[treelove]

I did a titration using potassium permanganate in water and my iron sample dissolved in sulfuric acid. I also used phosphoric acid to make the color change more visible. I found that the average volume I used was 25.7 mL, and then I found that I had used 5.14x10^-4 moles of KMnO₄. The equation I wrote out is this:
Fe⁺² + 8H⁺ + MnO₄^- + 5e^- Mn⁺² + 4H₂O + Fe⁺³ + e^-

Is that right? Or should I do 4e^- on the left and omit the electron on the right? Do I need to include the phosphoric or sulfuric acid somehow, or is that covered by the H ions?

I'm not really sure where to go from here to determine the percent of iron though, since I have the moles of KMnO₄ instead of just MnO₄^-, will that alter my results?
Sorry I really have never done this before and we haven't gone over it in class so these questions might sound kind of stupid.

[treelove]

Ok that equation is wrong, I think I got the right one now. I ended up getting about 14.35% Fe, will anyone confirm this answer? What compound could this be?

[Borek]

I got 92%, but I am not sure I have used the same sample mass 

We can't check your numbers not knowing all the relevant data.

[treelove]

what other information do you need?