Oxidation-Reduction Reactions Desk No. Date Lobo Sec. Name A. Oxidation-Reductio
ID: 498680 • Letter: O
Question
Oxidation-Reduction Reactions Desk No. Date Lobo Sec. Name A. Oxidation-Reduction Reactions 1. Doxidation of magnesium. write a description of the reaction. What did the litmus tests reveal write a balanced equation for the reaction of magnesium in air. Box the oxidizing agent in the equation. 2. oxidation of copper. Describe your observations of each test tube. Comment on the relative oxidizing strengths of the throe acids in the test tubes. 3. A series of redox reactions. On a separate sheet of paper, organize your data to record the test tube number and your observations for the 8 reaction mixtures in Table 27.1. Use the appropriate half-reactions (one for solution A and another for solution B) that appear under Reducing Agents and oxidizing Agents in the Introduction. Add the two half reactions such that the electrons gained by one solution equal the electrons lost by the other-this sum provides the overall balanced equation. oxidizing agent in each writen equation. write a balanced redox equation for each observed reaction: BoK the Submit this with the completed Report Sheet. B. Reactions with Hydronium Ion 1. Reactivity of Ni,cu, zn, Fe, Al, and Mg with H,0 Which metals show a definite reaction with HCI? Record this information on the table in Part Cof the Report Sheet Amange the metals that do react in order of decreasing activity. write a balanced equation for the reaction that occurs between Mg and HvoExplanation / Answer
A. 1. The oxidation of Mg can be representedas follows.
2Mg+O2=2MgO In this reaction metallic Mg(zero ogidation state) is oxidised by areal oxigen and converted to MgO
This reaction can be understood by trating with litmas. If red litmas is aaded then it will be converted to blue litmas . This is because aq. solution of MgoO is alkaline
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