A 3.75-g sample of iron ore is transformed to a solution of iron(II) sulfate, FeSO₄, and this solution is titrated with 0.150 M K₂Cr₂O₇ (potassium dichromate). If it requires 43.7 mL of potassium dichromate solution to titrate the iron(II) sulfate solution, what is the percentage of iron in the ore? The reaction is

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6FESO,(aq) + K,Cr,O,(aq) + 7H,SO.(aq) → 3Fe,(SO,);(aq) + Cr,(SO,);(aq) + 7H,O(1) + K2SO,(aq)