MadSci Network: Chemistry |
Firstly, a friendly warning regarding any experiments especially those at home. Always avoid arbitrary combination of chemicals... you cannot predict the outcome. As you found out in this case, a reaction can be quite violent. Always investigate the potential for exothermicity, generation of toxic or noxious gases etc. Always proceed with caution and do not forget personal protection (safety glasses for example). Back to your question: The vigorous exotherm you observed was the rapid decompostion of hydrogen peroxide into water and oxygen; 2H2O2 -> 2H2O + O2 This reaction has a whopping DeltaH (enthalpy change) of -99 kJ per mole. The negative sign is the cinvention used to indicate evolution of heat, that is an exothermic reaction. The decomposition was catalyzed by the presence of metal ions (copper sulphate in aqueous solution). It is doubtful that any surprising new compound was created, and evaporating the liquid merely reformed the original constituents, albeit in admixture. The decomposition of hydrogen peroxide is catalyzed just as well by many solid surfaces as ions in solution, for example iron oxide (rust) and manganese dioxide being the most commonly cited cases. I suspect that copper sulphate has similar propeties based on your observation. It is doubtful that any "exchange " of ions took place... perhaps you were anticipating that chloride anions would form ligands to the copper and replace some water molecules. It all depends on the relative concentrations as to the exact species present, and copper chloride complexes tend not to be formed, unless precipitated by the presence of large cations. The reaction rate would of course naturally slow as hydrogen peroxide was "consumed" as the reaction progressed. This is the case with all reactions where reactants are not replenished. You should consult a good undergraduate chemistry text, and look up "reaction order" and "reaction rate constants" Bibliography: I consulted "Advanced Inorganic Chemistry" by F.Albert Cotton & Geoffrey Wilkinson. You can even find some references to other reactions of hydrogen peroxide, including the catalyzed decomposition, in MadSci Network ARCHIVES (you can even learn about rocket engines!) If you are interested to learn more about hydrogen peroxide, I suggest visiting the web site http://www.h2o2.com. Thanks for your questions. STAY SAFE!
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