Question

Complete and balance the reaction: ${\mathrm{N}}_2+{\mathrm{O}}_2\to \mathrm{\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_}.$

Answer 1

• A chemical reaction is a process in which a given set of substances is transformed into another substance.
• The reaction between $\mathrm{Nitrogen}\left({\mathrm{N}}_2\right)$ and $\mathrm{Oxygen}\left({\mathrm{O}}_2\right)$ leads to the formation of $\mathrm{Nitric}\mathrm{oxide}\left(\mathrm{NO}\right)$
• Chemical equation: $\underset{\mathrm{Nitrogen}}{{\mathrm{N}}_2\left(\mathrm{g}\right)}+\underset{\mathrm{Oxygen}}{{\mathrm{O}}_2\left(\mathrm{g}\right)}\to \underset{\mathrm{Nitric}\mathrm{oxide}}{\mathrm{NO}\left(\mathrm{g}\right)}$

Steps involved in balancing the above chemical equation:

Step 1: Let us count the number of $\mathrm{Nitrogen}$and $\mathrm{Oxygen}$ atoms on both sides of the equation.

Name of the element	Reactants	products
$\mathrm{Nitrogen}$	2	1
$\mathrm{Oxygen}$	2	1

• There are 2 $\mathrm{Nitrogen}$ atoms and 2 $\mathrm{Oxygen}$atoms on the reactant side, but only 1 $\mathrm{Nitrogen}$ and 1 $\mathrm{Oxygen}$ on the product side. So we have to make 2 $\mathrm{Nitrogen}$ atoms and 2 $\mathrm{Oxygen}$ on the product side.

Step 2: Now, Balancing the equation

• Multiply the $\mathrm{Nitric}\mathrm{oxide}$ by 2 and write it as $2\mathrm{NO}$.
• The above equation is now written as : ${\mathrm{N}}_2+{\mathrm{O}}_2\to 2\mathrm{NO}$
• Let us count the number of $\mathrm{Nitrogen}$ and $\mathrm{Oxygen}$ atoms on both sides of the equation.

Name of the element	Nitrogen	Oxygen
Nitrogen	2	2
Oxygen	2	2

Since the number of $\mathrm{Nitrogen}$ and $\mathrm{Oxygen}$ are equal on both sides. Hence equation is balanced.

Balanced chemical equation: $\underset{\mathrm{Nitrogen}}{{\mathrm{N}}_2\left(\mathrm{g}\right)}+\underset{\mathrm{Oxygen}}{{\mathrm{O}}_2\left(\mathrm{g}\right)}\to \underset{\mathrm{Nitric}\mathrm{oxide}}{2\mathrm{NO}\left(\mathrm{g}\right)}$