In the following reaction explain which one is oxidising agent and which one is reducing agent ?
`H_(2)O_(2) + O_(3) rarr 2 O_(2) + H_(2)O`

Explanation

Ozone is behaving as an oxidising agent and `H_(2)O_(2)` is behaving as reducing agent.
`2e^(-) + 2H^(+) + O_(2) rarr O_(2) + 2H_(2)O`
`H_(2)O_(2) rarr O_(2) + 2H^(+) + 2e^(-)`
The above interpretations is further supported on the following grounds.
SRP of `H_(2)O_(2) " is " + 1.77V` while SRP of `O_(3) " is " + 2.07V`. Therefore, `O_(3)` is stronger oxidising agent than `H_(2)O_(2)`