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Experiment 0.0782 5: Redox (Dichromate Titrations) 8 sample of Iron ore is dissolved in H,PO/H₂SO, mixture passed over a reducing agent so that all the iron is in the form Fe. The Fe is completely oxidized by 31.6 mL of a 5.1 x10 M Cr₂O, solution. Calculate the mass percentage of the iron in the ore? (Fe-55.845 g/mol) Cr₂O₂ + 6Fe2+ 14H- 2Cr +6Fe³+ 7H₂O a) 44.0 % w/w b) 16.8 % w/w c) 24.3 % w/w d) 12.8 % w/w e) 6.91 %w/w A

Experiment 0.0782 5: Redox (Dichromate Titrations) 8 sample of Iron ore is dissolved in H,PO/H₂SO, mixture passed over a reducing agent so that all the iron is in the form Fe. The Fe is completely oxidized by 31.6 mL of a 5.1 x10 M Cr₂O, solution. Calculate the mass percentage of the iron in the ore? (Fe-55.845 g/mol) Cr₂O₂ + 6Fe2+ 14H- 2Cr +6Fe³+ 7H₂O a) 44.0 % w/w b) 16.8 % w/w c) 24.3 % w/w d) 12.8 % w/w e) 6.91 %w/w A

Chemistry
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Redox (Dichromate Titrations)

 

A 0.0782 sample of Iron ore is dissolved in H_{3}*P*O_{4} / H_{2} * S*O_{4} mixture passed over a reducing agent so that all the iron is in the form F e^ 2- , The Fe is completely oxidized by 31.6 mL of a 5.1 x10 M C*r_{2} O 7 ^ 2- solution. Calculate the mass percentage of the iron in the ore? (Fe - 55.845g / m * ol)

Experiment 5: Redox (Dichromate Titrations) of Iron ore dissolved in 0.0782 8 sample H,PO/H₂SO, mixture passed over a reducing agent so that all the iron is in the form Fe. The Fe is completely oxidized by 31.6 mL of a 5.1 x10 M Cr₂O, solution. Calculate the mass percentage of the iron in the ore? (Fe- 55.845 g/mol) Cr₂O₂ + 6Fe²+ 14H2Cr +6Fe³+7H₂O a) 44.0 % w/w b) 16.8 % w/w c) 24.3 % w/w d) 12.8 % w/w e) 6.91 %w/w A
Transcribed Image Text:Experiment 5: Redox (Dichromate Titrations) of Iron ore dissolved in 0.0782 8 sample H,PO/H₂SO, mixture passed over a reducing agent so that all the iron is in the form Fe. The Fe is completely oxidized by 31.6 mL of a 5.1 x10 M Cr₂O, solution. Calculate the mass percentage of the iron in the ore? (Fe- 55.845 g/mol) Cr₂O₂ + 6Fe²+ 14H2Cr +6Fe³+7H₂O a) 44.0 % w/w b) 16.8 % w/w c) 24.3 % w/w d) 12.8 % w/w e) 6.91 %w/w A
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