Question

A 3.75-G SAMPLE OF IRON ORE IS TRANSFORMED TO A SOLUTION OF IRON(II)SULFATE, FeSO4,AND THIS SOLUTION IS TITRATED WITH 0.150 M K2Cr2O7. IF IT REQUIRES 43.7 mL OF POTASSIUM DICHROMATE SOLUTION TO TITRATE THE IRON(II)SULFATE SOLUTION, WHAT IS THE PERCENTAGE OF IRON IN THE ORE? THE REACTION IS
6FeSO4(aq)+K2Cr207(aq)+7H2SO4(aq)¨
3Fe2(SO4)3(aq)+Cr2(SO4)3(aq)+7H2O(l)+K2SO4(aq)
mols dichromate = M x L = ?
Use the coefficients in the balanced equation to convert mols dichromate to mols FeSO4
Convert mols FeSO4 to mols Fe then to grams Fe. g Fe = mols Fe x atomic mass Fe.
%Fe = (mass Fe/mass sample)*100 = ?
62.81%

Related Questions

overall balanced reaction: 14H+ + C2O7^2- + 6Fe^2+ -> 2Cr^3+ + 7H2O + 6Fe^3+ .5021g of impure sa... Determine the of mole of water molecules in one mole of a sample of an iron containing (nh4)2so4. Fe... 7) A 3.33 g sample of iron ore is transformed into a solution of iron (II) sulfate. And this solutio... A potassium permanganate solution containing 1.58 g of KMnO4 per liter is added into 5 ml of an acid...