\\\\(HOCl + H_{2}O_{2}\\overset{H^+}{\\rightarrow}H_{3}O^{+} + Cl^{-} + O_2\\\\)Here, the \\\\(H_2O_2\\\\) act as the reducing agent, as the \\\\(Cl\\\\) has \\\\(+1\\\\) oxidation state of in \\\\(HOCl\\\\) and after reaction with the \\\\(H_2O_2\\\\) , in the presence of the acid, it reduces the \\\\(Cl\\\\) in \\\\(HOCl\\\\) to \\\\(Cl^{-}\\\\) having -1 oxidation state. So, as \\\\(Cl\\\\) oxidation state decreases from the +1 to -1 oxidation state, hence the \\\\(H_2O_2\\\\) is acting as the reducing agent.