1. Calculate the stoichiometric (theoretical) yield, experimental (actual) yield and percent yield for copper.
2. Determine/write out the balanced complete chemical reaction including phase.
3. Now assume that the Copper (II) sulfate pentahydrate (2019-2020 students used Copper (II) chloride dihydrate) solid is actually aqueous (which you do done in lab), determine the net ionic reaction showing all appropriate work.
4. Now rewrite the balanced complete chemical reaction again leaving some place above the chemical reaction for work. Now show all work and determine what is being oxidized, what is being reduced, oxidizing agent and reducing agent in the format discussed in your notes. Also, include the balancing of Redox reaction work also.
5. Did it you need to be as accurate with the volume of water added to the 250.ml container as when you massed out the Iron? What is the water used for so the chemical reaction could occur?
6. What caused the blue color in the aqueous reactant? What are the phase and color of each product.
7. What happened to the blue color from the reactant to the product.
8. Beside your calculations, what observation(s) in lab did you make to support which reactant was the limiting reactant in the reaction?
9. If in massing out the product, you spilled some of the solid product, how would the value of the percent yield of the solid product be affected? Explain.