Ozone can be destroyed by the following free radical(s)

The correct option is All of the above.

Ozone ($O_3$) in the stratosphere is highly reactive and can be broken down by various free radicals that act as catalysts in ozone depletion cycles. A general catalytic cycle can be represented by the following chemical equations:
$X+O_3\to \mathrm{XO}+O_2$
$\mathrm{XO}+O\to X+O_2$
Net reaction: $O_3+O\to 2O_2$
Where the catalyst $X$ is a free radical that is regenerated at the end of the cycle, allowing a single radical to destroy thousands of ozone molecules.

Let us examine how each of the given radicals participates in this destruction process:

1. Chlorine radical (Cl):
Chlorine atoms are released in the stratosphere when chlorofluorocarbons (CFCs) decompose under ultraviolet (UV) radiation. The chlorine radical reacts with ozone to form chlorine monoxide ($\mathrm{ClO}$) and oxygen:
$\mathrm{Cl}+O_3\to \mathrm{ClO}+O_2$
The chlorine monoxide then reacts with a free oxygen atom to release the chlorine radical back:
$\mathrm{ClO}+O\to \mathrm{Cl}+O_2$

2. Hydroxyl radicals (OH):
Hydroxyl radicals are generated in the stratosphere from the reaction of excited oxygen atoms with water vapor or methane. They destroy ozone via the following reactions:
$\mathrm{OH}+O_3\to {\mathrm{HO}}_2+O_2$
${\mathrm{HO}}_2+O\to \mathrm{OH}+O_2$

3. Nitric oxide radical (NO):
Nitric oxide is introduced into the stratosphere naturally from nitrous oxide ($N_{2}O$) released from the soil, or anthropogenically from high-altitude aircraft emissions. The catalytic cycle is:
$\mathrm{NO}+O_3\to {\mathrm{NO}}_2+O_2$
${\mathrm{NO}}_2+O\to \mathrm{NO}+O_2$

Since all three radicals—chlorine (Cl), hydroxyl (OH), and nitric oxide (NO)—catalyze the breakdown of ozone, they are all capable of destroying ozone. Therefore, "All of the above" is the correct choice.