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Answers:There are many, many reactions which do not fit the format of the common synthesis, decomposition and single and double replacement reactions. There are many more reactions which we classify as "redox" reactions, and while single replacement reactions are also redox reactions, there are many redox reactions which are not single replacement reactions. Oxidation-reduction reactions involve the simultaneous transfer of electrons such that one element is being oxidized (loss of electrons, increase in oxidation number), and another element is being reduced (gain of electrons, decrease in oxidation number). 2Fe2O3 + 3C -> 4Fe + 3CO2 In your example, iron is being reduced and carbon is being oxidized. The iron appears to be gaining 3 electrons per atom while the oxidation number decreases (being reduced, so to speak). Carbon appears to be losing four electrons while the oxidation number is increasing from 0 to +4. Keep in mind that in Fe2O3 iron does not have an actual charge of +3, and carbon does not have an actual charge of +4. Those are the oxidation numbers. The electron "transfer" is actually being mitigated by the oxygen which does not change its oxidation number. ----------- Follow up ----------- Typically a single replacement reaction occurs when one metal replaces another one in a compound, or when one halogen replaces another one. In this case the oxygen is originally part of a metal oxide, and then goes to a nonmetal oxide. The general format for single replacement is this: "An element and a compound react to form an element and a compound". I suppose from that standpoint you could call it single replacement.
Answers:To me this is splitting hairs, but a single displacement reaction usually involves a metal displacing a metal ion or a halogen displacing a halide ion. In these cases hydrogen can act as a metallic element. Check out these examples: Mg + 2HCl --> MgCl2 + H2 (magnesium displaces hydrogen) 2Al + 3CuCl2 --> 2AlCl3 + 3Cu (aluminum displaces copper) Cl2 + 2KBr --> 2KCl + Br2 (chlorine displaces bromine) What you've got here is a non-metal, carbon, displacing a metal, iron. Although this IS an oxidation-reduction reaction, I suppose it's not technically classified as single displacment because you don't have a metal displacing a metal or a halogen displacing a halide. The two definitions you're meant to use are probably specific to your particular class. I'd advise you to check your notes or textbook. As for your other question, iron is being reduced and carbon is being oxidized. There are two ways to know this: (1) Iron is "losing oxygen", which was one of the original definitions of reduction, while carbon is "gaining oxygen". (2) Iron's oxidation number decreasees from +3 to 0 while carbon's oxidation number increases from 0 to +4. I hope that helps. Good luck!
Answers:A. Yes. Al is higher in the activity series than Ag. B. No. Fe is a more active metal. C. Yes. Zn is higher in the activity series than Pb. You can check it with the source below.
Answers:No one is doing your homework for you. That is too much.