Aluminum and Copper 2 Sulfate Lab

PURPOSE
To determine the number of grams of copper that will be produced from an oxidation reduction reaction when you know the mass of Aluminum that reacted with a known amount of cooper II sulfate pentahydrate and to compare this to the actual yield of cooper.


MATERIALS AND SETUP
You will obtain a measure sample of aluminum foil and measured amount of copper sulfate pentaydrate. You will then react the two in a aqueous medium within a medium sized beaker; stirring frequently. You will filter, dry, and weigh the resulting product.


SINGLE DISPLACEMENT REACTION
A chemical reaction in which one element takes the place of another element.


INTRODUCTION
In this lab, we tried to find out how many grams of copper would be produced form an oxidation reduction reaction. We mixed a known amount of Aluminum with a known amount of copper 2 sulfate pentahydrate. We then compared the theoretical yield with the actual yield of copper, and turned it into a percentage efficiency.

OBSERVATIONS

Throughout the lab we observed many things such as heat, bubbles, popping, a change in color, and other things. When we mixed the copper and Aluminum together it changed colors and the copper sediment settled to the bottom of the beaker that was hot but not boiling. After we did all that we took the aluminum and copper mixture and ran it through the filter paper taking out all of the copper sediment to see what our actual yield would be. Which was .5 copper.

CONCLUSION

In this lab we observed a chemical reaction between Aluminum and copper. When we mixed them together under heat we noticed some bubbling and other indicators of chemical reactions. After we stirred vigorsly for 20 minutes and saw the copper was disloved we poured the chemicals into 40mm filter paper and sepereated the aluminum out of the chemical. We then recorded our percent yeild and actual yeild afterward.

Introduction:
In this lab we were to take certain chemicals and mix them together to observe the five types of chemical reactions. The chemicals we used were the follows.
CuSo4
Ba(no3)2
Mg ribbon
HCL
H2O2

Materials:
3 small test tubes
CuSo4
Ba(NO3)2
Hydrochloric acid
Bunsen burner
Propane gas
H2O2
MnO2
goggles
aprons
test tube holders

Types of Reactions:

Synthesis: A reaction that has two or more materials meld together into one more completed compound.

Decomposition: A reaction in which one substance breaks down into to or more substances.

Single Displacement: One element takes the place of another element.

Double Displacement: Two elements take the place of two other elements.

Combustion: When the products of the reaction are Co2 or H2O

Observations:
CuSo4: For the first few minutes nothing notable happened. There was absolutely no change. CuSo4+Zn-ZnSo4+Cu Single Displacement.


Ba(NO3)2: Lots of foam and bubbling but other then that there was very little change over the few minutes we observed it. Ba(NO3)2+CuSO4-BaSO4+Cu(NO3)2 Double Displacement

Magnesium ribbon HCL: Violent hissing and bubbling lots of heat is being created. Hydrogen gas is being released. The magnesium ribbon was eventually broke down. H2O2-HO Decomposition.

Conclusion: Some chemical reactions are much more active then others, and act differently then other reactions. Like a Magnesium ribbon in HCL creates a smoke ring that travels up and down the test tube, while CuSo4 just turns blue.

Pictures and data table will not load into this blog. Sorry!