Firstly, you need a balanced equation:
2Al(s) + 3CuCl2 (aq) ----> 2AlCl3 (aq) + 3Cu (s)
Now, you need to convert grams to moles:
Moles of Al = 0.25 g x 26.98 g mol-1 = 9.266 x 10-3 mol Al (s)
From the equation above we see that the ratio of CuCl2 to Al(s) is simply 3:2 so we must work out the moles of CuCl2 required to react completely with Al(s):
Moles of CuCl2 = 9.266 x 10-3 x 3/2 = 0.0139 mol CuCl2
Next convert moles to grams:
Grams CuCl2 = 0.0139 mol CuCl2 x 134.45 g mol-1 = 1.869 g
This means that you would need 1.869g of Copper II Chloride to reacted completely with 0.25 g Aluminium.
Therefore, Copper II Chloride is the Limiting Reactant.
Aluminum would be the limiting reagent
The products of the reaction are aluminium trichloride, copper and hydrogen.
For copper, it is an element. It could be both reactant and product. While purifying copper will be the product. But copper would be the reactant in case of preparing hydrogen or copper sulphate salts.
Stainless steel is heavier then aluminium.
No. Copper(I) chloride and copper(II) chloride are both ionic solids.
Aluminum would be the limiting reagent
2 Na OH + CuCl2
The products of the reaction are aluminium trichloride, copper and hydrogen.
For copper, it is an element. It could be both reactant and product. While purifying copper will be the product. But copper would be the reactant in case of preparing hydrogen or copper sulphate salts.
For copper, it is an element. It could be both reactant and product. While purifying copper will be the product. But copper would be the reactant in case of preparing hydrogen or copper sulphate salts.
Stainless steel is heavier then aluminium.
There are two kinds of copper chloride. Copper(I) chloride is CuCl. Copper(II) chloride is CuCl2.
No. Copper(I) chloride and copper(II) chloride are both ionic solids.
No. Copper(I) chloride and copper(II) chloride are both ionic solids.
copper + Chlorine = copper chloride
Copper I Chloride is CuCl and Copper II Chloride CuCl2
CuCl2.