<p>Left Over Aluminum Lab Discussion Questions 1) Write the balanced chemical equation for the reaction that occurred between the aluminum wire and the copper (II) chloride solution. 2) Identify the type of reaction (double replacement, combustion, oxidation-reduction, etc). 3) Which starting material in the reaction is the limiting reactant and which material is present in excess? Explain. 4) Calculate the percent yield of copper. 5) What physical evidence do you have that shows that copper (II) chloride is the limiting reactant? 6) Discuss reasonable and potential sources of error in this experiment. 7) Discuss potential reasons why the percent yield of recovered copper may be greater than 100% 8) Why do you think scientist add excess of one or more chemicals when performing a reaction rather than combine the exact stoichiometric ratio? 9) What factors do you think may lead scientists (in industry, for example) to choose one certain starting material as the limiting reactant and another as the excess chemical?</p><p>10) Calculate the “molarity” (moles of copper sulfate per liter of solution) present in your copper sulfate solution (remember: we used 25 ml of the copper II chloride solution, so you will need to convert them to Liters) 11) Given that the correct molarity is 0.50, calculate your % error: 12) Write a paragraph describing this experiment thoroughly, explain what was happening at the molecular level in each of the observations you recorded.</p><p>Left Over Aluminum Lab Discussion Questions 1) Write the balanced chemical equation for the reaction that occurred between the aluminum wire and the copper (II) chloride solution. 2) Identify the type of reaction (double replacement, combustion, oxidation-reduction, etc). 3) Which starting material in the reaction is the limiting reactant and which material is present in excess? Explain. 4) Calculate the percent yield of copper. 5) What physical evidence do you have that shows that copper (II) chloride is the limiting reactant? 6) Discuss reasonable and potential sources of error in this experiment. 7) Discuss potential reasons why the percent yield of recovered copper may be greater than 100% 8) Why do you think scientist add excess of one or more chemicals when performing a reaction rather than combine the exact stoichiometric ratio? 9) What factors do you think may lead scientists (in industry, for example) to choose one certain starting material as the limiting reactant and another as the excess chemical? 10) Calculate the “molarity” (moles of copper sulfate per liter of solution) present in your copper sulfate solution (remember: we used 25 ml of the copper II chloride solution, so you will need to convert them to Liters) 11) Given that the correct molarity is 0.50, calculate your % error: 12) Write a paragraph describing this experiment thoroughly, explain what was happening at the molecular level in each of the observations you recorded.</p>