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REPORT - Determination of Reaction Yield Mass of CuCl₂ + 2 H₂O Mass of Al foil used Mass of empty filter paper 4. Mass of filter paper plus copper 5. Mass of copper metal product [4]-[3] 6. Moles of Al used (show your calculation) 1. 2. 3. 7. Moles of CuCl₂ + 2 H₂O used (show your calculation) 8. Moles of copper product based on moles of Al (show your calculation) 9. Moles of copper product based on moles of CuCl₂ + 2 H₂O(show your calculation) Name 10. Limiting reactant 11. Grams of Cu product based on the limiting reactant (theoretical yield)(show your calculation) 12. Percent yield of Cu (2 to 3 significant figures) (show your calculation) 6.35 0.60 1.49 3.27 mols mols mols mols
Pre-Laboratory Questions and Exercises Answer in the space provided. 1. What safety precautions are cited in this 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, 4 Al(s) + 30₂ (g) a) What is the limiting reactant? b) How many moles of Al were used? c) How many moles of Al-O, would form, based on the moles of the limiting reactant? d) How many moles of O₂ are required to react completely with the aluminum? e) How many grams of O₂ are required to react completely with the aluminum? f) What is the theoretical yield of Al-O, in grams? g) If the student collected 0.918 grams of Al-0, product, what was the percent yield of Al-O; obtained? 2 Al;0; (s) mol of Al mol of Al2O, mol of 0: g of 0₂ g of Al₂O,
Post-Laboratory Questions and Exercises Due after completing the lab. Answer in the space provided. Name 1. Describe the appearance of the copper(II) chloride solution and the aluminum foil 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? Note: This lab handout has been adapted from CHEM 1105 at Houston Community College