Aluminum & Copper Sulfate Yield Lab

Introduction and Problem:
In Chemistry, percent yield is used to show what materials you have left and how much leeway you have in an experiment। This is a really great tool for scientists to use. It gives them a chance to see how much of a substance produces with the limited materials. With all this in mind, How does Aluminum take the place of Copper in Copper (II) Sulfate? I predict that Aluminum and copper switch places because of Single Displacement.

3CuSO4 + 2Al = Al2(SO4)3 + 3Cu

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 copper II sulfate pentahydrate and to compare this to the actual yield of copper. Also to determine the percent yield of Copper II Sulfate Pentahydrate by determining the theoretical percent yield.


Materials and Setup:
You will obtain a measured sample if aluminum foil and a measured amount of copper sulfate pentahydrate. You will then react the two in a n aqueous medium within a medium sized beaker: stirring frequently. You will filter, dry, and weigh the resulting product.

Procedure:
1. Obtain a medium sized( 250 to 400 ml) beaker.
2. add 75 to 100 ml of water to beaker: set-up apparatus to heat your mixture over a bunsen burner to begin heating.
3. measure out about 15g of Copper (II) sulfate pentrahydrate (CuSo4* 5H2O) and record the mass in the data table. Then slowly add the crystals to the heating water.

4. with a glass stirring rod, stir the solution until the Copper II sulfate pentahydrate is dissolved.

5. while the copper sulfate crystals are dissolving one member of the group can go and get the foil. Carefully weigh out a piece of aluminum foil that weighs between .7 to 1.0 grams. Record the mass exactly into the data table (thousandths place).

6. Tear the foil into small pieces and carefully add it to the hot solution with continuous stirring until all the foil is placed into the beaker.

7. Stirring frequently allow the reaction to occur until you cant see anymore silvery foil pieces. This will take 15 to 20 minutes so be patient. Once you can't see anymore foil pieces no matter how small, heat and additional 3 to 4 minutes, then remove from the heat.

8. write your names around the outside edge of a filter paper(so you can claim it later), weigh and record the mass in the data table.

9. use the filter paper and your funnel to filter the residue in the beaker, catching the filtrate into the Erlenmeryer flask provided.

10. Rinse out your beaker with a small (amount just covering the bottom of the beaker) of water to be sure you obtained all of the product/ residue.

11. Remove the filter paper from the funnel and spread it out on a paper towel to dry overnight.

12. Clean and dry the glassware. Be sure the propane is turned off and Bunsen burner disconnected and put away. Straighten up the area.

13. Upon returning the next day. Weigh the filter paper and dry residue and record that mass in the data table. Throw filter paper and residue away.

14. Construct a data table with the following parts:

mass of copper II sulfate pentahydrate

Mass of aluminum foil

mass of coffee filter

Mass of dry Residue/product+filter paper.

Safety:
In this lab safety is a big issue considering you are working with a Bunsen burner and potentially hazardous chemicals. So you should wear the proper safety gear, such as: Goggles, aprons, gloves and make sure that your instructor is in the room just in case something crazy like and explosion happens. Make sure you know where all the First Aid kits are and make sure that you know how to use the eye washer and shower stations just in case you get some of the chemicals explode on to you or your eyes.Also be aware where your fire blanket is in the room since we are dealing with fire. Be sure that if there is any broken glass to put it into the the designated area in your class room. We'd rather no one lose and eye during this product.

During Procedure:
During this procedure we used various amounts of lab equipment to make sure that it was a safe fun lab! During you need to make sure that you are taking notes on some of the variables that are subject to change such as the amount of copper used or aluminum flakes this is very important (reason for putting it twice).
Making a Table:

Materials	Mass (g)
Copper (II) Sulfate Pentahydrate	15
Aluminum	1
Coffee Filter	0.81
Product	2.53

Conclusion:
As I predicted, single displacement is what made Aluminum switch places with Copper in the Copper (II) Sulfate. By finding the yields, we come to the conclusion that materials are limited to their grams/ amount of grams. With this, Aluminum took the place of Copper, and produced copper outside of CuSO4, which made it AlSO4.

Types of Reactions Lab

Types of Reactions Lab

What are the reaction types of certain elements combined together?

