A 1.362 g sample of an iron ore that contained FegO4was dissolved in acid and all of the iron was reduced to Fe2*. The solution wasthen acidified with H2SO4 and titrated with 39.42 mL of 0.0281 M KMN04, which oxidized the iron to Fe. The net ionic equation forthe reaction is5Fe2* + MnO4 + 8H*5FE3+ + Mn2+ + 4H2OWhat was the percentage by mass of iron in the ore?What was the percentage by mass of Fe30z in the ore?Part 1X Your answer is incorrect.Calculate the number of moles of permanganate ion in the solution given.moles MnO4Attempts: 1 of 1 usedPart 2Using the previous answer and the balanced equation, find the number of moles of Fe".mol Fe2+

Answered: Image /qna-images/answer/fe9fc5ab-b8a1-4a4a-935e-97f3cee55dea.jpg

A 1.362 g sample of an iron ore that contained FezOawas dissolved in acid and all of the iron was reduced to Fe2*. The solution was then acidified with H2SO4and titrated with 39.42 ml of 0.0281 M KMNO4, which oxidized the iron to Fe. The net ionic equation for the reaction is 5FE2+ + MnO+ 8H* 5F 3+ + Mn2 +4H20 What was the percentage by mass of iron in the ore? What was the percentage by mass of Fe30gin the ore? Part 1 X Your answer is incorrect. Calculate the number of moles of permanganate ion in the solution given. moles MnO4 Attempts: 1 of 1 used

A 1.362 g sample of an iron ore that contained FezOawas dissolved in acid and all of the iron was reduced to Fe2. The solution was then acidified with H2SO4and titrated with 39.42 ml of 0.0281 M KMNO4, which oxidized the iron to Fe. The net ionic equation for the reaction is 5FE2+ + MnO+ 8H 5F 3+ + Mn2 +4H20 What was the percentage by mass of iron in the ore? What was the percentage by mass of Fe30gin the ore? Part 1 X Your answer is incorrect. Calculate the number of moles of permanganate ion in the solution given. moles MnO4 Attempts: 1 of 1 used

Chemistry

10th Edition

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

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Balance the following redox reactions by the half-reaction method: Cr(s) + N2H4(aq) = NH3(aq) + Cl(OH)3(aq) in basic solution
A 1.362 g sample of an iron ore that contained FegO4was dissolved in acid and all of the iron was reduced to Fe2*. The solution was then acidified with H2SO4and titrated with 39.42 mL of 0.0281 M KMNO4, which oxidized the iron to Fe. The net ionic equation for the reaction is 5FE2+ + MnO4+8H* 5FE3+ + Mn2+ + 4H2O What was the percentage by mass of iron in the ore? What was the percentage by mass of FegO4 in the ore? Part 1 Your answer is incorrect. Calculate the number of moles of permanganate ion in the solution given. moles MnO4 Attempts: 1 of 1 used Part 2 Using the previous answer and the balanced equation, find the number of moles of Fe2+. mol Fe2+
The following reaction occurs in acidic solution. As, O6(s) + MnO, (ag)AsO (aq) + Mn²* (aq) What is the sum of the coefficients in the balanced equation?
Give detailed Solution with explanation needed
A sample of iron ore weighing 0.962 g was dissolved in dilute acid solution, and all the Fe(II) was converted to Fe(III) ions. The solution required 32.32 mL of 0.0475M KMnO4 for titration. Fill in the table and calculate the % by mass of iron in the ore. Balance the equation: Fe +2 + MnO4 → Fe+3 + MnO2 Computation Name of analyte Iron ore Mass of analyte 0.2792 g Name of titrant KMnO4 Volume of titrant 23.30 mL Milliequivalents of the titrant 2.260 milliequivalents Mass of the analyte 0.125 g % Fe in analyte 44.81%
An aqueous solution of potassium permanganate KMnO4 is mixed with an aqueous solution of manganese (II) sulfate MnSO4.Justify that a redox reaction is possible and write the equation corresponding to this reaction.
A precipitate of AgCl + AgBr weighs 0.8132 gram. On heating in a current of chlorine, the AgBr is converted into AgCl, the mixture losing 0.1450 gram in weight. What was the percentage of chlorine in the original precipitate?
A 0.8040-g sample of an iron ore is dissolved in acid. The iron is then reduced to Fe²+ and titrated with 47.22 mL of 0.02242 M KMn 04 solution. Calculat the results of this analysis in terms of % Fe (55.847 g/mol).
After reducing a 0.4080 g iron to Fe²⁺, it was titrated with 42.72 mL of 0.1211 N KMnO₄ solution. Calculate the percent Fe₃O₄ (231.54 g/mol). The reaction is described by the equation: MnO₄- + 5Fe²⁺ + 8H⁺ → Mn²⁺ + 5Fe³⁺ + 4H₂O * Choices 50.81% 70.81% 36.77% 97.86% 58.72%
11. Identify the oxidizing agent in the chemical reaction 5Fe" (aq) + MnO4 (aq) + 8H"(aq) 5Fe+3 + Mn+2 (aq) + 4H2O
An aqueous solution of NaCl was electrolyzed with a current of 2.50 amps for 15.0 minutes. What volume (in mL) of 0.500 M HCl would be required to neutralize the resulting solution? (Hint: H2 is produced at the cathode and Cl2 at the anode.)
Balance each of the following reactions, and identify the type of reaction CrCl3 (aq) + H2S(g) → Cr2S3(s) + HCl(aq)