To determine the percentage of iron Fe in the given iron ore sample using gravimetric analysis, the student needs to follow these steps:1. First, the student needs to prepare the iron ore sample by dissolving it in an appropriate solvent, such as hydrochloric acid HCl , to convert all iron into iron II ions Fe .2. The student then needs to titrate the iron II ions in the solution with the standardized potassium dichromate KCrO solution. During the titration, the potassium dichromate oxidizes the iron II ions to iron III ions Fe , while the dichromate ions CrO are reduced to chromium III ions Cr . The balanced chemical equation for this reaction is:6 Fe + CrO + 14 H 6 Fe + 2 Cr + 7 HO3. The student needs to carefully record the volume of the potassium dichromate solution used to reach the endpoint of the titration. The endpoint can be detected using an appropriate indicator, such as diphenylamine sulfonate, which changes color when all iron II ions have been oxidized.4. Using the volume of potassium dichromate solution and its concentration, the student can calculate the moles of dichromate ions CrO used in the titration. From the balanced chemical equation, we know that 1 mole of dichromate ions reacts with 6 moles of iron II ions. Therefore, the student can calculate the moles of iron II ions in the iron ore sample.5. Knowing the moles of iron II ions, the student can calculate the mass of iron Fe in the sample using the molar mass of iron 55.85 g/mol .6. Finally, the student can calculate the percentage of iron Fe in the iron ore sample by dividing the mass of iron by the mass of the iron ore sample and multiplying by 100.Please provide the mass of the iron ore sample and the concentration and volume of the potassium dichromate solution used in the titration to calculate the percentage of iron Fe in the sample.