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Chemistry Forums for Students => High School Chemistry Forum => Topic started by: sci0x on December 16, 2005, 07:19:37 PM

Title: Balanced Equation for the reaction of K[MnO4] and Fe[C2O4]. xH2O
Post by: sci0x on December 16, 2005, 07:19:37 PM
Could someone write the balanced equation for the reaction of K[MnO4] and Fe[C2O4]. xH2O.

I need it to find the concentration of the iron compound in grams per liter and the value of X.
Title: Re:Balanced Equation
Post by: Albert on December 16, 2005, 07:56:32 PM
Could someone write the balanced equation for the reaction of K[MnO4] and Fe[C2O4]. xH2O.

Show us what you've done so far. Here is my help: manganese loses 5 electrons, while carbonon gains only 2 (carbon will be in its highest oxidation form).
Title: Re:Balanced Equation
Post by: sci0x on December 16, 2005, 08:35:30 PM
K[MnO4] + Fe[C2O4].xH2O = 5Mn + CO2 + Fe   ? I doubt this is right.
Title: Re:Balanced Equation
Post by: Albert on December 17, 2005, 05:09:30 AM
The only two reagents that change their oxidation number are MnO4- and C2O4--
The other things are 'redundant'. Oh, and acid condition are required for manganese to change its oxidation state.
Title: Re:Balanced Equation
Post by: Albert on December 17, 2005, 05:17:29 AM
Moreover, I infer you are looking for information about ferrous oxalate: Fe[C2O4].2H2O

The number of molecules of water does not depend on the reaction we :) are trying to balance: it is something which simply deals with properties of ferrous oxalate.
Title: Re:Balanced Equation
Post by: Borek on December 17, 2005, 07:02:23 AM
The only two reagents that change their oxidation number are MnO4- and C2O4--
The other things are 'redundant'.

Are you sure? What is oxidation number of Fe in FeC2O4?
Title: Re:Balanced Equation
Post by: Albert on December 17, 2005, 07:08:59 AM
+2

So, you mean also Fe2+ is involved in the reaction? Ok, it might be. However, I think sci0x is looking for what I wrote in my last post.
Title: Re:Balanced Equation
Post by: Borek on December 17, 2005, 08:40:15 AM
sci0x needs to balance whole reaction to be able to calculate amount of ferric oxalate in the sample.

Both Fe2+ and oxalic acid (or oxalates) are commonly determined by manganometric method. Thus both oxidation reactions will be taking place in the reaction setup mentioned, not only one of them.
Title: Re:Balanced Equation
Post by: sci0x on December 17, 2005, 09:05:01 AM
Could someone please, just write down the balanced equation. I'm getting confused and I need it to finish this question.
Title: Re:Balanced Equation
Post by: Albert on December 17, 2005, 09:11:48 AM
3MnO4- + 5Fe2+ +  5C2O4-- + 24H+ -> 3Mn2+ + 5Fe3+ + 10CO2 + 12H2O
Title: Re:Balanced Equation
Post by: sci0x on December 17, 2005, 11:09:30 AM
Thank you so much, you're a life saver
Title: Re:Balanced Equation
Post by: sci0x on December 17, 2005, 11:53:20 AM
Oh sorry bout this, i thought I could do this, how do you calculate x?

I have Conc of K[MnO4] is 0.018M
Volume K[MnO4] is 25ml
Conc of the Fe(C2O4}.xH2O is 4.325 g/litre
For my experiment it took 19.4cm K[MnO4] to standardise the iron compound.