Which reagent has been oxidized in the following equation ?

H2(g) + N2(g) === NH3(g)

Didn't we go over this yesterday? You need to learn to do this. I gave you a link. If you will identify your hang up I can help you through it.

To determine which reagent has been oxidized in the given equation, we need to examine the changes in oxidation numbers.

In the reaction:

H2(g) + N2(g) → NH3(g)

We can assign oxidation numbers to the elements involved. Hydrogen (H) typically has an oxidation number of +1, while nitrogen (N) has an oxidation number of 0 in molecular nitrogen (N2) and -3 in ammonia (NH3).

Initially, in H2, hydrogen has an oxidation number of 0, and in N2, nitrogen also has an oxidation number of 0. However, in NH3, hydrogen has an oxidation number of +1, and nitrogen has an oxidation number of -3.

By comparing the oxidation numbers before and after the reaction, we can determine the change. In this case, the oxidation number of hydrogen increased from 0 to +1, while the oxidation number of nitrogen decreased from 0 to -3.

Since the oxidation number of nitrogen decreased, we can conclude that nitrogen has been oxidized. Therefore, the reagent that has been oxidized in this equation is N2.