Introduction:

We all love explosions and doing labs. But what exactly happens when it does the explosions? As we look through the five different types of chemical reactions, we see that they all have their own characteristics on what happens in them. But what would happen if we add chemicals to chemicals? In this lab we will be observing the different types of chemical reactions and will be becoming more familiar with these different types of reactions.

Materials

• 3 small test tubes
  
• test tube rack
  
• Zinc
• 1 ml of CuSO4
• 1/2 ml of Ba(NO3)2
• Magnesium Ribbon
• 1/2 ml of HCL Solution
• Bunsen Burner
  
• Propane gas (C3H8)
• 2 ml H202 Solution
• pinch of MnO2
  

Procedure:

First we will obtain 3 test tubes. In our first test tube, we will place a piece of zinc and about 1/2 mL of CuSO4 solution. We will observe the combination of these components and write down our results of the data. Next in the third test tube we will place a piece of magnesium ribbon in it and then add about 1/2 ml of HCL solution. After that we will record our observations and results. We will then light a Bunsen burner which is burning propane gas, (C3H8) and we will record our observations of the flame. We will the rinse out our first test tube and add about 2 mL H2O2 solution. After that we will light the Bunsen burner and lightly heat up the H2O2 solution and record our observations and results. For our next reaction we will add a pinch of MnO2 (catalyst) to the H2O2 solution and we will lightly heat up the mixture and record our observations and results. After analyzing all of our reactions we have made a data table to neatly organize our data.

Results (Data):

Chemicals	Added Chem.	Products	Type	Evidence
CuSO4	Zn	Cu + ZnSO4	Single Displacement	Zn takes Cu Place
Ba(NO3)2	CuSO4	BaSO4 + Cu(NO3)2	Double Displacement	Ba and Cu switch places
HCl	Mg	H2 + MgCl2	Single Displacement	Mg takes H place
H2O2	C3H8	H2O + CO2	Combustion	Water and Carbon Dioxide is released
H2O2	none	H2O + O2	Decomposition	Bubbles and Splint, oxygen is present

Discussion:

This lab was very informative, and helped introduce more into chemistry and showed us actual reactions. After examining the reactions taken place in the lab, i can honestly feel like i am in an actual chemistry class now. Any other lab did not feel like chemistry, in other words other labs besides this one was lame. I can say for sure that the splint test was my favorite and was really awesome. It was so awesome that we had to do it again. Mixing chemicals are pretty awesome, and i am sure that everyone loves reactions that you can easily tell when something is happening. To all my homies out there, "Reactions rock!" and "Peace!"

Conclusions:

In conclusion we have learned how different chemicals and elements react with one another. We have examined the different evidence of certain types of chemical reactions. After viewing the results of each reaction we recorded and concluded that we have became more familiar with chemical reactions. Also we have concluded that the splint test was sweet! and that the whole lab was completely BAD A$$!!!!!!

CHEMISTRY ROCKS!!!!!!!!!!!!

Polarity and Molecular Shape Lab

Statement of the problem:

We have been talking in class about how to arrange atoms in Lewis Structures. Many people just disregard the electron pairs because they think they don't amount to anything. I think this is bogus. But with that in mind we searched for the real answer, How are molecular shapes determined?

Hypothesis:

We predict that unbonded pairs of electrons determine the shape of the molecule.

Materials:

• Molecular Model kit
• Polarity and Molecular Shape LAB Worksheet
• 6-3 worksheet

Procedure:

1. We built a model out of the molecules listed on the data table on the back of the Polarity and Molecular Shape LAB Worksheet. (CH4, BF3, C3H8, H2O, Si2H6, HF, CH3NH2, H2O2, N2, SeF4, C2H4, SiH2O, IF3, SF6, CO2, and SO3(-2))
2. Next, we drew all the lewis structures of the molecules.
3. Then, after we wrote down the structure the molecule was.
4. Next, we stated the bonds and if it was polar or non-polar

ANALYSIS:

1. Explain how water's shape causes it to be polar.
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.
1. CH4 Tetrahedron 109 degrees non polar No resonance structure.

