jacknife360 Posted March 15, 2006 Posted March 15, 2006 How does hydrogen peroxide (~ 30%) act as an oxidising agent (Co2+ --> Co3+), while at the same time a producing a gas (I assume it's oxygen)? This all happens in acidic solution. I can see how it works if it's in alkaline solution. Thanks for any help.
Tartaglia Posted March 15, 2006 Posted March 15, 2006 H2O2 +2H+ +2e --> 2H2O (H2O2 acting as an oxidant) H2O2 --> 2H+ +2e +O2 (H2O2 acting as a reductant) O2 should be released when H2O2 acts as a reductant, but loads of transition metals catalyse the decomposition of H2O2 and that is where the O2 comes from H2O2 --> H2O +1/2O2
jacknife360 Posted March 15, 2006 Author Posted March 15, 2006 But the H2O2 oxidised the Co 2+ to Co 3+, as well as effervescing. Maybe two simultaneous reactions involving Hydrogen peroxide a decomposition to oxygen and water and H2O2 acting as oxidising agent. Thanks for your help
Tartaglia Posted March 15, 2006 Posted March 15, 2006 The Co3+ will catalyse decomposition H2O2 +2Co3+ --> O2 + 2Co2+ +2H+ The Co2+ will then be reoxidised H2O2 + 2Co2+ + 2H+ --> 2H2O + 2Co3+
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