How to balance redox reactions?

Question

I realy need some help with this
Balance the following redox reaction:
a))KMnO4(aq)+HCl(aq)->MnCl2(s)+KCl(aq)+Cl2(g)+H2O(l)

Thanks

Answer 1

The equation you wrote cannot balance, because Mn(VII) in permanganate is being reduced to Mn(II) in MnCl2, but nothing is being oxidised.

Actually, in this reaction, the chloride is oxidised to chlorine.

Ignore the potassium; itispresent as the K+ ion from start to finish. You may as well also ignore the chloride in MnCl2, to avoid confusion. You can always add them back in later.

You now need to balance and combine the two half-equations

MnO4 - --> Mn2+

and

Cl- ---> Cl2

Someone explained just how to do this in detail earlier this evening; look back to find other questions about balancing redox.