Question

Complete the chemical equation and balance them

$\mathrm{AgCl}\left(\mathrm{s}\right)\stackrel{\mathrm{light}}{\to }\mathrm{Ag}\left(\mathrm{s}\right)+\mathrm{\_\_\_\_\_\_\_\_}$

Answer 1

A decomposition reaction occurs when one reactant breaks into two or more products.

When silver chloride is exposed to light, it decomposes into silver and chlorine gas.

$\mathrm{AgCl}\left(\mathrm{s}\right)\stackrel{\mathrm{light}}{\to }\mathrm{Ag}\left(\mathrm{s}\right)+{\mathrm{Cl}}_2\left(\mathrm{g}\right)$

Step 1:

Number of atoms in LHS, Ag = 1 atom, Cl = 1 atom

Number of atoms in RHS, Ag = 1 atom, Cl = 2 atoms

There is an extra atom of chlorine on the product side.

Step 2:

Multiply reactant by 2

$2\mathrm{AgCl}\left(\mathrm{s}\right)\stackrel{\mathrm{light}}{\to }\mathrm{Ag}\left(\mathrm{s}\right)+{\mathrm{Cl}}_2\left(\mathrm{g}\right)$

Now in LHS, Ag = 2 atoms, Cl = 2 atoms

In RHS, Ag = 1 atom, Cl = 2 atoms

Step 3:

Multiply Silver in product side by 2

$2\mathrm{AgCl}\left(\mathrm{s}\right)\stackrel{\mathrm{light}}{\to }2\mathrm{Ag}\left(\mathrm{s}\right)+{\mathrm{Cl}}_2\left(\mathrm{g}\right)$

Now in LHS, Ag = 2 atoms, Cl = 2 atoms

In RHS, Ag = 2 atom, Cl = 2 atoms

Therefore, the balanced equation is $2\mathrm{AgCl}\left(\mathrm{s}\right)\stackrel{\mathrm{light}}{\to }2\mathrm{Ag}\left(\mathrm{s}\right)+{\mathrm{Cl}}_2\left(\mathrm{g}\right)$