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It might be better to include Fe3+ is being reduced to Fe2+, just to show that you know which iron is being reduced. In addition, some problems specifically ask you to include which species is reduced or oxidized and from what oxidation number to what.
In past chem classes, I was taught OILRIG: Oxidation Is Loss, Reduction Is Gain. Since reduction is gaining electrons, the Fe ion is being reduced because its positive charge decreases, so it is becoming, relative to the original species, more negative. This is because electrons have a negative charge, so gaining electrons makes a species more negative.
You should try to be as specific as possible and show the redox half reactions to show and indicate you understand what is actually happening. I normally think of the reactions as OILRIG (oxidation is loss [of electrons]) (reduction is gain [of electrons]) so in this particular case, Fe is the one that's being reduced by the reaction.
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