Question

Given a reaction:
$4N{H_3}(g) + 5{O_2}(g) \to 4NO(g) + 6{H_2}O(g)$
When $1$ mole of ammonia and $1$ mole of ${O_2}$ are made to react to completion:
(A) $1.0$ mole of ${H_2}O$ 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

Hint: In order to solve this question, we should first understand the concept of limiting reagent or a limiting agent. In a chemical reaction, the reagent that is completely consumed when the chemical reaction is completed is known as a limiting reagent.

Complete Step by Step Solution:
The amount of product formed is generally limited by the limiting reagent because the reaction cannot continue without the limiting reagent. If one or more than one limiting reagents are present in more quantities needed to react with the limiting reagent, they are known as excess reagents.

In the chemical reaction given in the question, $4$ moles of ammonia react with $5$ moles of oxygen according to the given balanced chemical reaction. If only $1$ mole is present in the reaction, then it will react with only $1.25$ moles of oxygen. But there is only $1$ mole of oxygen available. So, here in this reaction, oxygen is the limiting reagent and it is consumed totally during the chemical reaction.
Therefore, the correct answer is option C.

Note: It is important to note that the limiting reagent should be identified so that we will be able to calculate the percentage yield of a chemical reaction as the theoretical yield is generally defined as the amount of product that is obtained when the limiting reagent reacts completely in the chemical reaction.