[Kimberly]

1.) The Iron in a 6.675gram sample containing iron(III) oxide is reduced to Fe²⁺. The Fe²⁺ is titrated with 14.42 mL if 0.1467 M K₂Cr₂O₇ in an acid solution. Find the mass of Fe and the % of Fe in the sample. (Hint, balance the reaction using redox rules then use stoichometry to find the mass of iron in the original sample)

I could do the stoichometry and the percentage but I just don't know how to start this off because I'm having trouble with balancing. I could do the rest, it's just that I don't know how to start.

[UG]

Hi Kimberly,
To start off balancing redox reactions, you need to identify the two half-reactions, you can then write the oxidation half equation as well as the reduction half equation. See if one of my earlier posts will help you. See if you can follow these rules to balance the oxidation half equation and then combine the two equations together.