91Ó°ÊÓ

The oxidation states for equation (1) are shown below,

$\stackrel{\mathbf{0}}{\mathbf{Cl}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{+}{\stackrel{\mathbf{0}}{\mathbf{O}}}_{\mathbf{3}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{→}\stackrel{\mathbf{+}\mathbf{1}}{\mathbf{Cl}}\stackrel{\mathbf{−}\mathbf{1}}{\mathbf{O}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{+}{\stackrel{\mathbf{0}}{\mathbf{O}}}_{\mathbf{2}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}$

From the equation, it can be concluded that oxidation state of chlorine increases from 0 to +1 and the oxidation state of oxygen decreases from 0 to -1. Thus, the equation (1) undergoes oxidation-reduction reaction.

The oxidation states for equation (2) are shown below,

$\stackrel{\mathbf{+}\mathbf{1}}{\mathbf{Cl}}\stackrel{\mathbf{−}\mathbf{1}}{\mathbf{O}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{+}\stackrel{\mathbf{+}\mathbf{1}}{\mathbf{Cl}}\stackrel{\mathbf{−}\mathbf{1}}{\mathbf{O}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{→}{\stackrel{\mathbf{+}\mathbf{1}}{\mathbf{Cl}}}_{\mathbf{2}}{\stackrel{\mathbf{−}\mathbf{1}}{\mathbf{O}}}_{\mathbf{2}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}$

From the equation, it can be concluded that there is no change in the oxidation states of reactants and products. Thus, the equation (2) does not undergoes oxidation-reduction reaction.

The oxidation states for equation (3) are shown below,

${\stackrel{\mathbf{+}\mathbf{1}}{\mathbf{Cl}}}_{\mathbf{2}}{\stackrel{\mathbf{−}\mathbf{1}}{\mathbf{O}}}_{\mathbf{2}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\stackrel{\mathbf{light}}{\mathbf{→}}\mathbf{+}\mathbf{2}\stackrel{\mathbf{0}}{\mathbf{Cl}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{→}{\stackrel{\mathbf{0}}{\mathbf{O}}}_{\mathbf{2}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}$

From the equation, it can be concluded that oxidation state of oxygen increases from -1 to 0 and the oxidation state of chlorine decreases from +1 to 0. Thus, the equation (3) undergoes oxidation-reduction reaction.

The oxidation states for equation (4) are shown below,

$\stackrel{\mathbf{+}\mathbf{1}}{\mathbf{Cl}}\stackrel{\mathbf{−}\mathbf{1}}{\mathbf{O}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{+}\stackrel{\mathbf{−}\mathbf{1}}{\mathbf{O}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{→}\stackrel{\mathbf{0}}{\mathbf{Cl}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{+}{\stackrel{\mathbf{0}}{\mathbf{O}}}_{\mathbf{2}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}$

From the equation, it can be concluded that oxidation state of oxygen increases from -1 to 0 and the oxidation state of chlorine decreases from +1 to 0. Thus, the equation (4) undergoes oxidation-reduction reaction.

The overall equation is,