[Chem] Balancing Redox Eqn Any Diff from Regular?

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SUMMARY

The discussion focuses on balancing a redox equation involving silver (Ag), hydrogen ions (H+), and nitrate ions (NO3-). The user initially attempted to balance the equation using conventional methods but arrived at incorrect coefficients. The correct balancing, as per the text, is 3 + 4 + 1 -> 3 + 2 + 1. The key takeaway is the importance of using the ion-electron method, which involves separating the reaction into oxidation and reduction halves, balancing elements, and ensuring charge equality through electron cancellation.

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  • Understanding of redox reactions and oxidation states
  • Familiarity with the ion-electron method for balancing equations
  • Knowledge of basic chemical equations and stoichiometry
  • Ability to identify oxidation and reduction processes in chemical reactions
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Homework Statement



Balance this redox equation.

Homework Equations



Ag + H^{+} + NO_{3} ^{-} \rightarrow Ag^{+} + H_{2}O + NO


The Attempt at a Solution



Using a conventional balancing mechanism I got these coefficients:

1 + 8 + 2 -> 1 + 4 + 2

but the correct answer according to the text is:

3 + 4 + 1 -> 3 + 2 + 1

I am guessing my answer is wrong because of something to do with the oxidation numbers... but what exactly is the problem? Are the oxidation numbers for each of the elements supposed to remain the same on both sides of the eqn? Are they supposed to change? My last chem class was a couple years ago so I don't quite remember :)

Thank you very much!
 
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No.Oxidation no. shoudnt be equal but the increase/decrease ratio of ON has to be equal.TO escape from this increase/decrease thing we use another way of balancing called ION ELECTRON method. IN this we break the reaction into 2 halves : Oxidation and reduction. Then we balance the elemets(apart from H and O) and then balance O and then lastly H.We have to balance charges and also multiply the 2 equations with suitable coeffecients so that the electrons you have added(to make charge equal) cancel out.
 

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