Question

What happens when ammonia reacts with chlorine?

Answer 1

$N{H_3}$ is the formula for ammonia, which is a nitrogen-hydrogen compound. Ammonia is a colourless gas with a pungent odour. It's a stable binary hydride and the simplest pnictogen hydride. It's a typical nitrogenous waste, particularly among aquatic organisms.

Complete answer:
Depending on the amount of reactants (ammonia and chlorine) in the reaction mixture, ammonia and chlorine gases react in one of two forms. When there is an excess of ammonia gas, the products are different from when there is an excess of chlorine gas. In this reaction, both chlorine and ammonia are in a gaseous state.
Types of reaction of ammonia and chlorine
According to the amount of ammonia and chlorine gases present, there are two possible reactions. So, depending on the reactions, different products will be offered, which we will go through in depth in this tutorial.
Reaction of excess ammonia with less chlorine
Reaction of excess chlorine with less ammonia
Reaction of excess ammonia with less chlorine
The final products of this reaction are generated in two stages. There is a redox reaction (oxidation redox reaction).
Ammonia reacts with chlorine to create nitrogen gas and hydrogen chloride vapour in the first step. The hydrogen chloride vapour produced will act as an acidic compound, releasing ${H^ + }$ ions into the water.
The hydrogen chloride then combines with the simple ammonia gas to form ammonium chloride, a solid white smog. Ammonia is necessary for the second phase reaction to take place. As a result, the necessary amount of ammonia is very high.
$2N{H_3}\; + {\text{ }}3C{l_2}\; = {\text{ }}{N_2}\; + {\text{ }}6HCl \\\ N{H_3}\; + {\text{ }}HCl{\text{ }} = {\text{ }}N{H_4}Cl \\\ Balanced{\text{ }}equation: \\\ 8N{H_3}\; + {\text{ }}3C{l_2}\; = {\text{ }}{N_2}\; + {\text{ }}6N{H_4}Cl \\\$
Reaction of excess chlorine with less ammonia
Nitrogen trichloride ( $NC{l_3}$ ) and hydrogen chloride vapour are formed when ammonia reacts with chlorine. There is a redox reaction, as well.
$Balanced{\text{ }}equation: \\\ 2N{H_3}\; + {\text{ }}3C{l_2}\; = {\text{ }}2NC{l_3}\; + {\text{ }}6HCl \\\$
Nitrogen trichloride is a pungent-smelling yellow oily liquid.
Chlorine is reduced and oxidised in this reaction. As a result, we have a disproportionate reaction. The chlorine oxidation number (O) is now $- 1$ and $+ 1$ . When products are given, there is no change in nitrogen oxidation number.

Note:
Ammonia is a flammable gas that is poisonous if inhaled, causing coughing and respiratory arrest, as well as serious skin burns and eye injury. It is also toxic to marine life. Chlorine gas can cause intense fires, it can be oxidised, it can cause serious skin burns and eye injury, it can be lethal if inhaled, and it is harmful to marine life.