# 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. 👎

## 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