Question

Question #f7240

Answer 1

Yes, it will.

Explanation:

Hydrogen peroxide, `"H"_2"O"_2`, will reduce gold(III) oxide, `"Au"_2"O"_3`, to gold metal, `"Au"`.

Gold will be reduced from a `+3` **oxidation state in gold(III) oxide, to a `0` oxidation state in gold metal.

At the same time, oxygen will be oxidized from a `-1` oxidation state in hydrogen peroxide to a `0` oxidation state in oxygen gas, `"O"_2`.

As far as I know, hydrogen peroxide acts as a reducing agent in alkaline and acidic solutions, so I'm not sure which is applicable here.

The balanced chemical equation for this reaction looks like this - oxidation states included

`stackrel(color(blue)(+3))("Au"_2)"O"_text(3(s]) + 3"H"_2stackrel(color(blue)(-1))("O")_text(2(aq]) -> 3stackrel(color(blue)(0))("Au")_text((s]) + 3"H"_2"O"_text((l]) + 3stackrel(color(blue)(0))("O")_text(2(g])` `uarr`