I did a lab where we had to determine the iron content in ore...i am confused about the reactions that occured during the reaction...i need reactions for the following...

1) The samples were treated with 6M HCl until all the iron ore dissolved.Assuming all of the ore is in the form Fe2O3m, what is the balanced equation for this process?

What I have is..

Fe2O3(s) + 6HCl (aq) --> 2FeCl3(aq) + 3H2O (l)

2) Samples were then treated with Zn metal according to the following balanced chemical equation...

i have the following, but am unsure if it is correct and if it is i am unsure how to balance it (charges..)

2FeCl3(aq) + 3Zn(s)--> 3ZnCl2(aq) + 2Fe^3+

3) Immediately prior to titration, any excess zinc was removed by treatment with 3M H2SO4 according to the following balanced chemical equation:

I am not sure how to go about writing this equation....

Any help or guidance would be greatly appreciated!!

  1. 👍 0
  2. 👎 0
  3. 👁 162
  1. The 2nd reaction is
    2FeCl3(aq) + 3Zn(s)--> 3ZnCl2(aq) + 2Fe(s)
    The excess zinc removal reaction is
    Zn(s) + H2SO4(aq) --> ZnSO4(aq) + H2(g)

    1. 👍 0
    2. 👎 0

Respond to this Question

First Name

Your Response

Similar Questions

  1. Chimestry

    (Iron ore is impure Fe_2O_3. When Fe_2O_3 is heated with an excess of carbon (coke), metallic iron and carbon monoxide gas are produced. From a sample of ore weighing 950kg , 533kg of pure iron is obtained). What is the mass

    asked by Inni on September 11, 2012
  2. Chemistry

    An iron ore sample contains Fe2O3 together with other substances. Reaction of the ore with CO produces iron metal: αFe2O3(s)+βCO(g)→γFe(s)+δCO2(g) A)Balance this equation. B)Calculate the number of grams of CO that can react

    asked by COR on February 25, 2020
  3. Chemistry

    Iron ores have different amounts of iron per kilogram of ore. Calculate the mass percent composition of iron for each iron ore: Fe2O3{\rm Fe_2O_3} (hematite), Fe3O4{\rm Fe_3O_4} (magnetite), FeCO3{\rm FeCO_3} (siderite).

    asked by Ana on March 5, 2014
  4. Chemistry

    In the recovery of iron from iron ore, the reduction of the ore is actually accomplished by reactions involving carbon monoxide. Use the following thermochemical equations, Fe2O2(s) + 3CO(g) ---> 2Fe(s) +3CO2(g) ΔH° = -28kJ

    asked by Lenny on March 24, 2015
  5. Chemistry

    check answer please 10. 2 Ca3(PO4)2(s) + 6 SiO2(g) + 10 C(s) ---> P4(s) + 6 CaSiO3(s) + 10 CO(g) If 39.3 g of Ca3(PO4)2, 24.4 g of SiO2 and 8.00g of C are available, find the limiting reagent. n Ca3(PO4)2= 0.127 moles n SiO2=

    asked by Shine bright shine far on March 3, 2019
  1. Chemistry

    How many grams of pure H2SO4 can be obtained from 250 grams of iron ore if the ore is 82% FeS2? The reactions involved are given below: 4FeS2 + 11 O2 --> 2 Fe2O3 + 8 SO2 (95% efficient) 2SO2 + O2 --> 2SO3 (90% efficient) SO3 + H2O

    asked by Veronica on June 7, 2014
  2. linear programming

    Exeter Mines produces iron ore at four different mines; however, the ores extracted at each mine are different in their iron content. Mine 1 produces magnetite ore, which has a 70% iron content; mine 2 produces limonite ore, which

    asked by uma on June 6, 2012
  3. Chemistry

    The rock in a particular iron ore deposit contains 84 % Fe2O3 by mass. How many kilograms of the rock must be processed to obtain 1100 kg of iron?

    asked by Aria on March 31, 2016
  4. Quantitative methods

    Missouri Mineral Products (MMP) purchases two unprocessed ores from Bolivia Mining, which it uses in the production of various compounds. Its current needs are for 800 pounds of copper, 600 pounds of zinc, and 500 pounds of iron.

    asked by Anonymous on August 20, 2012
  5. Chemistry

    1.630 g of iron ore is dissolved in an acidic solution. This solution is titrated to a pink endpoint with 27.15 mL of a 0.020 M KMnO4 solution. a. How many moles of MnO4- ions were consumed? b. How many moles of Fe2+ were in the

    asked by Ray on September 8, 2014
  6. ap chemistry

    A 25.2 g of iron ore is treated as follows. The iron in the sample is all converted by a series of chemical reactions to Fe2O3. The mass of Fe2O3 is measured to be 12 grams. What was the percent iron in the sample of ore? Answer

    asked by cheri on September 10, 2012

You can view more similar questions or ask a new question.