Question

Balance the following equation:
$N{H_3} + C{l_2} \to {N_2} + N{H_4}Cl$

Answer 1

At first we will write about what is given in the question. Then we will write about the law of conservation of mass. Then we will write the steps to balance the equation. In the end we will write the correct balance reaction.

Complete step-by-step answer: Step1. A balanced reaction always follows the law of conservation of mass. This law says that mass can neither be created nor be destroyed. It can only transform from one form to another form. It means that the total number of atoms on the reactant side are equal to the number of individual atoms on the product side.
Step2. There is one atom of Nitrogen on the reactant side and three on the side of the product. Three atoms of the hydrogen on the reactant side and four atoms of the hydrogen on the product side. There are two chlorines on the reactant side and one of the product side.
Step3. So now when the $N{H_3}$is multiplied by the eight and the chlorine by three on the reactant side. Then we would multiply the $N{H_4}Cl$ by the six.
Step4. On the reactant side:
Number of the nitrogen atoms is eight
Number of hydrogen atoms is twenty four
Number of chlorine atoms is six
On product side:
Nitrogen atoms are eight
Hydrogen atoms are twenty four
Chlorine atoms six
So both sides are equal the reaction would b:
$8N{H_3} + 3C{l_2} \to {N_2} + 6N{H_4}Cl$

Note: Ammonia which formula is $N{H_3}$ . It is a colorless gas. It is produced naturally in the human body and in nature. It is very important and vital to the metabolic processes.