Question

In the reaction, $4NH_3 (g) + 5O_2 \rightarrow 4NO(g) + 6H_2O (I)$ When 1 mole of ammonia and 1 mole of $O_2$ are made to react to completion, then

• A. 1.0 mole of $H_2O$ is produced
• B. 1.0 mole of NO will be produced
• C. all the oxygen will be consumed
• D. all the ammonia will be consumed

Answer 1

Answer: (C)

all the oxygen will be consumed

Answer 2

The correct answer is– all the oxygen will be consumed

The chemical reactions would be –

4NH3 + 5O2 → 4NO + 6H2O

Here, 5 mole of Oxygen = 4 mole of Ammonia

So, 1 mole of O2 = 4/5 = 0.8 mole of NH3

By reversing it one can say, 1 mole of NH3 requires 5/4 = 1.25 mole of O2

So, when a reaction between one mole of ammonia and one mole of oxygen is brought to a successful conclusion, all of the oxygen is then consumed.

The charge of nitrogen in ammonia increases from -3 to +2, and the charge of oxygen falls from 0 to -2, making the equation a form of redox reaction. Any elemental compound or atom has an oxidation state of zero. Redox reactions are those in which oxidation and reduction both take place concurrently. Ammonia is undergoing oxidation in this instance, whereas oxygen is undergoing reduction.