[ikariotis]

Hey!

Please help me balance following formula

C₇H₅NO₃ + KMnO₄  C₇H₅NO₄

Ox: .
Red: ...

Total: .

No representation of electron-es in the total reaction.

[Jorriss]

Where's your Manganese in the products?

[Borek]

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?

[ikariotis]

the problem is just an oxidation whitout any conditions, but we have to do an redoxreaction scheme.

My example

Ox: MnO₄^- + 4H⁺ + 3e^-  MnO₂ + 2H₂O
Red: C₇H₅NO₃ + H₂O  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?

[Schrödinger]

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.

[Borek]

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^-  MnO₂ + 2H₂O
Red: C₇H₅NO₃ + H₂O  C₇H₅NO₄ + 2H⁺ + 2e^-

You got Red & Ox reversed.

[Schrödinger]

Ox: MnO₄^- + 4H⁺ + 3e^-   MnO₂ + 2H₂O
Red: C₇H₅NO₃ + H₂O   C₇H₅NO₄ + 2H⁺ + 2e^-

You got Red & Ox reversed.

I didn't notice that