2. BF3 Triangular Planar 130.7 degrees Polar No resonance structure.

3. C3H8 Octahedral unknown degree non polar No resonance structure.

4. H2O Linear 104.5 degrees non polar No resonance structure.

5. Si2H6 Octahedral 130 degrees non polar With a resonance structure.

6. HF Linear 180 degrees Polar and No resonance structure.

7. CH3NH2 Triangular bi pyramid 150 degrees non polar With a resonance structure.

8. H2O2 Angular bent unknown degree Polar and With a resonance structure.

9. N2 Linear 180 degrees non polar With a resonance structure.

10. SeF4 Tetrahedron 90 degrees non polar with No resonance structure.

11. C2H4 120 degrees non polar With resonance structure.

12. SiH2O Triangular Planar Polar With resonance structure.

13. IF3 Triangular Planar 86 degree non polar with No resonance structure.

14. SF6 Octahedral 90 degree non polar with No resonance structure.

15. CO2 Linear 180 degree non polar with No resonance structure.

16. SO3 Triangular Planar 90 degree Polar with No resonance structure.

1. CH4-

2. BF3-

3.C3H8-

4.H2O-

5.Si2H6-



6.HF-

7.CH3NH2-

8.H2O2-

9.N2-

10.SeF4-

11.C2H4-

12.SiH2O-


13.IF3-


14.SF6-


15.CO2-



16.SO3-2-

Chromatography Lab

EXTREME COLOR SEPARATION

Introduction:

The Chromatography Lab is a way in which we can examine how different solvents separate a mixture into their pure components. The mixture that will be used in the lab are markers of different color that will be marked onto chromatography paper. The solvents will then separate the markers into different colors onto the chromatography paper. After the solvents separate the mixtures into their pure components, we can then examine and analyze our results and come up with a conclusion of which solvent is the best at separating mixtures.

Statement of the Problem:

What is the best solvent in separating a mixture into its pure components?
We will be using these solvents: Water (H2O), Methanol (CH3OH), Proponol (C3H7OH), Hexane (C6H14)

Hypothesis:

We believe that water (H2O) is the best solvent for separating mixtures into their pure components.

Materials:

• Goggles
• Aprons
  
• 24 well plate
  
• Chromatography paper
• Water (H2O),
  
• Methanol (CH3OH)
  
• Proponol (C3H7OH)
  
• Hexane (C6H14)
• Markers (Black, red, blue, green, yellow)
  

Keep goggles on at all times while working with solvents and keep solvents under fume hood.

Procedure:

First we got 4 strips of chromatography paper and labeled each one according to the solvent it was in. We then bent each strip 1.5 cm. at one end of the paper. We marked the creases of the paper with a pencil and then we put 2 dots of black marker ink. We filled 4 of the wells in our 24 well plate with these solvents:Water (H2O), Methanol (CH3OH), Proponol (C3H7OH), and Hexane (C6H14). We placed a strip of chromatography paper in each of the filled wells and examined them as they separated the black marker ink into its pure components. We took notes and wrote down our results. We repeated this procedure with the colors: blue, green, yellow, and red. Also we only used the solvent water in each of the 4 wells for it had the greatest ability to separate a mixture into its pure components. After examining the results we answered the questions on our Chromatography lab papers.

Results (Data):

The results of the lab in order from greatest ability to separate a mixture into its pure components to the least are: Water (H2O), Methanol (CH3OH), Proponol (C3H7OH), Hexane (C6H14). After our experiment we can clearly conclude that Water (H2O) is the best solvent for separating a mixture into their pure components. As you can see on the left side of the photo below, water went all the way across the chromatography paper separating the mixture very well.

Conclusions:

After examining our results we can conclude that our hypothesis was correct and Water (H2O) has the greatest ability to separate a mixture into its pure components. The results of the lab in order from greatest ability to separate a mixture into its pue components to the least are: Water (H2O), Methanol (CH3OH), Proponol (C3H7OH), Hexane (C6H14). I have learned that water has a great ability for separating mixtures into their pure components and Hexane (C6H14) has a poor ability for separating mixtures into their pure components.

1. The solvents that produced the best separation of ink to the least are: Water (H2O), Methanol (CH3OH), Proponol (C3H7OH), Hexane (C6H14)

2. Some solvents worked better than others did on our ink because they are less dense.

3. The ink in the black overhead pen is a mixture of polar molecules, because as the time goes by the different colors appear down the chromatography paper.

4. Hexane (C6H14) would not be an appropriate solvent choice, because it does not separate pigments very well.

5. All colors should be classified as mixtures, because the all had colors in them.

6. Chromatography is a technique for seperating components of a mixture by placing the mixture in a mobile phase that is passed over a stationary phase.