example of single replacement reactions
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Answers:Ca + Sn(NO3)2 -----> Sn + Ca(NO3)2 Ag + Ni(NO3)2 ------> no reaction Cu + Pb(NO3)2 ------> no reaction Use the Elecctrochemical Series. http://www.answers.com/topic/electrochemical-series-1 Any element below the series will be replaced by the element on top of the series. Example, since in the series, nickel is below calcium, zinc or aluminum then any of these metals can liberate elemental nickel from any compound that contains nickel. However, since silver or copper is below nickel, then addition of any of these metals to the nickel compound will not produce any reaction. The nickel will remain in ion (compound) form. On the other hand, addition of elemental nickel to a compound of silver or copper will produce elemental silver or copper.
Answers:Combination: the rusting of iron (4Fe + 3O2 2Fe2O3) Decomposition: the production of quicklime (Ca(OH)2 CaO + H2O) Single displacement: the polishing of silverware by soaking with aluminium (2Al + 3Ag2S 6Ag + Al2S3) Double displacement: the extraction of magnesium from seawater (MgCl2 + 2NaOH Mg(OH)2 + 2NaCl) Combustion: burning natural gas for heat (CH4 + 2O2 CO2 + 2H2O)
Answers:Nothing happens. Copper is less active than the protons in water, which is why copper is used for plumbing.
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.