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: a.N 2 + 3H 2.

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Starter w.c In the following redox reactions use oxidation numbers to explain what has been oxidised and what has been reduced: a.N 2 + 3H 2  2NH 3 b.3Mg + 2Fe(NO 3 ) 3  3Mg(NO 3 ) 2 + 2Fe c.MnO 2 + 4HCl  MnCl 2 + Cl 2 + 2H 2 O

Answers a.N 2 + 3H 2  2NH Nitrogen reduced: oxidation number decreases from 0 in N 2 to -3 in NH 3; hydrogen oxidised: oxidation number increases from 0 in H 2 to +1 in NH 3 3Mg + 2Fe(NO 3 ) 3  3Mg(NO 3 ) 2 + 2Fe Iron reduced: oxidation number decreases from +3 in Fe(NO 3 ) 3 to 0 in Fe ; magnesium oxidised: oxidation number increases from 0 in Mg to +2 in Mg(NO 3 ) 2

Answers c. MnO 2 + 4HCl  MnCl 2 + Cl 2 + 2H 2 O Manganese reduced: oxidation number decreases from +4 in MnO 2 to +2 in MnCl 2; chlorine oxidised: oxidation number increases from -1 in HCl to 0 in Cl 2