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

3Fe2O2(s) + CO(g) ---> 2Fe3O4(s)+ CO2(g)
ΔH° = -59kJ

Fe3O4(s) + CO(g) ---> 3FeO(s) + CO2(g)
ΔH° = +38kJ

What is ΔH° for the reaction
FeO(s) + CO(g) ---> Fe(s) +CO2(g)

  1. 👍
  2. 👎
  3. 👁
  1. Note that Fe2O2 isn't correct. Didn't you intend to type Fe2O3

    1. 👍
    2. 👎
  2. Correction:
    3Fe2O3(s) + CO(g) ---> 2Fe3O4(s)+ CO2(g)
    ΔH° = -59kJ
    Is this right?
    FeO(s) + CO(g) ---> Fe(s) +CO2(g)
    ΔH° = -28/2
    ΔH° = -14

    1. 👍
    2. 👎
  3. No, I don't get that answer. I only went through it once so I could have made an error. Here is what I did.
    The reverse of twice equation 3 + the reverse of equation 2 + 3x equation 1 and that gave me
    6FeO + 6CO ==> 6Fe + 6CO2 and -101 kJ/mol. That divided by 6 = about -17 kJ/mol.

    1. 👍
    2. 👎

Respond to this Question

First Name

Your Response

Similar Questions

  1. science

    Are rocks considered valuable natural resources?(1 point) No, rocks are not valuable because they contain a lot of waste. No, rocks are not valuable because they are nonliving solids. Yes, rocks are valuable because they are

  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

  3. chemistry

    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

  4. Chemistry

    A sample of 1.55g of iron ore is dissolved in a acid solution in which the iron is converted into Fe2+. The solution formed is then titrated with KMnO4 which oxidises Fe2+ to Fe3+ while the MnO4- ions are reduced to Mn2+ ions.

  1. chemistry

    A 1.362 g sample of an iron ore that contained Fe_3O_4 was dissolved in acid and all the iron was reduced to Fe^2+. the solution was then acidified with H_2SO_4 and titrated with 39.42 mL of 0.0281 M KMnO_4 , which oxidized the

  2. chemistry

    a sample iron ore is dissolved in an acidic solution in which yhe iron is converted into fe2+. the solution formed the titrated with kmno4 which oxidies fe2+ to fe3+ while kmno- ions are reduced to mn2+. 92.95 ml of 0..02M of

  3. 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

  4. 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

  1. Social Studies/Economics

    Which of these is an example of a capital resource? A. Workers B. iron ore (my answer) C. entrepreneurs D. computers

  2. 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).

  3. chemistry 2

    the balanced equation for the reduction of iron ore to the metal using CO is Fe2O3+3CO(g) -> 2Fe+3CO so what is the maximum of iron in grams that can bbe obtained from 454g (1.00 lb) of iron (III) oxide? AND what mass of CO is

  4. AP Chemistry

    An ore contains Fe3O4 and no other iron. The iron in a 36.5-gram sample of the ore is all converted by a series of chemical reactions to Fe2O3. The mass of Fe2O3 is measured to be 26 g. What was the mass of Fe3O4 in the sample of

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