Reactions Lab

1. Introduction/Background: In this lab we investigated 6 different reactions and determined what types of reactions they were. The different reaction types are
1. Combustion - A rapid combination with oxygen that releases a lot of heat as well as CO2 and water.
2. Synthesis - The combining of two smaller elements or compounds to make larger compounds.
3. Decomposition - The breaking down of larger compounds into smaller elements or compounds.
4. Single Displacement - The replacement of one or more atoms of the same type in a compound with an atom or atoms of a different.
5. Double Displacement - Two compounds exchange an atom or atoms of equal charge, usually metals. (i.e. Ba(NO3)2 and CuSO4 exchanging Cu and Ba)
2. Procedure
1. We obtained three small test tubes.
2. We placed a piece of zinc and about 1/2 ml of CuSO4 solution.
3. In the second test tube we added about 1/2 Ba(NO3)2 solution to about 1/2 of CuSO4 solution.
4. In the third test tube we placed a small piece of magnesium ribbon along with about 1/2 ml of HCl solution.
   
5. Then we lighted a bunsen burner and observed the flame.
6. We then rinsed out the first test tube and put some H2O2 into it. We then heated and observed what happened.
7. After this we added a pinch of MnO2 as a catalyst to the H2)2 solution. We heated it and observed the reaction that followed.
3. Data:

   Reactants	Reactions
   Zinc and Copper Sulfate	The Zinc turns brown as it exchanges places with the copper in the copper sulfate compound. Heat is given off as this single displacement reaction occurs.
   Barium Nitrate and Copper Sulfate	Mixture fizzes up and drops in temperature. Double displacement reaction.
   Magnesium and Hydrochloric acid	Fizzes, turns white, and releases heat and energy. Precipitates sink to the bottom of the test tube. Single displacement.
   Bunsen Burner	Hot and blue flame with occasional orange flames. Combustion reaction
   Hydrogen Peroxide Heated	Boils violently and releases a large amount of oxygen. The mixture remaining is water. Decomposition reaction.
   Hydrogen Peroxide and Manganese Oxide	Boils even more readily and mixture turns black. Double displacement.

4. Data Analysis:
1. Zinc and CuSO4 Zn + CuSO4 --> Cu + ZnCuSO4
2. Barium Nitrate and Copper Sulfate CuSO4 + Ba(NO3)2 --> BaSo4 + Cu(NO3)2
3. Magnesium and HCl Mg + 2HCl --> H2 + MgCl2
4. Propane burning C3H8 + 5O2 --> 4H2O + 3CO2
5. H2O2 heated 2H2O2 --> 2H2O + O2
6. MnO2 and H2O2 MnO2 + 2H2O2 --> MnO2 + 2H2O + O2
5. Results:In doing these experiments and examining the formulas we determined the reaction types
1. Zinc+Copper Sulfate-single displacement
2. Barium Nitrate+Copper Sulfate-double displacement
3. Magnesium+Hydrochloric Acid-single displacement
4. Propane Burning-combustion
5. Hydrogen Peroxide Heated-decomposition
6. Manganese Oxide+Hydrogen Peroxide-decomposition
6. Discussion:
1. In the first reaction zinc replaces copper in copper sulfate because zinc is higher than copper on the activity series.
2. Similarly in the second reaction barium is higher than copper on the activity series.
3. In this reaction magnesium replaces hydrogen which is not a metal but behave similarly to one.
4. Any reaction in which a hydrocarbon rapidly combines with oxygen to produce carbon dioxide and water is a combustion reaction which is how you can identify this.
5. The bonds between the oxygen and hydrogen in hydrogen peroxide is relatively weak which is why when heated it turns to water.
6. This reaction is similar to number 5 but manganese oxide acts as a catalysts and is not changed in the reaction but speeds it up.
7. Conclusion:
1. We concluded that you can determine the type of a reaction not only by observing it but by observing the formula.
2. We also determined the type of reactions. (see results)