Solved: Redox, Catalyzed Decomposition Reaction

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Discussion Overview

The discussion revolves around the classification of a chemical reaction involving ammonium nitrate (NH4NO3) and zinc (Zn) in the presence of water and a chlorine catalyst. Participants explore whether this reaction is solely a redox reaction or if it involves decomposition and other steps. The context includes theoretical and experimental aspects of chemical reactions.

Discussion Character

  • Exploratory
  • Technical explanation
  • Debate/contested

Main Points Raised

  • Some participants propose that the reaction is a redox reaction where zinc is oxidized to zinc oxide (ZnO) and nitrogen in ammonium nitrate is reduced to nitrous oxide (N2O).
  • Others question whether there is a decomposition reaction occurring prior to the redox process, suggesting that the addition of water facilitates contact between reactants.
  • A participant mentions that the presence of chlorine gas (Cl2) is not necessary for the reaction to proceed, indicating that the change in NH4NO3 is due to the oxidation of zinc.
  • Another participant outlines a sequence of reactions, suggesting that water dissolves salts to form ammonium ions, which may lead to further reactions involving zinc and nitrate ions.
  • There is mention of ammonium chloride (NH4Cl) potentially reacting with dilute acid to produce hydrochloric acid (HCl), which could influence the reaction dynamics.

Areas of Agreement / Disagreement

Participants express differing views on whether the reaction is solely a redox reaction or if it involves multiple steps, including decomposition. The discussion remains unresolved regarding the exact nature of the reactions taking place.

Contextual Notes

Some participants highlight the complexity of the reaction mechanisms and the potential influence of reactant concentrations on the products formed. There are also unresolved questions about the role of the catalyst and the specific conditions required for the reactions.

Who May Find This Useful

This discussion may be of interest to those studying chemical reactions, particularly in the context of redox processes, decomposition reactions, and the role of catalysts in chemical systems.

Soley101
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[SOLVED] Quickie; what reaction

I'm trying to find out what type of reaction this is.
a drop of water is added to a small pile of chemicals in a dish, after a few seconds, a blue flame and smoke is produced.

NH4NO3 reacts to form (with chlorine as catalyst) N2O and water

the experiment is called oxidation of zinc, so another equation is Zn and NH4NO3 react to form ZnO and water.

this is definitely a redox reaction right? but is there not a decompostition reaction first that allows the zinc to oxidize? so really, this reaction is oxidation reduction, catlyzed, and decomposition?
 
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Ammonium cloride.
Ammonium nitrate.
Zinc.
I have seen this formula before, it is called Negative X.
http://www.unitednuclear.com/negx.htm"
 
Last edited by a moderator:
but is the reaction soley redox, or are the steps different reactions as well.
 
the drop of water I suspect is only to get the materials in close contact

there seems to be no Cl2 (is a gas) around to promote the decompostion, otherwise it would already make the N2O and water (without the drop of water and the mixture would be wet)

therefore the change in NH4NO3 must be due to the oxidation of Zn

btw there is no NO2 in your 3rd equation

so I would say it is a pure redox reaction with Zn being oxidized to ZnO and the N in NH4NO3 reduced to N2O
 
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hmmm, thanks, ill have to look into decompositon in more detail next time, merci.
 
de rien
 
Soley101 said:
I'm trying to find out what type of reaction this is.
a drop of water is added to a small pile of chemicals in a dish, after a few seconds, a blue flame and smoke is produced.

NH4NO3 reacts to form (with chlorine as catalyst) N2O and water

the experiment is called oxidation of zinc, so another equation is Zn and NH4NO3 react to form ZnO and water.

this is definitely a redox reaction right? but is there not a decompostition reaction first that allows the zinc to oxidize? so really, this reaction is oxidation reduction, catlyzed, and decomposition?

1. H2O dissolves the salts forming NH4+ ions which make the solution acid.
2. Zn reacts with NO3- (and probably even with water) now that the solution is acid; the products are Zn++ and NO, N2O, N2 or NH4+, depending on the relative concentrations of Zn and NO3-: NO and N2O when NO3- is in eccess, NH4+ when Zn is in eccess. Also N2O is generated by the heat decomposition of NH4NO3 itself:
NH4NO3 + heat --> N2O + 2H2O.
3. The heat generated in reaction 2. starts the reaction between solid Zn and solid NH4NO3 that now proceeds on its own.
NH4Cl is used as catalist, but I don't know its exact functioning.
 
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It could be that the NH4Cl reacts with the dilute acid to produce HCl. The HNO3 present would react with it producing an http://en.wikipedia.org/wiki/Aqua_regia" type reagent.
 
Last edited by a moderator:
who new this was so difficult, i am trying to simplify it , thanks for yer help maties.
 

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