Question

- Hydrogen peroxide is an effective oxidizing agent, accepting two electrons. It will oxidized iron(II) to iron(III). This process strips some of the oxalate ion from the iron, so the product is a mixture of Fe3+ (aq), FeC204+ (aq), and Fe(C204)2 (aq). Assume that the predominant product is Fe3+ (aq). This is a redox reaction; therefore you must balance the electrons (charge) as well as the atoms. _Fe(C2O4)22- (aq) + H2O2 (aq) → (aq) + _ C2042- (aq) + _ OH+ (aq) The resulting solution is basic, causing some or all of the iron to precipitate as iron (III) hydroxide, a reddish-brown precipitate. (aq) + OH® (aq) →

Answer 1

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1. fe (9200), Tom + regas in e-Won - France and more - H2O2 low → Fe 3* + C2O4 + OH Cas; Loc) (aq) haif Oxidation 1. half reduction 2 x (fezt —— Fe3t+e-) 2e + H2O2 - 2014 n o n combination 2 Fe2+ + H₂O - 2fe3+ + zoh | 2 Fe (9200),- +14202 -> 2643* + 4904420 | Festas +381 - Feconds is (a Reddish boown precipitate .