Question

The Cu2+ ions in this experiment are produced by the reaction of 1.0g of copper.

Information already found out

.016 mol Cu2+ produced

Overall reaction is
Cu2+(aq)+Cl-(aq)+Cu(s)=2 CuCl(s)

Maximum mass of CuCl that can be prepared from the reaction sequence of this experiment using 1.00g of Cu turnings to prepare the Cu2+ solution is 3.1679 g CuCl




A sample of the compound prepared in this experiment, weighing .1021g, is dissolved in HNO3 and diluted to a volume of 100mL. A 10mL aliquot of that solution is mixed with 10mL 6 M NH3. The [Cu(NH3)4 2+] in the resulting solution is 5.16x10^-3 M.

How many moles of Cu were in the original sample, which had been effectively diluted to a volume of 200mL?

How many grams of Cu were in the sample?

How many grams of Cl were in the sample?How many moles?


What is the formula of the Copper Chloride compound?
What exactly do you not understand about this?

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