For the following redox reaction, identify the oxidizing agent and the reducing agent.
Cu(NO3)2 (aq) + Mg(s) ® Cu(s) + Mg(NO3)2 (aq
1. Go through and assign oxidation numbers to each element.
2. Mark those that have changed.
3. Determine the ones that lost/gained electrons.
4. The oxidizing agent gains electrons; the reducing agent loses electrons.
Post your work or explain in detail what you don't understand.
My problem is the CU(NO3)2 and Mg(NO3)2
Mg alone is 0 and Cu alone is 0
Ok i think i got it, Cu in the compound is +2 and Mg in the compound is +2
So Cu is the OD and Mg is the RA
Yes, you have it. Good work.
To identify the oxidizing agent and reducing agent in a redox (reduction-oxidation) reaction, we need to determine which species is getting oxidized and which one is getting reduced.
In the given reaction:
Cu(NO3)2 (aq) + Mg(s) → Cu(s) + Mg(NO3)2 (aq)
Cu(NO3)2 (aq) undergoes a change from Cu(II) to Cu(0), while Mg(s) undergoes a change from Mg(0) to Mg(II).
To identify the oxidizing agent, we look for the species that is causing oxidation. In this case, Cu(NO3)2 is getting reduced (going from Cu(II) to Cu(0)), so it cannot be the oxidizing agent.
To identify the reducing agent, we look for the species that is causing reduction. In this case, Mg is getting oxidized (going from Mg(0) to Mg(II)), so it is the reducing agent.
Therefore, the oxidizing agent is Cu(NO3)2 and the reducing agent is Mg.