Three experiments were performed in the lab. The first experiment involved producing solid copper from a copper(II) chloride solution with zinc. The second experiment’s purpose was to determine the percent composition of water-soluble sweeteners and flavorings in gum. The third experiment was performed in order to determine the empirical formula for two hydrated compounds: magnesium sulfate and copper(II) sulfate. All three experiments _____.
For the “Empirical Formula of Copper Chloride” lab, the amount of Zn that reacted was calculated to be 0.20g Zn, converted to moles, this amount was found to be 3.05 x 10-3mol Zn. The amount of Zn that reacted is also equal to the amount of Copper chloride that reacted. This value was then converted to grams of Copper chloride, which was found to 0.41g CuCl2. Using the amount of copper obtained at the end of the lab (0.29g), we calculated the amount of chloride that reacted to be 0.12g. The masses of both the copper and chloride were then converted to moles: 4.56 x 10-3mol and 1.69 x 10-3mol respectively. A ratio of 2.70:1 was found and rounded to 3:1. The formula Cu3Cl2 was obtained and compared to the actual formula, CuCl2. All calculations for this lab are shown in-depth in Figure 3.
Determine the amount of Zn that reacted, and then convert this amount to moles. The amount of Zinc that reacted is equal to the amount of Copper chloride that reacted.3.05×10-3mol Zn = 3.05 × 10-3mol CuCl2Determine the molar mass of the Copper chloride compound, assuming that the compound is Cu21mol CuCl2=63.6g Cu+ 2 35.5g Cl= 134.6gConvert the moles of the Copper chloride compound into grams. Determine the amount of chloride in the Copper chloride compound using the amount of copper produced. Convert the masses of copper and chloride to moles. Determine the ratio between the amount of copper and chloride atoms to find the formula for the Copper chloride based on this lab’s results. Determine the percent...