Balance each of the following chemical equations:

$$\begin{gathered} \text{a.}{\mathrm{N}}_2\left(g\right)+{\mathrm{O}}_2\left(g\right)⟶\mathrm{NO}\left(g\right) \\ \text{b.}\mathrm{HgO}\left(s\right)⟶\mathrm{Hg}\left(l\right)+{\mathrm{O}}_2\left(g\right) \\ \text{c.}\mathrm{Fe}\left(s\right)+{\mathrm{O}}_2\left(g\right)⟶{\mathrm{Fe}}_2{\mathrm{O}}_3\left(s\right) \\ \text{d.}\mathrm{Na}\left(s\right)+{\mathrm{Cl}}_2\left(g\right)⟶\mathrm{NaCl}\left(s\right) \end{gathered}$$

We have been given an equation.${\mathrm{N}}_2\left(g\right)+{\mathrm{O}}_2\left(g\right)⟶\mathrm{NO}\left(g\right)$

To balance the equation, follow the steps below.

• Count the number of distinct types of atoms in the reactants and products.
• To increase the amount of atoms or molecules in the substances, place coefficients in front of symbols or formulas as needed.
• Reverse the first and second steps until the equation is balanced.

We can achieve this by repeating these procedures.

${\mathrm{N}}_2\left(g\right)+{\mathrm{O}}_2\left(g\right)⟶2\mathrm{NO}\left(g\right)$

We have been given an equation.$\mathrm{HgO}\left(s\right)⟶\mathrm{Hg}\left(l\right)+{\mathrm{O}}_2\left(g\right)$

To balance the equation, follow the steps below.

• Count the number of distinct types of atoms in the reactants and products.
• To increase the amount of atoms or molecules in the substances, place coefficients in front of symbols or formulas as needed.
• Reverse the first and second steps until the equation is balanced.

We can achieve this by repeating these procedures.

$2\mathrm{HgO}\left(s\right)⟶2\mathrm{Hg}\left(l\right)+{\mathrm{O}}_2\left(g\right)$

We have been given an equation.$\mathrm{Fe}\left(s\right)+{\mathrm{O}}_2\left(g\right)⟶{\mathrm{Fe}}_2{\mathrm{O}}_3\left(s\right)$

To balance the equation, follow the steps below.

• Count the number of distinct types of atoms in the reactants and products.
• To increase the amount of atoms or molecules in the substances, place coefficients in front of symbols or formulas as needed.
• Reverse the first and second steps until the equation is balanced.

We can achieve this by repeating these procedures.

$4\mathrm{Fe}\left(s\right)+3{\mathrm{O}}_2\left(g\right)⟶2{\mathrm{Fe}}_2{\mathrm{O}}_3\left(s\right)$

We have been given an equation$\mathrm{Na}\left(s\right)+{\mathrm{Cl}}_2\left(g\right)⟶\mathrm{NaCl}\left(s\right)$

To balance the equation, follow the steps below.

• Count the number of distinct types of atoms in the reactants and products.
• To increase the amount of atoms or molecules in the substances, place coefficients in front of symbols or formulas as needed.
• Reverse the first and second steps until the equation is balanced.

We can achieve this by repeating these procedures.

$2\mathrm{Na}\left(s\right)+{\mathrm{Cl}}_2\left(g\right)⟶2\mathrm{NaCl}\left(s\right)$