Answer Happy

7. Moles of CuCl2​⋅2H2​O used mols (show your calculation) 8. Moles of copper product based on moles of Al mols (show your calculation) 9. Moles of copper product based on moles of mols CuCl2​⋅2H2​O (show your calculation) 10. Limiting reactant 11. Grams of Cu product based on the limiting reactant B (theoretical yicld)(show your calculation) 12. Percent yield of Cu ( 2 to 3 significant figures) % (show your calculation)
1. What safety precautions are cited in thas experiment? 2. What it the purpose of adding hydrochloric acid to the reaction mixture? 3. A student combusted 0.500 g of purified aluminum powder with excess oxygen in an oxygen atmosphere according to the reaction. 4Al(s)+3O2​( B)⟶2Al2​O3​(5) a) What is the limiting reactant? b) How many moles of Al were used? mol of Al c) How many moles of Al2​O3​ would form, based mol of Al2​O3​ on the moles of the limiting reactant? d) How many moles of O2​ are required to react mol of O2​ completely with the aluminum? c) How many grams of O2​ are required to react g of O1​ completely with the aluminum? f) What is the theoretical yield of Al2​O3​ in grams? g of Al2​O3​ g) If the student collected 0.918 grams of A2​O2​ product, 06 what was the percent yield of Al2​O3​ obtained?
1. Describe the appearance of the copper(II) chloride solution and the aluminum foul before the reaction starts. (from video) 2. Describe the appearance of the solution and any solids after the reaction. (from video) 3. Heating the copper product at too high a temperature in an oxygen atmosphere results in the formation od copper (II) oxide. Write down the balanced chemical reaction. 4. If the copper is not completely dried, how would this change the yield of copper metal? 5. What are some reasons for obtaining a percent yield of less than 100 percent?