Can ethanol be oxidized by hydrogen peroxide? Is it possible to oxidize ethanol to acetic acid with hydrogen peroxide and if yes then 
under what circumstances? I tried it in room temperature but either concentration was too small (of hydrogen peroxide(3%)) or I couldn't quite precisely read the the results of the universal indicator. I also tried heating it up, but it didn't change anything. The color stayed the same (of indicator). Can someone please explain me if the mistake was in my experiment (if the reaction can happen in room temperature) or the reaction needs some specific catalyst or other conditions.
The reaction would be:  

\begin{align}
\ce{\underset{(ethanol)}{C2H6O} + H2O2 &amp;-&gt; 
  \underset{(aldehyde)}{C2H4O} + 2H2O}\\
\ce{\underset{(aldehyde)}{C2H4O} + H2O2 &amp;-&gt; 
  \underset{(acetic acid)}{C2H4O2} + H2O}
\end{align}  

Or the reaction without the middle part (since aldehyde will try to oxidize faster then ethanol) would be:  

$$\ce{C2H6O + 2H2O2 -&gt; C2H4O2 + 3H2O}$$
First things first: Don't mess with higher concentrations of hydrogen peroxide unless you are a trained and well-equipped chemist. We're talking "steel-reinforced gauntlets" here. This chemical is as volatile as nitroglycerine.

At 3% you have mostly de-ionized water and for good reason. Hydrogen peroxide is extremely, violently unstable, and is just as likely to oxidize anything else than what you actually intend to react it with.

Anything above a concentration of 30% is very dangerous. Above 60% is suicidal in ill-equipped scenarios. 100% is a hypothetical, and is in essence a potential component of rocket fuel.

So, yes it will work. You may lose a hand, but it will work.