Understanding Redox Reactions: Balancing Multiple Reductions and Oxidations

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In the discussed redox reaction, both cadmium (Cd) and nitrogen (N) are reduced, indicating a complex process. It is possible for multiple atoms to be reduced or oxidized simultaneously, but this typically involves separate parallel reactions. For a valid redox reaction, both reduction and oxidation must occur concurrently. The presence of dilute acid, such as HNO3, can facilitate these reactions. Accurate calculation of oxidation numbers is crucial to ensure the balance of the reaction.
hiturtle
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I am supposed to balance the following reaction:
CdS + HNO3 (dil) → Cd(NO3)2 + NO + S + H2O

After writing out all the oxidation numbers for each atom, I found that Cd and N are both reduced (Cd5+ → Cd 1+ and N5+ → N2+).

I am wondering how to approach this problem. Is it possible to have 2 atoms reduced? Is this what the dilute acid does?
 
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Show how you calculated oxidation numbers for Cd and S.

Yes, it may happen that more than one atom gets reduced or oxidized, but in such situations it usually means there are two separate, parallel processes going on - and they can be described by two reaction equations. However, for the redox reaction to proceed you need BOTH reduction and oxidation to be taking place at the same time. So if you have found only elements that are being reduced, there is for sure something wrong.
 
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