Oxidation Number to balance a redox reaction

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Discussion Overview

The discussion revolves around balancing a redox reaction involving chlorine and sodium hydroxide, specifically the reaction Cl2 + NaOH -> NaCl + NaClO3 + H2O. Participants explore the oxidation numbers of the involved species and the methodology for balancing the equation.

Discussion Character

  • Homework-related
  • Technical explanation
  • Debate/contested

Main Points Raised

  • One participant suggests starting by determining the oxidation numbers of all species involved in the reaction.
  • Another participant proposes a method to equalize the oxidation numbers of chlorine and sodium, leading to a balanced equation of 3Cl2 + 6NaOH -> 5NaCl + NaClO3 + 3H2O, but expresses uncertainty about the correctness of their approach.
  • A different participant challenges the concept of "equalizing the oxidation numbers," noting that sodium's oxidation number does not change and that it acts as a spectator in the reaction.
  • This participant identifies the reaction as a disproportionation, where chlorine is both oxidized and reduced, and questions how many chlorine atoms are oxidized if one is reduced.

Areas of Agreement / Disagreement

Participants do not reach a consensus on the method for balancing the reaction. There are competing views regarding the treatment of oxidation numbers and the nature of the reaction.

Contextual Notes

There are unresolved aspects regarding the interpretation of oxidation numbers and the balancing process, particularly concerning the role of sodium and the nature of the disproportionation reaction.

agnibho
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Homework Statement


Balance Cl2+NaOH -> NaCl + NaClO3 + H2O
 
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Start by determining the oxidation numbers of all species.
 
Cl02 + Na+1O-2H+1 -> Na+1Cl + Na+1Cl-1O3-2 + H2+1O-2

To equalize the Oxidation Numbers of Cl and Na, 3 atoms of Cl and 6 atoms of Na are required. Thus,
3Cl2 + 6NaOH -> 5NaCl + NaClO3 + xH2O
By inspection x = 3
∴ 3Cl2 + 6NaOH -> 5NaCl + NaClO3 + 3H2O

I think this is correct, but if I have done something wrong please tell me so, as I'm new to this topic.
Thanks in advance.
 
No idea what you mean by "equalize the ON", specially in the context of sodium - ON for sodium doesn't change, and Na+ is only a spectator.

You have Cl(0) on the left and Cl(+1) and Cl(-1) on the right. This is disproportionation - the same element becomes both oxidized and reduced at the same time. Can you tell how many atoms of Cl get oxidized if 1 atom gets reduced?
 

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