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The following skeletal oxidation-reduction reaction occurs under acidic conditions. Write the balanced REDUCTION half reaction.Fe + SO42- Fe2+ + SO2 |
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Answer» Answer: An example is given below of the reaction of iron(III) sulfate with magnesium. Unbalanced reaction: Mg(s) + Fe2(SO4)3(aq) → Fe(s) + MGSO4(aq) This reaction is split into two half-reactions, one that involves oxidation and one that involves reduction. Reduction: Fe3+(aq) + 3e– → Fe(s) Oxidation: Mg(s) → Mg2+(aq) + 2e– This pair of half-reactions can be balanced by ENSURING that both have the same NUMBER of electrons. To do this, multiply the oxidation half-reaction by 3 and the reduction half-reaction by 2, so that each half-reaction has 6e–. 2 Fe3+(aq) + 6e– → 2 Fe(s) 3 Mg(s) → 3 Mg2+(aq) + 6e– Adding these two half reactions TOGETHER gives the balanced equation: 2 Fe3+(aq) + 3 Mg(s) → 2 Fe(s) + 3 Mg2+(aq) Notice that the sulfate ion (SO42-) is ignored. This is because it does not take part in the reaction; it is a spectator ion. |
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