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Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: Deathknight on March 16, 2009, 05:54:41 PM

Title: Pre-Lab Question (Oxidation reaction)
Post by: Deathknight on March 16, 2009, 05:54:41 PM

Here is the only problem I am having problems with on my chemistry lab.

Hydrogen peroxide is an effective oxidizing agent in basic solution, accepting two electrons.  It will oxidize iron(II) to iron(II). Unlike iron(II) oxalate, iron(III) oxalate is soluble under these conditions and forms the iron(III) oxalate ion.  This is a redox reaction; you must balance the electrons (charge_ as well as the atoms.  Some brown Fe(OH)2 is also formed, but this is a side reaction for which you do not need to write an equation.

Here is the chemical equation I was given to complete

_FeC2O4*2H2O(s) + _H2O2 (aq) -> _Fe(___)_(aq) + ___OH-(aq) + ___H2O(l)

Title: Re: Pre-Lab Question (Oxidation reaction)
Post by: Borek on March 16, 2009, 06:21:51 PM

Quote from: Deathknight on March 16, 2009, 05:54:41 PM

It will oxidize iron(II) to iron(II)

Looks like no oxidation to me ;)

http://www.chembuddy.com/?left=balancing-stoichiometry&right=balancing-redox

http://www.chembuddy.com/?left=balancing-stoichiometry&right=half-reactions-method

http://www.chembuddy.com/?left=balancing-stoichiometry&right=oxidation-numbers-method

But first of all:

http://www.chemicalforums.com/index.php?topic=58.0

Please read point 4.