Chemistry 1 Stoichiometry Lab Essay Example
Stoichiometry
04/09/12
Chemistry I B
Ms. Norton
Introduction/Pre-laboratory Assignment: 1. Write out and balance each of the following equations. A. CuSO4 + Fe Cu + FeSO4 B. 3CuSO4 + 2Fe 3Cu + Fe(SO4)3 2. If Iron (III) Sulfate were formed, what mass of Copper would be expected and what is the limiting reagent? C. 2.26 g Cu D. Fe 3. If Iron (II) Sulfate were formed, what mass of Copper would be expected and what is the limiting reagent? E. 2.8 g Cu F. CuSO4
Driving Question: What compound is formed when you add 7 g of CuSO4 to 2 g of Fe?
Goal: To correctly identify what compound is formed and how close it is to the theoretical yield.
Materials:
* Safety Goggles * Lab Apron * Two 250-mL Beakers * Ring Stand * Ring * Wire Gauze * Bunsen Burner * Balance * Stirring Rod * Matches * Water (H2O) * Iron (Fe) * Copper (II) Sulfate (CuSO4)
Chemical Names: * Water (H2O) * Iron (Fe) * Copper (II) Sulfate (CuSO4) * Iron (II) Sulfate (FeSO4) * Iron (III) Sulfate (Fe2(SO4)3) * Copper (Cu) * Methane (CH4) * Copper (II) (Cu2+) * Iron (II) (Fe2+) * Sulfate (SO4) Procedure: I. Place 7.00g of copper (II) sulfate in a beaker. II. Add about 50mL of water to the beaker III. Light the Bunsen Burner and place it under the beaker. Adjust the burner so the hottest part of the flame touches the bottom of the beaker. IV. Carefully heat and stir the mixture in the beaker. The solution should be hot, but not boiling. After all of the crystals have dissolved, remove the beaker form the heat. V. Add 2.00g of iron filings slowly to the hot copper sulfate solution while stirring. Record observations. VI. Allow the beaker to cool for 10-15 minutes. VII. Pour off (decant) the solution into a different beaker. Pouring the solution down a stirring rod is recommended. Make sure not to disturb the
04/09/12
Chemistry I B
Ms. Norton
Introduction/Pre-laboratory Assignment: 1. Write out and balance each of the following equations. A. CuSO4 + Fe Cu + FeSO4 B. 3CuSO4 + 2Fe 3Cu + Fe(SO4)3 2. If Iron (III) Sulfate were formed, what mass of Copper would be expected and what is the limiting reagent? C. 2.26 g Cu D. Fe 3. If Iron (II) Sulfate were formed, what mass of Copper would be expected and what is the limiting reagent? E. 2.8 g Cu F. CuSO4
Driving Question: What compound is formed when you add 7 g of CuSO4 to 2 g of Fe?
Goal: To correctly identify what compound is formed and how close it is to the theoretical yield.
Materials:
* Safety Goggles * Lab Apron * Two 250-mL Beakers * Ring Stand * Ring * Wire Gauze * Bunsen Burner * Balance * Stirring Rod * Matches * Water (H2O) * Iron (Fe) * Copper (II) Sulfate (CuSO4)
Chemical Names: * Water (H2O) * Iron (Fe) * Copper (II) Sulfate (CuSO4) * Iron (II) Sulfate (FeSO4) * Iron (III) Sulfate (Fe2(SO4)3) * Copper (Cu) * Methane (CH4) * Copper (II) (Cu2+) * Iron (II) (Fe2+) * Sulfate (SO4) Procedure: I. Place 7.00g of copper (II) sulfate in a beaker. II. Add about 50mL of water to the beaker III. Light the Bunsen Burner and place it under the beaker. Adjust the burner so the hottest part of the flame touches the bottom of the beaker. IV. Carefully heat and stir the mixture in the beaker. The solution should be hot, but not boiling. After all of the crystals have dissolved, remove the beaker form the heat. V. Add 2.00g of iron filings slowly to the hot copper sulfate solution while stirring. Record observations. VI. Allow the beaker to cool for 10-15 minutes. VII. Pour off (decant) the solution into a different beaker. Pouring the solution down a stirring rod is recommended. Make sure not to disturb the