Aluminum & Copper II sulfate Redox Lab

Introduction: The purpose of this lab is to find out the number of grams of copper that will be formed from an oxidation reduction reaction when you know the mass of Aluminum that reacted with a known amount of copper 2 sulfate pentahydrate and to compare this to the actual yield of copper.

Purpose: To determine the # 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 copperII sulfate 5hydrate and to compare this to the actual yield of copper.

Materials & setup: 1.) measured sample of aluminum powder, and measured amount of copper sulfate pentahydrate 2.) React the 2 in a aqueous medium within a medium sized beaker, 3.) stir frequently 4.) Filter 5.) dry 6.)Weigh the resulting product.7.) Safety equipemt-goggles&aprons 8.0 Bunsen Burner and striker 9.)Medium sized beaker & funnel

Procedure: First we got a medium sized beaker. We added about 150 ml of water to the beaker, and set up the Bunsen Burner to the gas. Measured out about 15g of Copper(II) sulfate pentahydrate (CuSO4---> 5 H2O and then recorded the mass in the data table.We slowly added the crystals(CuSO4) to the heating water. With a glass stirring-rod, we stirred the solution until the crystals were mostly all dissolved. Then we got about 2 grams of aluminum powder and carefully added it into the hot solution. We continued stirring for about 15 minutes until you we could hardly see any pieces left. We heated the solution for about 3-4 mintues after all the pieces were dissolved, then removed from heat. Then we used the filter paper and filtered out the residue in the beaker, catching the filtrate in the Erlenmeyer flask. We rinsed out the beaker with a small amount of water to rinse out the residue in the bottom. We spread out the filter paper and let it dry overnight. We cleaned and dried the glassware and turned off the Bunsen burner and put it away. The next day we looked at our results of the dried filter paper. We made a table of our results:

Name	Mass
CuSO4	16.79
Al	2.13
coffee filter	1.1
1.7	1.7

Analysis:
1. Write a balanced reaction equation. 3CuSO4+2Al---> 3Cu+Al2(SO4)3
2. Write the net ionic equation: 3CuSO4(s) + 2Al(s) --> 3Cu + Al2(SO4)3(s)
3. What is the reducing agent and oxidizing agent?
4. Calculate the mass of the copper:22.1g Al X 1 mol Al/26.98g Al X 1 mol Cu/1 mol Al X 63.55g Cu/1 mol Cu = 78.1g Cu
5. Subtract the filter paper from the dry residue/ product in our data table(actual yield of Cu)
6. Percent yield of experiment
7. Give 3 reasons of why the amount of copper that should have formed and the amount of copper that actually formed might be different.

Types of Reactions.

1. Introduction/Background: In this lab, we will perform various chemical reactions. We will record our observations and then identify the types of reactions and balance each chemical equation. The lab purpose is to become more familiar with the 5 reaction types we use.



The 5 reaction types:


2. Procedure:
A. First we got on all our safety gear(goggles and aprons)
B. Next we obtained 3 small test tubes from the lab kit & cleaned them out.
C. In the first test tube we placed one piece of zinc and about 1/2 ml of CuSo4 solution.
D. We observed the reaction and waited for around 5 mins.
E. In the second test tube we added 1/2 ml Ba(No3)2 solution to about 1/2 ml of CuSo4 solution.
F. In the third test tube we placed a pinch of magnesium, to 1/2 ml oh HCl solution.
G. We lit a Bunsen burner & observed the flame.
H. Over the flame we put H2O2 and lightly heated it.
I. Then we added a pinch of MnO2(magnesium oxide).
J. Then we observed the reactions that took place, and cleaned up the lab station.

3. Data Analysis:
Balanced equations (( 8===D O: ))
1. Zn + CuSO4 --> ZnSO4 + Cu
Single-Displacement Reaction

2. Ba(NO3)2 + CuSO4 --> BaSO4 + Cu(NO3)2
Double-Displacement Reaction

3. Mg + 2HCl --> MgCl2 + H2
Single-Displacement Reaction

4. C3H8 + 5O2 --> 3CO2 + 4H2O
Combustion Reaction

5. 2H2O2 --> 2H2O + O2
Decomposition Reaction

Polarity and Molecular Shape Lab

Title:
Polarity and Molecular Shapes Lab.

Statement of the Problem: How are molecular shapes determined?

Objectives: Construct models of molecules. Next, determine molecular shapes. Then, predict polarity of molecules.

Materials:
Molecular model kit, and lab sheet.

Procedure:
1.) The first thing we did was draw each Lewis structure for the following formulas: CH4, BF3, C3H8, H2O, Si2H6,HF, CH3NH2, H2O2, N2, SeF4, C2H4,SiH2O, IF3,SF6,CO2, and SO3(2-). 2.) Next, we constructed each 3-dimensional figure. 3.)We then drew each figure onto the lab sheet, We used solid lines to represent bonds, dashed lines to point back to the plane of the paper, and wedged lines for bonds that point out from the plane toward the viewers. 4.) Finally we looked on our other lewis structure papers to find the shape, bond angle, and polarity & resonance of each structure.

Analysis:
1) Explain how water shape causes it to have polarity. 2) Describe how water’s properties would be different if the molecules were linear instead of bent. 3) Based on the results of this experiment, list the molecules from the experiment that would be water-soluble.

Results:

Lab Report Period 3 Group 11

Title:
Paper Chromatography Lab

Statement of the problem:
What is the mobile phase on a paper chromatography investigation?
What is the stationary phase in a paper chromatography investigation?
What is meant by the term retention time?
Paper chromatography is an important separation technique that depends on difference in both absorption and solubility.


Hypothesis:
Our hypothesis was H2O. It would be best because it has polarity and water is good.


Materials:
The materials that we used included: 9 strips of chromatography paper, H2O, CH3OH, C3H7OH, C6H14, 24 well plate,water-soluble overhead pens(black, red, green,brown,purple,yellow,blue).


Safety:
We used goggles and aprons. We stayed out of the fumes, and the fume hood. We put the chemicals under the fume hood. We used all of the safety precautions on this lab, and followed the directions.


Procedure:
First, we got on our safety equipment, then we got all of our materials together. Next, we filled up the 24 well plate with H2O, CH3OH, C3H7OH, and C6H14. Then we marked our paper strips with black marker. After that, we put the dots on the piece if paper and put it in the liquids and watched it rise. Our group let the paper sit in the liquids for approximately 30 minutes. We used the different colors to see which one of them would rise the most. After we wrote down all of our data, and finished the lab, we cleaned up and dumped the stuff out and finished the lab procedure.


Results:
During our lab, we figured out that H2O would rise the most with the black. We tried to use the other colors to compare them to the black. The liquid that rose the least was C6H14 because, the polarity is low.

Conclusion:
In conclusion, we found out that H2O was most polar, and rose up the paper quicker than the other solutions.