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Introduction

Types of Reactions Lab Purpose: To observe chemical change, to write balance equations for the chemical reactions observed, and to identify different types of chemical reactions. Procedure: Prepare a suitable Data Collection Table to record all your observations. * Reaction 1: Reaction of aluminum metal with copper (II) nitrate solution Materials: small beaker, copper (II) nitrate solution and a piece of aluminum strip 1. Place an adequate amount of copper (II) nitrate solution into the beaker 2. Add a piece of Aluminum. 3. Record initial observations in the Data Collection Table. 3. Allow the solution to react with the aluminum for a few minutes. 4. Feel the test-tube. 5. Record final observations at the end of the experiment, after filtering the products when all the other procedures have been completed. 6. Clean Up: A metal pan is to be used to collect all solid materials. * Reaction 2: Reaction between cobalt (II) chloride solution and sodium hydroxide solution. ...read more.

Middle

Add a very small amount, (a few grains) of manganese dioxide to the hydrogen peroxide. 4. When the test tube begins to bubble, place the glowing splint into the mouth of the test tube. 5. Feel the test tube. 6. Record all observations. 7. Clean Up: Do not pour the contents of the test tube down the sink! Pour the contents of the test tube into the waste reservoir. Rinse the test tube thoroughly. Data Collection Before Reaction During Reaction After Reaction Reaction 1: Reaction of Aluminum metal with Copper (II) Nitrate Aluminum: -lustrous -solid -grey in colour -metallic -malleable -odourless Copper (II) Nitrate: -liquid (solution) -blue in colour -transparent -odourless -no odour -bubbling -becomes foggy (translucent) -copper precipitate forms -liquid became whiter in colour -no longer transparent, became translucent -releases heat (exothermic) -brittle, flaky precipitate in the liquid -solid brown in colour (the precipitate) Reaction 2: Reaction between Cobalt (II) Chloride solution and Sodium Hydroxide solution Cobalt (II) ...read more.

Conclusion

Chloride + Sodium Hydroxide --> Cobalt (II) Hydroxide + Sodium Chloride CoCl2(l) + 2NaOH(l) --> Co(OH)2(s) + 2NaCl(s) - Precipitate is formed - Colour change Double Displacement Reaction 3 Magnesium + Oxygen gas --> Magnesium Oxide 2Mg(s) + O2(g) -->2MgO(s) - Combustion - Exothermic reaction Synthesis Reaction 4 Hydrogen Peroxide + Manganese (IV) dioxide --> Oxygen gas + Water H2O2(l) --> O2(g) + H2O(l) - Bubbling - Heat - Exothermic reaction Decomposition Conclusion The purpose of this lab was to observe chemical changes, to write balanced equations, and to identify different types of reactions. Within the following lab, all of the reactions were classified as chemical reactions, because of a colour change, a precipitate forming, combustion, or an exothermic reaction. A balance equation was then written in order to determine the amount of matter within the product in comparison to the reactants that reacted at the start and the types of reactions they resulted in such as single displacement, synthesis, decomposition, and double displacement. Throughout the lab we observed chemical change, used balance equations and identified different types of reactions, therefore the purposed of the lab was achieved. ...read more.

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