Which reagent has been oxidized in the following equation ?
H2(g) + N2(g) === NH3(g)
In the given equation: H2(g) + N2(g) → NH3(g), the reagent that has been oxidized is hydrogen (H2).
In the given equation: H2(g) + N2(g) → NH3(g)
To determine which reagent has been oxidized, we need to look at the oxidation states of the elements in each compound.
1. Hydrogen (H) usually has an oxidation state of +1 when combined with nonmetals.
2. Nitrogen (N) usually has an oxidation state of -3 when combined with hydrogen.
Let's assign the oxidation states:
H2(g) → 2H with an oxidation state of +1 each (total: +2)
N2(g) → 2N with an oxidation state of 0 each (total: 0)
NH3(g) → N with an oxidation state of -3 and H with an oxidation state of +1 each (total: 0)
From the oxidation state changes, we can see that the oxidation state of nitrogen changes from 0 in N2 to -3 in NH3. Therefore, nitrogen has been oxidized in this reaction.
To summarize, the reagent that has been oxidized in the given equation is N2(g).
Oxidation is the loss of electrons.
Do you know know to determine the oxidation state? H on the left is zero and on the right is +1. N on the left is zero and on the right it is -3.
Here is a link that will show you how to calculate the oxidation state.
http://www.chemteam.info/Redox/Redox-Rules.html