What is the mass of the H2O2and iron(III) nitrate assuming they’re mostly water and the density of water is 1g/mL?
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Answer:
Detection of oxygen: Detection of O2 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 O2 produced (by PV=nRT) then moles H2O2 decomposed stoichiometrically by the formula you've written.
Choice of catalyst: Using MnO2 would be better if you want to make sure you have a catalyst. MnO2 will not be consumed during the decomposition; I'm not sure about iron(III) nitrate.
Or, detecting change in Fe(NO3)3 concentration: Addition of a very small concentration of potassium thiocyanate, KSCN (say 1/100 of your Fe+3 concentration) will yield a deep red product, iron thiocyanate (Fe(SCN)+2). If you have access to a spectrometer you can measure absorbance of the initial solution's product and the product after decomposing H2O2.
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 MnO2 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. H2O2 and H2O have small albeit detectably different densities at RT. H2O2 is more dense than water so your density should decrease.
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