Balancing Redox Reactions (another question) help?

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Discussion Overview

The discussion revolves around balancing redox reactions using half reactions, specifically focusing on a given equation involving zinc and nitric acid. Participants explore methods for identifying oxidation and reduction processes within the reaction.

Discussion Character

  • Homework-related
  • Technical explanation
  • Conceptual clarification

Main Points Raised

  • One participant expresses uncertainty about how to break down the redox reaction into half reactions, particularly due to the presence of water in the equation.
  • Another participant suggests assigning oxidation numbers to all elements on both sides of the reaction to identify what is being oxidized and reduced.
  • A participant reiterates the importance of using half reactions for balancing but emphasizes the need to first identify the oxidized and reduced species.
  • There is a query about how to use oxidation numbers to determine oxidation and reduction, with a participant seeking clarification on the method since they have not learned it in school yet.
  • One response indicates that understanding the oxidation numbers calculation is crucial and suggests focusing on that aspect without needing to read all details.

Areas of Agreement / Disagreement

Participants generally agree that identifying oxidation and reduction is essential for balancing redox reactions, but there is no consensus on the best approach to achieve this, as some prefer half reactions while others suggest oxidation numbers.

Contextual Notes

Participants express varying levels of familiarity with oxidation numbers and half reactions, indicating a potential gap in understanding the methods for balancing redox reactions.

kshah93
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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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