Experimental Data: Mass of empty 250mL beaker 110.58g107.548g Mass of 250-mL beaker with copper (II) chloride sample Mass of copper (II) chloride sample (by subtraction) Mass of watch glass and filter paper (pre-weighed) Mass of watch glass, filter paper, and dried copper metal Additional Data: Molar Mass of Copper Molar Mass of Chlorine 3564 Mass of copper metal produced by the reaction (by subtraction) Calculation: Mass of chlorine in original sample of copper (II) chloride (by subtraction) Calculation: Moles of copper metal (grams to moles conversion) Calculation: Moles of chlorine (grams to moles conversion) Calculation: Experimentally determined mole ratio of chlorine to copper Calculation: Chemical formula of copper (II) chloride as determined experimentally 1. One way to express the fixed proportion of elements in the compound copper (II) chloride is the chemical formula. Another way is the mass percent of each element in the compound: MassPercentofCopper=MassofCopper(II)ChlorideMassofCopper100% The theoretical mass percent of copper in the compound (as predicted by the true chemical formula, CuCl2, would be: MassPercentofCopper=MolarMassofCopper+2(MolarMassofChlorine)MolarMassofCopper100% Complete this calculation and determine the theoretical mass percent of copper in copper (II) chloride: 2. Now calculate the Mass Percent of Copper from the experimental data: MassPercentofCopper=MassofCopper(II)ChloridesampleMassofCumetalproduced100% 3. Compare the experimental mass percent of copper to the theoretical value by calculating the Percent Error. Experimental Data