All of the iron in 1734 g of an iron sample is converted

Question

All of the iron in 1.734 g of an iron sample is converted into Fe²⁺, which was then titrated with dichromate:

14H¹⁺ + Cr₂O₇^2- + 6Fe²⁺ -> 6Fe³⁺ + 2Cr³⁺ + 7H₂O

What is the mass percent iron in the sample if 29.65 mL of 0.10682 M K₂Cr₂O₇ were required to reach the equivalence point?