NH3(g) + 2O2 (g) = HNO3 (aq) + H2O (l)
How do I calculate the oxidation states of Nitrogen and figure out if it is reduced, oxidized or neither?
14 years ago
14 years ago
Thank you for the link! Here is my answer below. I am not sure if I am figuring it right. Please advise.
NH3(g) + 2O2 (g) = HNO3 (aq) + H2O (l)
N is -3,H3 is +1, 2o2 is 0,
H is +1, N is X ??, O3 is -2, H2O is -2
Therefore X=-2
I am not sure how to figure N. Is it X or is N include NO3?
and it is
Oxidized
1 year ago
To calculate the oxidation states of nitrogen (N) in a compound, you can use the following guidelines:
1. The oxidation state of a neutral atom is 0.
2. The sum of the oxidation states in a molecule or ion must equal the overall charge of the species.
3. Oxygen (O) generally has an oxidation state of -2, unless it is in a peroxide where it is -1. Hydrogen (H) usually has an oxidation state of +1.
Let's apply these rules to the reaction NH3(g) + 2O2(g) = HNO3(aq) + H2O(l):
1. Start by assigning an oxidation state of 0 to H2O, since hydrogen and oxygen are in their usual oxidation states: H2O(l) --> 0
2. Now, consider NH3. Since hydrogen usually has an oxidation state of +1, and there are three hydrogens in NH3, the total oxidation state contributed by hydrogen is +3. This leaves N with an oxidation state of -3, as it balances out the charge: NH3(g) --> H3^+ + N^3- (-3 + 3 = 0)
3. Next, examine O2. Oxygen typically has an oxidation state of -2, and since there are two oxygens, the total oxidation state contributed by oxygen is -4. This leaves N with an oxidation state of +5, considering the overall charge: O2(g) --> 2O^- + 2e^- (-4 + 4 = 0)
4. Finally, look at HNO3. Since hydrogen usually has an oxidation state of +1, and there are three hydrogens in HNO3, the total oxidation state contributed by hydrogen is +3. Oxygen typically has an oxidation state of -2, and there are three oxygens in HNO3, making the total oxidation state contributed by oxygen -6. Considering the overall charge, we can determine the oxidation state of N: HNO3(aq) --> 3H^+ + NO3^- (+1 × 3 + (-6) = -2)
Now that we have the oxidation states of nitrogen in NH3 and HNO3, we can compare them:
In NH3, nitrogen has an oxidation state of -3. In HNO3, nitrogen has an oxidation state of +5. Nitrogen is therefore oxidized (its oxidation state has increased) from -3 to +5 during the reaction.
Please note that this is a basic method for calculating oxidation states, and in some cases, exceptions and special rules may apply.