemical formula for the compound that you tested.

CuCl2.2H2O How do I calculate this with my data? Did I calculate something wrong in my data of Cl?

Explanation / Answer

Your approach is absolutely correct. You have only done a small calculation mistake i.e., in calculation of chlorine. If you multiply .006294 by 2 you will get .012588 and not .0012588. Try doing it again carefully.

So , now the ratio Cu:Cl: H2O becomes .006294: .012588 : .011 which on simplifying gives 1:2:2. It's not exactly 2 for H2O but rounding off to nearest whole number gives 2. .011099/.006294=1.76 which is pretty close to 2.

Hence the formula becomes CuCl2.2H2O

If you still have any doubt, do leave a comment. I will try to clarify it.

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