Two tests are run during this lab, in two separate beakers. The first beaker contains 0.50 g of copper(II) chloride dihydrate and 0.08 g of aluminum. After reacting and drying the product, 0.178 g of solid copper is massed. The second beaker contains 0.53 g of copper(II) chloride dihydrate and 0.05 g of aluminum. After reacting and drying the product, 0.182 g of solid copper is massed.

1-Write the balanced net ionic equation for the reaction in this lab using equation editor.

2-For the reaction in beaker 2, what experimental errors could have contributed to your percent yield? Explain how your error is consistent with your observations in the lab and with your results.

3-If all water was removed from beakers 1 and 2 after the reaction has gone to completion but before adding HCl and filtering, list the chemical species left in the beakers. Remember that there are no ions when all of the water has evaporated.

beaker 1-

beaker 2-

4- uppose you wanted to try a third test where there would be no limiting reactant, instead, you would have exactly the right amount of copper(II) chloride dihydrate and aluminum to fully react together with neither reactant in excess. If you use 0.723 g of CuCl2 2H2O, how much aluminum, in grams, would you need to add?