question archive a chemist wants to extract copper metal from copper chloride solution
a chemist wants to extract copper metal from copper chloride solution
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a chemist wants to extract copper metal from copper chloride solution. The chemist places 1.5 grams of aluminum foil in a solution of 14 grams of copper (II) chloride. A single replacement reaction takes place. what best explains the state of the reaction after the mixture
This is what I have so far but I'm stuck
Molar mass of Cooper=27
Given Mass = 1.5
Moles = .0555
Molar mass of Cooper Chloride = 134.45
Given mass = 14
3 moles of Copper chloride reacts with 4 moles of aluminium
4/3 * .1041 = .1388
3 moles of copper chloride produces 3 moles of copper metal.
3/3 * .1041 = .1041
Molar mass of cooper = 63.5
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Answer:
mass of Cu extracted=5.3g
Step-by-step explanation
Since copper is being extracted from copper chloride solution by reaction with aluminium foil,we have to determine the mass of the extract.
The reaction equation is as follows;
2Al(s)+3CuCl2(aq)-----2AlCl3(aq)+3Cu(s)
moles of Al=1.5/27=0.0556moles
moles of CuCl2=14/134.45=0.1041moles
mole ratio according to the reaction equation=Al:CuCl2=2:3=0.67
mole ratio according to the reactants available=Al:CuCl2=0.0556/0.1041=0.53
Therefore Al is the limiting reactant;
Use the moles of the limiting reactant to calculate the moles of Cu formed
Al:Cu=2:3
mole of Cu formed=(3/2)*0.0556=0.0834moles
mass of Cu formed=moles*molar mass=0.0834*63.5=5.2959g
Hence mass of Cu extracted=5.3g
