2 zinc zn or aluminum al and copper ii sulfate cuso4

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Unformatted text preview: think they were? Balance the equation. 4. Potassium Perchlorate In a test tube, place about one scoopula full of potassium perchlorate (KClO 3 ) and a little bit (about a pea size) of manganese dioxide (a catalyst). Shake the test tube to mix the contents. Using proper procedures, heat the test tube and its contents over a Bunsen burner and note the reaction. Test the gases in the test tube with a glowing splint. Single Replacement Reactions: 1. Copper (Cu) Metal in Silver Nitrate (AgNO3 ) (conclusion) Take careful observations of the test tube you prepared earlier with the copper metal and the silver nitrate solution. If copper has a +2 charge, determine the formulas of the products. Balance the equation. 2. Zinc (Zn) or Aluminum (Al) and Copper (II) Sulfate (Cu(SO4 ).6H2 O) (conclusion) Take careful observations of the test tube you prepared earlier with the zinc or aluminum metal and the copper (II) sulfate solution. If zinc has a +2 charge (you should already know the charge of aluminum if this is the reagent you used), determine the formulas of the products. Balance the equation. Double Replacement Reactions: 1. Hydrochloric acid (HCl) and sodium hydroxide (NaOH) The reaction between an acid and a base is called a “neutralization reaction”, and typically results in the formation of some type of salt and water. Add about half a milliliter of 2.0 M HCl to about half a milliliter of 2.0 M NaOH. Note any temperature changes that occur. Balance the equation. 2. Reactions of Salt Solutions Dakota State University Page 65 of 232 Experiment 3: Chemical Reactions General Chemistry I and II Lab Manual You’ll find a table for this section of the experiment listing several salts (use 0.4 M salt solutions). Fill in the table, mixing 2-3 drops of each salt solution with every other solution in the table in separate SMALL test tubes (that is, one test tube for each salt solution pair). If there is no noticeable change after careful observation, write N.R. (“No Reaction”) in the table. Balance all chemical equations; if no reaction seemed to occur, simply write “N.R.” as the product. Dakota State University Page 66 of 232 Experiment 3: Chemical Reactions General Chemistry I and II Lab Manual Data Page Copper and Silver Nitrate Solution: Reactant Observations Copper Silver Nitrate Zinc or Aluminum in Copper (II) Sulfate Solution: Reactant Zinc or Aluminum Copper Sulfate Observations II Cyclohexene and Bromine: Reactant Cyclohexene Observations Bromine Observations of the product: _____ C6 H10 (l) + _____ Br2 (l) à _____ C6 H10 Br2 (l) Dakota State University Page 67 of 232 Experiment 3: Chemical Reactions General Chemistry I and II Lab Manual Magnesium and Oxygen: Reactant Magnesium Observations Oxygen Observations of the product: _____ Mg (s) + _____ O2 (g) _____ Mg__ O__ (s) (HINT! Using charges, figure out the chemical formula for the magnesium oxide first.) Anhydrous Copper (II) Sulfate and Water: Reactant Anhydrous Copper (II) Sulfate Water Observations Observations of the product: _____ CuSO4 (s) + _____ H2 O (l) à _____ CuSO4 .6H2 O (s) Dakota State University Page 68 of 232 Experiment 3: Chemical Reactions General Chemistry I and II Lab Manual Sugar: Reactant Observations Sugar Sulfuric acid (the catalyst) Observations of the products: Product “smoke” Observations “cylinder” _____ C6 H12 O6 (s) à Hydrogen peroxide: Reactant Hydrogen peroxide Observations Manganese Dioxide (the catalyst) Observations of the...
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This note was uploaded on 09/18/2012 for the course CHEMISTRY 1010 taught by Professor Kumar during the Fall '11 term at WPI.

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