Experimental Data 3 pts for blanks in experimental section M

Experimental Data (3 pts. for blanks in experimental section) Mass of copper(II) chloride CuCl Mass of aluminum Mass of aluminum remaining after reaction Mass of aluminum that reacted Mass of filter paper and watchglass Mass of filter paper, watchglass, and copper Mass of copper recovered 3.ooi \' ! 15242 .3849 Show calculations with each blank except for the molar mass of Cu (Unless otherwise noted, 6 pts. for blanks including calculations in this section) Copper Molar mass of CuCl2 131.4S 3.54 taos 4S3) y.uul 6.03a3 mo Mole of CuCl dissolved Ma b. 0383 ml Balanced equation for the dissociation of CuClz in water (4 pts.) Mole of copperll) ions (Cu?\") initially in solution Balanced net ionic equation for the reaction of copper(II) chloride with aluminum (4pts.) Mole of copper metal (Cu) expected to be formed 0.0 oy mol m e Amol

Solution

Answer from Cu part:-

The experimental error which causes the percent of yield less than 100% is that in the reaction all the reactant are not completely converted into product.

Answer from Al part:

Molar mass of AlCl₃=26.83+3(35.4)=133.18

Mass of AlCl₃ after the raection= 3.0049-1.3849=1.6209 g

Moles of AlCl3 =1.6209/133.18=0.011 mole

Balanced equation= 2 AlCl3------>2Al+3Cl₂

moles of aluminium initially present in sloution

=0.011 mol AlCl₃*2 mol aluminium/2 mol AlCl₃=0.011 mole aluminium

Molar mass of Aluminium=0.011 mole*26.83g/mol=0.29678 g

therefore theoretical molar mass of aluminium=0.29678 g