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Understanding Redox Reactions through Oxidation Numbers

This resource explores the concept of redox reactions by analyzing the changes in oxidation numbers. It examines three specific reactions: the production of ammonia from nitrogen and hydrogen, the reaction between magnesium and iron(III) nitrate, and the reaction of manganese dioxide with hydrochloric acid. In each case, we identify which elements have been oxidized (increase in oxidation number) and which have been reduced (decrease in oxidation number). By understanding these changes, learners can gain valuable insights into the nature of chemical reactions.

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Understanding Redox Reactions through Oxidation Numbers

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  1. Starter w.c. 31.10.11 In the following redox reactions use oxidation numbers to explain what has been oxidised and what has been reduced: N2 + 3H2 2NH3 3Mg + 2Fe(NO3)3  3Mg(NO3)2 + 2Fe MnO2 + 4HCl  MnCl2 + Cl2 + 2H2O

  2. Answers N2 + 3H2 2NH3 0 0 -3 +1 Nitrogen reduced: oxidation number decreases from 0 in N2to -3 in NH3; hydrogen oxidised: oxidation number increases from 0 in H2 to +1 in NH3 3Mg + 2Fe(NO3)3  3Mg(NO3)2 + 2Fe 0 +3 +5 -2 +2 +5 -2 0 Iron reduced: oxidation number decreases from +3 in Fe(NO3)3to 0 in Fe; magnesium oxidised: oxidation number increases from 0 in Mgto +2 in Mg(NO3)2

  3. Answers c. MnO2+ 4HCl  MnCl2 + Cl2 + 2H2O +4 -2 +1 -1 +2 -1 0 +1 -2 Manganese reduced: oxidation number decreases from +4 in MnO2to +2 in MnCl2; chlorine oxidised: oxidation number increases from -1 in HClto 0 in Cl2

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