jacknife360 Posted March 15, 2006 Share 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. Link to comment Share on other sites More sharing options...
Tartaglia Posted March 15, 2006 Share 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 Link to comment Share on other sites More sharing options...
jacknife360 Posted March 15, 2006 Author Share 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 Link to comment Share on other sites More sharing options...
Tartaglia Posted March 15, 2006 Share 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+ Link to comment Share on other sites More sharing options...
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