To analyze the redox reaction 3 NO + Hg → 2 NO2 + HgO, we need to assign oxidation numbers to the elements involved.
Let’s break it down:
- In nitric oxide (NO), nitrogen (N) has an oxidation number of +2 and oxygen (O) has an oxidation number of -2.
- In nitric dioxide (NO2), nitrogen (N) has an oxidation number of +4.
- In mercury(II) oxide (HgO), mercury (Hg) has an oxidation number of +2 and oxygen (O) remains at -2.
Now, let’s summarize the oxidation states before and after the reaction:
- For NO: N is +2 and O is -2.
- For NO2: N is +4 (increased from +2 to +4).
- For Hg: Hg is 0 (elemental state) and becomes +2 in HgO.
From this analysis:
- The element oxidized is nitrogen (N) because its oxidation number increases from +2 to +4.
- The element reduced is mercury (Hg) because its oxidation number decreases from 0 to +2.
Now, identify the agents:
- Since nitrogen is oxidized, it acts as the reducing agent.
- Since mercury is reduced, it serves as the oxidizing agent.
In conclusion:
- Oxidized element: Nitrogen (N)
- Reduced element: Mercury (Hg)
- Oxidizing agent: Mercury (Hg)
- Reducing agent: Nitrogen (N)