Reaction Lab

Introduction:

In this reaction lab we had a single displacement reaction that was going on which involved 3CuSo4 + 2 Al which combined with aluminum would form 3Cu + Al2(So4)3 since aluminum is a more active metal than copper it therefore switches place with copper in the reaction and our product then was copper. The limiting reactant is aluminum because in the reaction it is consumed completely. In the lab we had also used aluminum powder which in turn created more surface area in the reaction and caused it to go faster. We can identify that it is a chemical change due to the fact that a precipitate was formed and that there was a color change that took place. In the lab we had also calculated our theoretical, actual and percent yield.

.8gAl * 1 mol Al/26.98mol Al * 3 mol Cu/2 Mol Al * 9 g Cu/ 1 mol Cu=2.83 grams of Cu

our theoretical yield, which is the maximum amount of product given from an amount of reaction , was .9 and our actualy yield, the amount actually produced, is 2.72 gave us a percent yield of 46.46%. The percent yield was to accurately show the real amount of copper given off from the reaction.


List of materials

• Scale
• propane
• Beaker
• CuSO4 * 5H2O
• Bunsen Burner
• Aluminum powder
• Filter paper
• funnel
  

Procedure

1. Medium sized beaker
2. add 75 to 100 ml of water to the beaker.
3. Measure out .7 and 1g of CuSO4*5H2O
4. Stir the solution until the CuSO4 is dissolved
5. Weigh out a piece of paper.
6. Stir frequently allow the reaction to occur until you cant see any more silvery foil pieces.
7. filter out solution then allow to dry for a day
8. weighed the copper in the filter paper
9. then found percent yield, actual and theoretical yield

Data

Aluminum & Copper (II) Sulfate Redox Lab
Substance	Mass (grams)
Cu2SO4●5H2O	15
Al dust	.9
Filter paper	1.3
water	80ml

evaluation
the purpose of this lab was to find out the percent yield with the given amount of solution and material. to find out how much of one substance you will get from another after the process

conclusion
The steps we took were to help us find the percent yield. The percent yield is found to show us how much of an element will come from a solution. This in turn can help us in many ways. Air bags for example can save our lives.

Reactions Lab

Lab Writeup
Types of Reactions:

Combustion: a violently exothermic reaction with oxygen to form oxides.

Single Displacement: where one element Is displaced in a reaction usually metal with another metal

Double Displacement: a reaction where two elements change positions in a reaction.

Synthesis: a chemical reaction in which atoms or simple molecules combine to form a compound that is more complex.

Decomposing: a chemical reaction in which a single compound is broken down to produce two or more simpler substances

Procedure:

1. Obtain 3 Small Test tubes.

2. In first test tube, place small amount of Zinc and about ½ mL ofCUSO4 Solutions.

3. In Second Test tube add about ½ mL Ba(NO3)2 solution to about ½mL of CUSO4 solution.

4. In third test tube place a piece of Magnesium Metal ribbon. Add then about ½ mL of HCL Solution.

5. Light a Bunsen burner. Record observations of the flame

6. Rinse out the first test tube. Add about 2 mL H2O solution. Lightly hear it, then record observations

7. Add a pinch of MnO2 to the h2o2 solution. Lightly heat and record observations

Data:










Data Analysis:
Chemical Equation Types of Reaction Observations

1. ZN + CuSo4 -> Cu + ZN(So4) Single displacement Formation of Copper

2. Ba(NO3)2+Cu(So4) ->Ba(SO4)+CU(NO3)2 Double Displacement Precipitation/Color

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

4. C3H8 + 14O2 -> 3CO2 + 8H2O Combustion Flame, Water given off

5. H2O3 -> H2O + O2 Decomposition Two simpler molecules made

Discussion

In this lab we made several mixtures looking at what kind of reaction they are. In the results we found all of the possible reaction types but synthesis's. we were then able to determine many things from observing these types of reactions such as like wether the reaction was endothermic or exothermic.


Conclusion

We observed five reactions but only four of the five types of reactions were present in this lab, there where two single displacements, one double displacement, and one decomposition Our observations and such are shown above.

Polarity and molecular shape lab

Title: Polarity and Molecular shape lab

Statement of the Problem:

* We are trying construct molecular shapes by looking at their Lewis structure and see if we could determine polarity.

* We found out that there was one resonance structure and a majority of the structures were indeed polar.

Hypothesis: The molecules with hydrogen and oxygen will not be polar due to their electro negativity with other elements.

Materials:

*we had small little tubes like structures that were our bonds, and we had small little round molecules which acted as our central atom.

Procedure:

* We had determine the Lewis structures of following molecules such as SF3 or H2O and the resonance structure SO3 (-2) we then constructed the molecules by the following Lewis structure we had just done for that individual molecule. We then looked at the structure and determined the polarity simply by looking at the structure. There was one resonance structure.

Results (Data):

Octahedral, 90 degree, non-polar, resonance





Tetrahedron, 90-109.5, degrees, non-polar, and non-resonance




Tetrahedron, 109.5 degrees, non-polar, non-resonance




T-Shaped, 120 degrees, polar, and non-resonance




Octahedral, 90 degrees, non-polar, and non-resonance



Tetrahedron, 180 degrees, non-polar, and non-resonance



Tetrahedron, 90-109.5 degrees, and polar and non-resonance


Tetrahedron, 109.5 degrees, non-polar, and non-resonance

Conclusions:

* Our hypothesis was somewhat rejected because there was some molecules with hydrogen that were polar.

We had all learned about how you can determine polarity just by looking at the structure and that we could make Lewis structures and create models by using there Lewis structure

Problems that could have occurred that our calculation of the electro negativity between the molecules so that would throw off our polarity accuracy.

By: James, Marco, Justin

Libby High School Chem lab blog

Title: Chromatography lab

Statement of the Problem:

* We are trying to answer or see what happens when solvents (such as water methanol isopropyl and hexon) separate black pigment and to figure out which solvent was more effective and what colors made up the black pigment.

* We found out that some were more polar others and there was one non-polar solvent.

Hypothesis:

* I hypothesis that hexone because will work well because its non polar and is a complex molecule.

Materials:

*Filter paper, Water, Hexon, isopropyl, methanol

*Black, red, green, yellow and blue markers

* Always wear goggles, do not inhale fumes, wear aprons wash hands after touching solvents.

Procedure:

* We first began with cutting 1cm *8cm strips of filter paper. Fold 1.5 cm from one end then. Then added 3 dots maximum of black marker on filter paper of creased line. Fill 4 holes of well plate with solvents such as water, hexon, isopropyl, and methanol and dipped the folded one of each filter paper end in each hole which contained the solvents then watch what happens for 30 minutes. Part step you repeat the process but instead with different colored markers and the only solvent is water.

Results (Data):

We found out that hypothesis wasn’t correct water was the best and fastest solvent because it’s a polar molecule and is the smallest of the solvent.

Conclusions:

* Our hypothesis is rejected because although hexon is a complex molecule it is non polar which did not allow the pigment to separate it.

We conclude that in order from best to worst: Water, methanol, isopropyl, hexon.

We learned about chromatography paper and how it can separate pigments.

A problem that could have occurred in this lab is that if the amount of solvent could change the rate of separation (of pigment)

Other problems that could have arose are things such as the filter paper was not working properly or maybe the solvents were not working to its full potential.

By: James, Marco, Justin