Balance the following redox equation using the half reaction method under acidic

Question

Balance the following redox equation using the half reaction method under acidic conditions:

MnO4-(aq) + Fe2+(aq)-->Mn2+(aq) + Fe3+(aq)

1. Assigning oxidation states, determining what is oxidized/reduced:

Mn

MnO4 is reduced. Fe2+ is oxidized.

2. Write the half reactions.

MnO4-(aq)-->Mn2+

Fe2+-->Fe3+

3. Balance except for O and H, then balance for O and H using water of H+.

MnO4- + 8H+-->Mn2+ 4 H2O

Fe2+-->Fe3+ + e-

I ma having trouble figuring out how to determine the # of electrons to add to the first equation. I know its 5 because the problem is worked but I don't see an easy way to figure that out. Please help.

Mn

Explanation / Answer

Balance the following redox equation using the half reaction method under acidic

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