I need a way to prove/show that hydrogen peroxide was decomposed through use of catalyst.
I want to ensure that my catalyst: Fe(NOX3)X3 or iron(III) nitrate is a catalyst, not a reactant/ consumed during the reaction.
2HX2OX2(aq)Fe(NOX3)X3(s)→2HX2O(l)+OX2(g)
- When the reaction is happening, I will introduce a wooden glowing splint over the bubbling reaction and the wooden splint glowing brighter or reigniting will show that oxygen is being produced.
Question:
Now, how do I show that water is produced? Would I just boil the product I get after reaction (image above) and put cobalt chloride paper at the water vapour?
Also, if I were to use the orange solution above again as a catalyst (since it still contains iron(III) nitrate), would hydrogen peroxide decompose again? If so, is there a way to put iron(III) nitrate back to its solid state? or any way to reuse as catalyst?
Edit:
If it is easier to answer, it doesn't have to be with iron(III) nitrate. I have an option to use manganese dioxide, which is another catalyst that I can substitute for iron(III) nitrate. I think it should be OK since it does the exact same reaction.
Answer
Detection of oxygen: Detection of OX2 by a glowing splint is a good way to detect the oxygen. Also you could capture the gas by a simple fixture e.g. and demonstrate the volume change in the receiver. This way you can actually measure moles OX2 produced (by PV=nRT) then moles HX2OX2 decomposed stoichiometrically by the formula you've written.
Choice of catalyst: Using MnOX2 would be better if you want to make sure you have a catalyst. MnOX2 will not be consumed during the decomposition; I'm not sure about iron(III) nitrate.
Or, detecting change in Fe(NOX3)X3 concentration: Addition of a very small concentration of potassium thiocyanate, KSCN (say 1/100 of your FeX+3 concentration) will yield a deep red product, iron thiocyanate (Fe(SCN)X+2). If you have access to a spectrometer you can measure absorbance of the initial solution's product and the product after decomposing HX2OX2.
Prove water was produced: The best way I can think of is to measure the (subtle) change of density of your solution before and after decomposition. Using MnOX2 would make this easy because you can remove/filter it as a solid after decomposition and thus measure mass/volume of your solution before and after. HX2OX2 and HX2O have small albeit detectably different densities at RT. HX2OX2 is more dense than water so your density should decrease.
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