Question

Complete the following reaction:
$N{{H}_{3}}+C{{l}_{2}}(excess)\to $

Answer 1

Hint: When chlorine gas is made to react with the ammonia , it reacts vigorously with the ammonia and results in the formation of yellow colored compound which is explosive in nature and the oxidation of the chlorine in that very compound is -3. Now solve the given reaction.

Complete step by step answer:
First of all, let’s discuss the ammonia and chlorine before proceeding to their reaction.
Ammonia is formed by the combination of nitrogen and hydrogen gases. It is colourless gas having a pungent smell. It is lighter than the air and is sparingly soluble in the water and can be easily liquefied due to the strong hydrogen bonding between the molecules.
-In ammonia, the hybridization is $s{{p}^{3}}$ with the bond angle of ${{107}^{\circ }}$ and has pyramidal or distorted tetrahedral geometry.
-On the other hand, chlorine is green-yellow in colour and is a poisonous gas. It is also sparingly soluble in water and is very reactive in nature and reacts very violently with the ammonia. Now considering the statement; When ammonia gas is reacted with the excess of the chlorine gas it results in the formation of the compound i.e. nitrogen trichloride which is yellow in colour along with the formation of the HCl gas . the reaction occurs as;
 $\begin{matrix}
N{{H}_{3}} \\
ammonia \\
\end{matrix}+\begin{matrix}
C{{l}_{2}} \\
(excess) \\
\end{matrix}\to 2HCl+\begin{matrix}
NC{{l}_{3}} \\
\begin{align}
& nitrogen \\
& trichloride \\
\end{align} \\
\end{matrix}$
The nitrogen trichloride, thus, formed is very explosive and very reactive in nature , so, therefore should be properly handled and stored safely.

Note: When ammonia gas is made to react with the excess of chlorine gas, it results in the formation of the nitrogen trichloride and on the contrary if the ammonia gas is taken in the excess , it results in the formation of the ammonium chloride.