Chemistry Lab II 4 28 15 Experiment 27 Oxidation Reduction Reactions The objectives of this lab were to observe and predict the products of oxidation and reduction reactions and to also determine the comparative reactivity of a series of metallic elements Introduction Experimental Section report sheet attached Procedure Part A First a clean and dry 50 mL beaker was obtained and filled with 10 mL of deionized water and this beaker was heated until the water was close to boiling The water was tested with litmus paper and the litmus paper was saved Next a 2 cm piece of Mg ribbon was obtained and was put under a lit bunsen burner The Mg ribbon became white ash This white ash was put into the 50 mL beaker that contained the close to boiling water this was done while simultaneously swirling the wa ter After the successful addition of the white ash the solution was let sit until the end of the lab period Once the lab was nearing its end the solution was tested again with litmus paper The before and after litmus paper tests were observed and recorded on the report sheet Next three clean and dry test tubes were obtained and were labeled 1 3 In the 1st test tube 1 mL of 6 M HCl was added in the 2nd 1 mL of 6 M HNO3 was added and in the 3rd and last test tube 1 mL of concentrated HNO3 was added Then the 3 test tubes were transferred extremely carefully to the fume hood After the successful and safe transfer of the 3 tests tubes a 1 cm strip of copper was added to each of the 3 test tubes The results and observations were recorded on the reports sheet First 1 cm strips of Ni Cu Zn Fe Al and Mg were obtained Next 6 test tubes were obtained and labeled 1 6 Then 1 5 mL 6 M HCl were added into each of the 6 test tubes Each of the 6 metals were polished with sand paper in order to remove any of the oxide coating After the polishing was finished each of the metals were immediately placed into the 6 test tubes containing the 6 M HCl After successfully immediately adding each of the metals to their respective test tubes the test tubes were let sit for 15 seconds Once the allotted time had passed the test tubes were scrutinized and the results were Part B recorded Part C Part 1 First 1 cm strips of Cu Zn Fe and Ni were obtained Next three clean and dry test tubes were obtained and ap proximately 1 mL of 0 2 M NiSO4 were placed into each of three test tubes Then a strip of Cu Zn and Fe were placed in the test tubes each in a separate test tube containing the 1 mL of 0 2 M NiSO4 The solutions that contained each of the metals were let sit for 10 minutes After the allotted time had elapsed observations of the test tubes were made and were recorded on the report sheet After successfully completing this first experiment 9 clean and dry test tubes were obtained and were filled with 1 mL of 0 2 M test solutions Cu NO3 2 Zn NO3 2 and Fe NH4 2 SO4 2 After gathering and filling all of the test tubes Cu Zn Fe and Ni were obtained and their reactivity were tested in each of the aforementioned solutions Cu NO3 2 Zn NO3 2 and Fe NH4 2 SO4 2 The results were observed and the reactivity table on the report sheet was filled Analysis Part A 1 Part A 2 Part B 2 Part C At the end of the laboratory the litmus tests from before and after the experiment were compared and the first litmus test turned was red and therefore acidic and the second litmus test was blue and therefore basic In the balanced reaction with Mg in air the oxidizing agent is O2 because of the fact that oxygen was getting reduced from 0 2 In part A 2 the copper metal reacted vigorous with the concentrated HNO3 and the color initially became green and then it turned into a reddish brown solution Copper reacts less vigorously with 6 M HNO3 and a blue solution was formed in the test tube Copper did not react with 6 M HCl and therefore nothing happened as a result in the test tube In part B2 all of the metals expect Cu reacted with the 6 M HCl The Mg and Al metals reacted the most vigorously with the 6 M HCl The Fe and Zn metals reacted at a very steady rate The Ni metal reacted very slow with the 6 M HCl The metals that had reacted with 6 M HCl in order of decreasing activity was Mg Al Zn Fe Ni The observations that were noticed after the test tubes with the metals were let sit for 10 minutes were if the reaction was present An indication that a reaction was present was a slight fizzing dulling had occurred on the metals that were placed in the solutions and the solution had changed color The decreasing reactivity the metals was Mg Al Zn Fe Ni Cu H and hydrogen the non metal is the least reactive The net ionic equations are written on the attached report sheet along with the filled table of with reactions occurred and also those that had not occurred Conclusion The objectives of this experiment again was to notice and anticipate the products of oxidation and reduction reac tions and to also determine the relative reactivity of a series of metallic elements The use of proper techniques e g thorough cleaning and drying before using all laboratory materials and meticulous addition of metals and solutions into test tubes in order to have successful redox reactions were essential in carrying out the experiment with out failures and errors The objec tives of the lab were achieved and the experiment was a success Questions NaOH per II 1 When sodium metal reacts with oxygen sodium oxide is produced If sodium oxide is dissolved in water then the is produced which is basic and therefore the litmus paper would turn blue 2 Oxygen will slowly oxidize copper metal which becomes copper II ion Patina the green coating is mainly Cop Carbonate CuCO3 caused by slow chemical reactions involving the copper metal and water and carbon dioxide 3 The Fe2 ion works as a reducing agent The product of the oxidation is Fe3 4 a The color would be brown due to the presence of the Iodine ion b The I solution functions as a oxidizing agent because it gains electrons when put into that solution 5 The 6 M HNO3 acts as an oxidizing agent so all of the metals would react with 6 M HNO3 but not all would react with the 6 M HCl 6 The reactions in Part C would all be classified as redox reactions that are single displacement because of the fact that a more active metal displaces a less active …
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