Need some help with writing this redox equation.

[Ematuro]

A manganese ore was analysed by titration with a freshly prepared acidified iron(II) sulfate solution.
The manganese was first oxidised to permanganate ion (MnO4−). The permanganate obtained from a 0.269 g sample of ore required a titre of 22.41 mL of 0.500 M FeSO4 solution to reach the endpoint.

How would you go about writing an equation for this?
I began with Mn --> MnO₄^-

But the answer does it the other way round. I dont get why? I mean in the equation it says permanganate obtained FROM a 0.269g sample of ore. So how come in the solutions they put it the other way round? Or did I misinterpret something?

[huaxiadragon]

Well the Mn --> MnO4 is the first part of the solution.

The second part is where

The permanganate reacts with Iron to change colour and form the Manganese ions.

P.S OMG I just learnt how to write equations in forum!

[huaxiadragon]

But the answer does it the other way round. I dont get why? I mean in the equation it says permanganate obtained FROM a 0.269g sample of ore. So how come in the solutions they put it the other way round? Or did I misinterpret something?

You didn't misinterpret. But the titration actually occurs with the permanagate. Think of obtaining permanganate from the ore as a process BEFORE the titration is conducted.

[Ematuro]

OH! I get it now thanks! I guess I didn't fully read the question properly after all

[pi]

This sounds a lot like the steel wool prac...