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- Fe in ore can be analyzed by oxidizing Fe to Fe2+ then titrating Fe2+with K2Cr2O7 . See equation below. K2Cr2O7(aq) + 6Fe2+(aq) + 14H+(aq) → 2Cr3+(aq) + 2K+(aq) + 6Fe3+(aq) + 7H2O(l) What is the stoichiometry of the analyte and titrant ? a. 6 mol titrant to 1 mol analyte b. 6 mol analyte to 1 mol titrant c. 2 mol titrant to 1 mol analyte d. 2 mol analyte to 1 mol titrantAll arsenic in the mineral containing 20 g of arsenic is dissolved by converting it into As3+. Calculate the percentage of arsenic in the mineral since the solution is titrated with 43.8 mL of decinormal KBrO3 solution.0.683 grams of iron mineral dissolves with acid. Fe2+ is titrated with Ce(SO4)2 solution. Calculate the percentage of iron since 38.5 mL of 0.161 M titrant is consumed in the titration. ( Fe:56 g/mole)
- 1. What is the oxidation state of Ti in TiO2? Group of answer choices 2- 2 4 0 4- 2, 2.Which element is oxidized in the reaction below? Fe2+ + CrO42- + H2O→ Fe3+ + Cr3+ +OH- Group of answer choices A, Cr6+ B, O2+ C, Cr3+ D, Fe2+ E, Fe3+25.00 mL of a solution containing KIO4 is treated with excess potassium iodide. IO4- + 8H+ + 7I- → 4I2 + 4H2O The resulting solution is titrated with 0.15 M sodium thiosulfate pentahydrate. The average titre was 21.76 mL. I2 + 2S2O32- → 2I- + S4O62- What mass of KIO4 (in g) was dissolved in water to make the original solution?A sample of an iron ore is dissolved in acid, and the iron isconverted to Fe2+. The sample is then titrated with 47.20 mLof 0.02240 M MnO4- solution. The oxidation-reduction reactionthat occurs during titration isMnO4-1aq2 + 5 Fe2+1aq2 + 8 H+1aq2¡Mn2+1aq2 + 5 Fe3+1aq2 + 4 H2O1l2(a) How many moles of MnO4- were added to the solution?(b) How many moles of Fe2+ were in the sample? (c) Howmany grams of iron were in the sample? (d) If the samplehad a mass of 0.8890 g, what is the percentage of iron in thesample?
- The oxidizing agent in the reaction below is 3CuCl2(aq)+2Al(s) →3Cu(s)+2AlCl3(aq) Cu2+ Al Cu Al3+Iron can be extracted from haematite, Fe2O3, using either C or CO2 as the reducing agent.The reactions are shown below.Fe2O3(s) + 3 C(s) → 2 Fe(s) + 3 CO(g) ΔH = +492.7 kJ /molFe2O3(s) + 3 CO(g) → 2 Fe(s) + 3 CO2(g) ΔH = - 24.8 kJ/molSubstance S° (J/ K·mol)Fe2O3 (s) 87.4Fe (s) 27.3C (s) 5.7CO (g) 197.6CO2 (g) 213.6Use available data given to:1. Calculate the minimum temperature at which reduction with carbon is feasible2. Prove by calculation that reduction with carbon monoxide is feasible at all temperaturesWhich substance is the oxidizing agent in the reaction below?Fe(CO)5 (l) + 2HI (g) →→ Fe(CO)4I2 (s) + CO (g) + H2(g) HI Fe(CO)4I2 Fe(CO)5 H2 CO
- 0.1745 g of primary standard Na2C2O4 is used to set a freshly prepared KMnO4 solution and 30.24 mL of KMnO4 solution is spent at the turning point. Since 36.92 mL of this KMnO4 solution is consumed for the determination of iron in 0.5618 g ore sample, calculate the amount of iron in the ore in terms of % iron (III) oxide and % iron (III) chloride. (Fe: 56, K: 39, Mn: 55, O: 16, Na:23, C: 12, Cl: 35.5 g/mol) (Please type answer)The reaction of hydroxylamine and Fe(III) produces nitrous oxide, Fe(II) and water: 2H2NOH + 4Fe3+ N2O(g) + 4Fe2+ + 4H+ + H2O. A 50 ml sample of hydroxylamine was treated with Fe(III) solution and the released Fe(II) was titrated with 0.0325 M K2Cr2O7 solution, which consumed 19.83 ml. Calculate the hydroxylamine concentration of the sample.0.683 grams of iron mineral dissolves with acid. Fe2+ is titrated with Ce(SO4)2 solution. Calculate the percentage of iron since 38.5 mL of 0.161 M titrant is consumed in the titration (Fe:56 g/mol)