Element being oxidized or reduced..

Please help me on how to determine which element is being oxidized or reduced on the following equation for the decomposition of hydrogen peroxide, producing water and oxygen gas.

2H2O2(aq) ----> 2H20(l) + 02(g)

I know the oxidation number for hydrogen is 1+ and peroxide is 2-. In this case, how can I determine which element is being oxidized or reduce.
Please help me.

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this is a so-called disproportionation.

O is being both reduced and oxidized.

Ox# for O in H2O2 is -1 and in H2O -2 and finally in O2 0..

[quote="Frodo"]this is a so-called disproportionation.

O is being both reduced and oxidized.

Ox# for O in H2O2 is -1 and in H2O -2 and finally in O2 0..[/quote]

[color=darkgreen]It's fairly common to make the same species both oxidized and reduced at the same time. My personal favourite is "Iron is dipped in a solution of ferric chloride". :)[/color]

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