Oxidation Number to balance a redox reaction

AI Thread Summary
The discussion focuses on balancing the redox reaction involving chlorine and sodium hydroxide. The oxidation numbers are determined, revealing that chlorine undergoes disproportionation, where one atom is oxidized and another is reduced. The proposed balanced equation is 3Cl2 + 6NaOH -> 5NaCl + NaClO3 + 3H2O. Clarification is sought regarding the concept of "equalizing the oxidation numbers," particularly since sodium's oxidation state remains unchanged. The conversation emphasizes the complexity of balancing redox reactions and the need to understand oxidation states in such processes.
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 - teh 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?
 
Thread 'Confusion regarding a chemical kinetics problem'

Thread 'Confusion regarding a chemical kinetics problem'

TL;DR Summary: cannot find out error in solution proposed. [![question with rate laws][1]][1] Now the rate law for the reaction (i.e reaction rate) can be written as: $$ R= k[N_2O_5] $$ my main question is, WHAT is this reaction equal to? what I mean here is, whether $$k[N_2O_5]= -d[N_2O_5]/dt$$ or is it $$k[N_2O_5]= -1/2 \frac{d}{dt} [N_2O_5] $$ ? The latter seems to be more apt, as the reaction rate must be -1/2 (disappearance rate of N2O5), which adheres to the stoichiometry of the...
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