Chemical Forums
Chemistry Forums for Students => Organic Chemistry Forum => Topic started by: ikariotis on June 03, 2010, 05:17:35 PM
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Hey!
Please help me balance following formula
C7H5NO3 + KMnO4 :rarrow: C7H5NO4
Ox: .
Red: ...
Total: .
No representation of electron-es in the total reaction.
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Where's your Manganese in the products?
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Obviously this is just a scheme that has to be filled up with lacking substances.
First of all - do you know what are conditions (acidic, neutral, basic) of the reaction?
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the problem is just an oxidation whitout any conditions, but we have to do an redoxreaction scheme.
My example
Ox: MnO4- + 4H+ + 3e- :rarrow: MnO2 + 2H2O
Red: C7H5NO3 + H2O :rarrow: C7H5NO4 + 2H+ + 2e-
When I do like this I am gonna have electron-es on my total reaction so how can I eliminate this problem and still balance the reaction?
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If you want to eliminate the electrons, then multiply each reaction by suitable factors (Least Common Multiple LCM) that will make the number of electrons equal in both the half reactions. Then just add the reactions.
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the problem is just an oxidation whitout any conditions
So it can't be done, as products of permanganate reduction depend on the pH.
Ox: MnO4- + 4H+ + 3e- :rarrow: MnO2 + 2H2O
Red: C7H5NO3 + H2O :rarrow: C7H5NO4 + 2H+ + 2e-
You got Red & Ox reversed.
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Ox: MnO4- + 4H+ + 3e- :rarrow: MnO2 + 2H2O
Red: C7H5NO3 + H2O :rarrow: C7H5NO4 + 2H+ + 2e-
You got Red & Ox reversed.
I didn't notice that :-[