Balancing Redox Reactions (another question) help?

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SUMMARY

The discussion focuses on balancing redox reactions using half-reactions, specifically the reaction of zinc with nitric acid (Zn + HNO3 → Zn(NO3)2 + NH4NO3 + H2O). Participants emphasize the importance of identifying oxidation and reduction processes by assigning oxidation numbers (ON) to elements in the reaction. The oxidation number method is highlighted as a reliable approach to determine which species is oxidized and which is reduced, facilitating the balancing of the equation through half-reactions.

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  • Understanding of redox reactions and their components
  • Familiarity with half-reaction method for balancing equations
  • Knowledge of oxidation numbers and their significance in redox chemistry
  • Basic skills in chemical equation manipulation
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  • Study the half-reaction method for balancing redox reactions in detail
  • Learn how to assign oxidation numbers to elements in chemical reactions
  • Practice balancing various redox reactions using the oxidation number method
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Homework Statement


Use half reactions to balance the following redox reactions and underline the oxidizing agent
m) Zn + HNO3 --------> Zn(NO3)2 + NH4NO3 + H2O

Homework Equations


Not applicable

The Attempt at a Solution


I would usually start by breaking down the equation into half reactions, but I'm not actually sure how to do this with this equation, since I have an H2O in there.
 
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If you are not sure what is getting oxidized and what is getting reduced, start assigning oxidation numbers to all elements on both sides of the reaction equation.
 
Borek said:
If you are not sure what is getting oxidized and what is getting reduced, start assigning oxidation numbers to all elements on both sides of the reaction equation.

Yeah, but the question asks me to use half reactions to balance the redox equation, not oxidation numbers. Is there a way to do this using half reactions?
 
There is no problem with balancing using half reactions, but first you have to find out what is being reduced and what is being oxidized. If you don't see it at the first sight, ON are a sure way of finding out.
 
Borek said:
There is no problem with balancing using half reactions, but first you have to find out what is being reduced and what is being oxidized. If you don't see it at the first sight, ON are a sure way of finding out.

How would you use the oxidation numbers to determine what is being oxidized and reduced? Is it to do with the change, so if the oxidation number increases you have an oxidation and if it decreases you have a reduction? I haven't really learned the oxidation method for balancing redox equations in school yet, so I'm still kind of iffy about doing that. Could you explain to me how to determine this?
 

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