As a sideproject to another project on yeast viability in beer brewing me and my friend intend to extract ethanol from the beer as it is unable to be consumed due to the location it has been brewed and school policies etc.We were just wondering if any had any ideas on how best to go about this.So far we have used a basic distilation setup in order to extract the ethanol with varying levels of success.However this method isn't very scientifically viable as we keep running into the issue of not being able to get the beer to the right temperature without it either bumping or not getting hot enough to evaporate the ethanol.We do not currently have access to a fractional distilation collumn but are looking into investing in one through the schools chemistry budget.A water bath was also attempted to be used to head the liquid more reliably, however the equipment in the school labs is not precise enough to heat the beer well enough to evaporate the ethanol reliable.

A further note bleach is sodium hypochlorite in aqueous solution. 

There is a 2007 review article by Barni and coworkers on luminol.  They give the Weber formulation of this reagent as follows:

"Prepare 0.5 L of 0.4 M NaOH (8 grams NaOH).  Stock solution A.
Add 10 mL of 30% H2O2 to 490 mL water.  Stock solution B.
Dissolve 0.354 g luminol in 62.5 mL of 0.4 M NaOH, and dilute to a final volume of 500 mL.  Stock solution C (final concentration is 4 mM).
Store solutions A, B, and C at 4°C away from direct light.
Mix 10 mL of each stock with 70 mL of water to obtain 100 mL of working solution.  Decant solution into a vaporizer or sprayer and use immediately as an aerosol.  Wear goggles, gloves, and protective clothing.  Use a respirator, and keep the number of people to a minimum.  Apply in the dark.  Aerate the room after investigation."

Obviously, this could be scaled up or down as needed.  I will try to add some further comments, probably about copper ion as a catalyst, when I am a little less pressed for time.

I added 0.2g solid luminol, 115ml water and 10ml NaOH to make it basic

10 mL NaOH doesn't tell us anything about the amount of NaOH present (was it 1M NaOH solution, or 0.01 M solution?) and this is a crucial information, as it can mean several unit differences in the final pH.

(same about other parts of your text, 10 mL hydrogen peroxide is just half of the information needed, just like 1M CuSO₄)

Perhaps our organikers will have something to add, but bonds in hydrazides (luminol is a hydrazide) are similar to those present in amides and look susceptible to hydrolysis in high/low pH. So yes, could be leaving the solution for a week was not a good idea. If anything, I wouldn't add NaOH.

98% sulfuric acid contains plenty of water stoichiometrically, water has very low mol mass. It's not 100% sure how this reaction happens, what intermediates are in play