Oxidation Numbers: Fe203+3CO to 2Fe+3CO2

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Discussion Overview

The discussion revolves around identifying the oxidation and reduction processes in the chemical reaction Fe2O3 + 3CO -> 2Fe + 3CO2, with a focus on using oxidation numbers to determine which elements are oxidized and reduced. The scope includes theoretical understanding and application of oxidation states in chemical reactions.

Discussion Character

  • Technical explanation
  • Conceptual clarification
  • Debate/contested

Main Points Raised

  • Some participants propose that in the reaction, iron (Fe) is reduced as it gains electrons, while carbon (C) is oxidized as it loses electrons.
  • There is a discussion about the use of periodic table valencies to determine oxidation numbers, with one participant noting that this method may not always be accurate.
  • One participant mentions that while carbon typically has a valency of 4, in this reaction it is represented as 2+, raising questions about the consistency of oxidation states.
  • Another participant confirms that oxygen is always -2 in compounds and highlights that metals can have multiple oxidation states, which may not align with their valency.

Areas of Agreement / Disagreement

Participants generally agree on the identification of oxidation and reduction in the reaction, but there is some uncertainty regarding the application of valency and oxidation numbers, indicating that multiple views on this topic remain.

Contextual Notes

Limitations include the potential inaccuracies in using periodic table valencies to determine oxidation states and the variability of oxidation numbers for certain elements, particularly metals.

markosheehan
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By using oxidation numbers can someone show me what is oxidised and reduced

Fe203+3co->2Fe+3co2
 
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markosheehan said:
By using oxidation numbers can someone show me what is oxidised and reduced

Fe203+3co->2Fe+3co2

Hi Marko,

Making the ion forms explicit, we have:
$$
{Fe^{3+}}_2{0^{2-}}_3+3C^{2+}O^{2-}\to 2Fe+3C^{4+}{O^{2-}}_2
$$
So $Fe$ gains electrons and as such it is reduced.
And $C$ loses electrons, meaning it is oxidized.
 
I like Serena said:
Hi Marko,

Making the ion forms explicit, we have:
$$
{Fe^{3+}}_2{0^{2-}}_3+3C^{2+}O^{2-}\to 2Fe+3C^{4+}{O^{2-}}_2
$$
So $Fe$ gains electrons and as such it is reduced.
And $C$ loses electrons, meaning it is oxidized.

thanks
I usually go to the periodic table and look at the elements valency and then i take this as the oxidation number. this is not always correct though?
for example carbon has a valency of 4 but in the above equation it is 2+.
so you go off the ones you know like oxygen is always -2 and the oxidation number of a compound must always equal zero.
 
markosheehan said:
thanks
I usually go to the periodic table and look at the elements valency and then i take this as the oxidation number. this is not always correct though?
for example carbon has a valency of 4 but in the above equation it is 2+.
so you go off the ones you know like oxygen is always -2 and the oxidation number of a compound must always equal zero.

Yes, in compounds oxygen is always -2.
The metals (that are oxidized) usually have more than one oxidation number, and the valency doesn't even have to be one of them (copper for example).
 

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