Copper Lab
Balanced EquationIntroduction
In this lab we will be mixing aluminum powder with a mixture of copper sulfate and water. The purpose of this lab is to measure out different quantities of chemicals and along with there molar mass incorporate those numbers into equations that will give us info such as the limiting reactant, percent yield, and theoretical yield. With this lab you are also given the opportunity to observe multiple chemical reactions.
Supplies
In this lab we will be mixing aluminum powder with a mixture of copper sulfate and water. The purpose of this lab is to measure out different quantities of chemicals and along with there molar mass incorporate those numbers into equations that will give us info such as the limiting reactant, percent yield, and theoretical yield. With this lab you are also given the opportunity to observe multiple chemical reactions.
Supplies
Copper Sulfate Pentahydrate (CuSO4)
Aluminum Powder (Al)
Medium Sized Beaker
Glass Stirring Rod
Periodic Table
Paper Towels
Asbestos Pad
Paper Filter
Appron
Goggles
Stand
Scale
Aluminum Powder (Al)
Medium Sized Beaker
Glass Stirring Rod
Periodic Table
Paper Towels
Asbestos Pad
Paper Filter
Appron
Goggles
Stand
Scale
Flask
Safety
For this lab there are should be more safety standards in place than previous labs. The chemicals when mixed together can and are very reactive when heated. Due to this you need to wear aprons, goggles, and it is highly recommended to not wear open toed shoes due to the high possibility of an overflow of the hot contents. Keep the chemicals under the hood vent at all times, follow other instructions, and don't be stupid.
Procedure
We began our lab by aquiring all of our equipment and dressing out in the proper gear. We then measured out 73 grams of water in our beaker along with 10 grams of CuSO4. We accidentally measured out 4.12 grams of aluminum so we will later alalyze how this effects our final results. We heated our water until it reached a
slow boil then slowly added the CuSO4 while stirring with our glass rod. Afterwards we turned off the bunsen burner so as to keep from reaching a rapped boil and added the aluminum still stirring thoroughly. We then waited and observed the reactions taking place including spontaneous heat, copper chunks rising to the surface, and the change in color of the liquid. After it was done we seperated the copper chunks from the liquid through a paper funnel. The liquid that ended up in the bottom of the beaker after the seperation was perfectly clear due to the large amount of aluminum used in the experiment.
Safety
For this lab there are should be more safety standards in place than previous labs. The chemicals when mixed together can and are very reactive when heated. Due to this you need to wear aprons, goggles, and it is highly recommended to not wear open toed shoes due to the high possibility of an overflow of the hot contents. Keep the chemicals under the hood vent at all times, follow other instructions, and don't be stupid.
Procedure
We began our lab by aquiring all of our equipment and dressing out in the proper gear. We then measured out 73 grams of water in our beaker along with 10 grams of CuSO4. We accidentally measured out 4.12 grams of aluminum so we will later alalyze how this effects our final results. We heated our water until it reached a
slow boil then slowly added the CuSO4 while stirring with our glass rod. Afterwards we turned off the bunsen burner so as to keep from reaching a rapped boil and added the aluminum still stirring thoroughly. We then waited and observed the reactions taking place including spontaneous heat, copper chunks rising to the surface, and the change in color of the liquid. After it was done we seperated the copper chunks from the liquid through a paper funnel. The liquid that ended up in the bottom of the beaker after the seperation was perfectly clear due to the large amount of aluminum used in the experiment. Equations
2Al + 3CuSO4 -> 2Al3(SO4) + 3Cu
Limiting Reactant
4.12g. Al X 1mol Al/ 26.98 g. Al= .153 mol Al
10g. CuSO4 X 1mol CuSO4/ 111.66 g. CuSO4= .09mol CuSO4
.09mol CuSO4X 2mol Al/3mol CuSO4= .06mol Al needed
Aluminum is the limiting reactant...
Grams of Copper
4.12g Al X 1 mol Al/26.98g Al X 1 mol Cu/1 mol Al X 63.55g Cu/1 mol Cu=9.7g. Cu
Theoretical Yield4.12 g. Al X 1mol Al/ 26.98g. Al X 3mol Cu/ 2mol Al X 63.6g. Cu/ 1mol Cu= 14.57 g. Cu
Percent Yield9.7g. actual/ 14.57g. theoretical X 100= 67%
Mole Ration
Al 2:3 Cu
Molar MassAl= 26.98gCu= 63.46gCuSO4=111.66g
Observations
- White Foam - Spontaneous Heat - Formation of a Solid (Copper) - Constant Bubbles - Change in Color of Water
- White Foam - Spontaneous Heat - Formation of a Solid (Copper) - Constant Bubbles - Change in Color of Water
Conclusion
From our equations and observations during the lab we came to some interesting conclusions. We found our limiting reactant to be Aluminum along with our percent yield being 67%. We used a large amount of Aluminum which did change the out come of our experiment. Our theoretical yield came out to be 14.57 g. of copper. There were also a large number of chemical reactions taking place. After the bunson burner was turned off the liquid continued to heat up, a thin foam formed at the top of the liquid, there was a formation of a solid(Cu), and there was constant bubbling from the copper located at the bottom of the beaker.
