Long QuestionIf Possible please help.

Question

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Answer 1

2Al(s) + 3CuCl₂•2H₂O(aq) ==> 3Cu(s) + 2AlCl₃(aq) + 6H₂O(l) ... balanced equation

The reaction occurs because Al is more reactive than Cu and so will displace Cu in this single replacement reaction.

4.00 g CuCl₂•2H₂O x 1 mol CuCl₂•2H₂O/170.5 g x 2 mol Al/3 mol CuCl₂•2H₂O x 26.98 g Al/mol = 0.422 g Al

Theoretical yield of Cu:

4.00 g CuCl₂•2H₂O x 1 mol CuCl₂•2H₂O/170.5 g x 3 mol Cu/3 mol CuCl₂•2H₂O x 63.55 g Cu/mol = 1.49 g Cu

Hypothesis: Al metal will replace copper in copper(II) chloride to produce copper metal and soluble aluminum chloride because aluminum is more reactive than copper.

Materials: Aluminum metal, copper(II) chloride dihydrate, balance, distilled water, beakers/flasks, pipets, filter paper, filter funnel, drying oven.

Procedure: Use your common sense. I'll give you a brief outline, but will not write the entire procedure for you. You should be able to do that with the following assistance.

Weigh 4.00 g CuCl₂•2H₂O

Weigh 5 x 0.422 g Al (to be sure it is in excess)

Add both reagents to a given volume of water and stir the mixture to allow reaction to take place

Color change will indicate reaction has taken place (look up why the color changes for CuCl₂ vs Cu solid)

Filter the reaction mixture to obtain the solid copper

Dry the product and weigh the product

% yield:

The % yield is the actual yield/theoretical yield (x100%)

We will pick an actual yield of 0.75 g (minimum value given above)

% yield = 0.75 g/1.49 g (x100%) = 50.3% yield (note: if you chose 1.75 g, % yield would be >100% which is not possible.)

I'll leave the Discussion and Conclusions to you. Good luck.