Question 1.A chemist was given the job of analyzing a sulfur-bearing ore in order to determine its suitability as a feed stock to produce sulfuric acid. She was informed that

the ore contained Cus and FeS2 as well as some inert material. She decided to do two determinations: one for the sulfur content and the other for iron.She took a 0.2046 g sample of ore and, after suitable preparation, precipitated all the sulfur as barium sulfate. This yielded 0.5465 g of BaSO4.In a separate experiment, the iron content of a 9.8650 g sample of ore was determined by firstly converting all the iron to Fe2(SO4)3, reducing the iron in the sample to Fe2*, and making the solution up to 250 ml in a volumetric flask. 25 ml aliquots of this solution were titrated with a standard potassium dichromate, K2Cr2O7, solution (0.02540 M). [The products of this reaction are Fe* and Cr*]. The average titre was 20.27 ml.Calculate the wt% of each of the metal sulfides in the ore.