# Question #f7240

Mar 12, 2016

Yes, it will.

#### Explanation:

Hydrogen peroxide, ${\text{H"_2"O}}_{2}$, will reduce gold(III) oxide, ${\text{Au"_2"O}}_{3}$, to gold metal, $\text{Au}$.

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, ${\text{O}}_{2}$.

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

${\stackrel{\textcolor{b l u e}{+ 3}}{\text{Au"_2)"O"_text(3(s]) + 3"H"_2stackrel(color(blue)(-1))("O")_text(2(aq]) -> 3stackrel(color(blue)(0))("Au")_text((s]) + 3"H"_2"O"_text((l]) + 3stackrel(color(blue)(0))("O}}}_{\textrm{2 \left(g\right]}}$ $\uparrow$