Question

Calculate Δ*H*rxn for the following reaction:

Fe2O3(*s*)+3CO(*g*)→2Fe(*s*)+3CO2(*g*)

Use the following reactions and given Δ*H*′s.

2Fe(*s*)+3/2O2(*g*)→Fe2O3(*s*), Δ*H* =
-824.2 kJ

CO(*g*)+1/2O2(*g*)→CO2(*g*), Δ*H* =
-282.7 kJ

Answer #1

2Fe(s) + 3/2O2(g) ---> Fe2O3(s). DeltaH = -824.2kJ

Inversing the reaction we get-

Fe2O3(s) ---> 2Fe(s) + 3/2O2(g). DeltaH = +824.2kJ. ......(1)

CO(g) + 1/2O2(g) --->CO2(g). DelataH = -282.7kJ

Multiplying by 3-

3CO(g) + 3/2O2(g) ---> 3CO2(g). DeltaH = 3*-287.7 = -863.1kJ

Adding this reaction to reaction 1 we get-

Fe2O3(s)+3CO(g)+3/2O2(g)--->2Fe(s)+3/2O2(g)+3CO2

Cancelling same terms we get-

Fe2O3(s) + 3CO(g)--> 2Fe(s) + 3CO2(g)

Delta Hrxn = +824.2kJ -863.1kJ = -38.9kJ

Calculate the enthalpy of reaction for the following reaction:
Fe2O3(s) + 3CO(g) → 2Fe(s) + 3CO2(g) ΔHfo(Fe2O3(s)) = -824.2 kJ/mol
ΔHfo(CO(g)) = -110.5 ΔHfo(Fe(s)) = ? ΔHfo(CO2(g)) = -393.5
kJ/mol

Given the following data:
2Fe(s) + 3CO2(g) → Fe2O3(s) +
3CO(g)
ΔH° = 23.0 kJ
3FeO(s) + CO2(g) → Fe3O4(s) +
CO(g)
ΔH° = -18.0 kJ
3Fe2O3(s) + CO(g) →
2Fe3O4(s) + CO2(g)
ΔH° = -39.0 kJ
Calculate ΔH° for the reaction:
Fe(s) + CO2(g) → FeO(s) + CO(g)

Calculate ΔG° for the reduction of Fe2O3 by CO at 25°C: Fe2O3(s)
+ 3CO(g) → 2Fe(s) + 3CO2(g) (ΔG°f data: CO2(g), –394.4 kJ/mol;
Fe2O3(s), –741.0 kJ/mol; CO(g), –137.3kJ/mol) (Consider: Is the
value that you calculate for ΔG° here the same value that you
calculated for ΔG° using ΔH°f and S° data in the other
question?)
+60.6 kJ
-60.6 kJ
-30.3 kJ
+30.3 kJ
-15.1 kJ

At 1000 K, Kp = 19.9 for the reaction
Fe2O3(s)+3CO(g)⇌2Fe(s)+3CO2(g).
What are the equilibrium partial pressures of CO and CO2 if CO
is the only gas present initially, at a partial pressure of 0.940
atm ?

At 1000 K, Kp = 19.9 for the reaction
Fe2O3(s)+3CO(g)?2Fe(s)+3CO2(g)
What are the equilibrium partial pressures of CO and CO2 if CO
is the only gas present initially, at a partial pressure of
0.904atm ?
Enter your answers numerically separated by a comma.

Given the following reactions:
Question (1)
Calculate for the change in enthalpy of the reaction of
(3Fe2O3(s) + CO(g) yields CO2(g) + 2Fe3O4(s))
Fe2O3(s) + 3CO(g) yields 2Fe(s) + 3CO2(s)(Change in enthalpy=
-28.0 kJ)
3Fe(s) + 4CO2(s) yields 4CO(g) + FE3O4(s) (Change in enthalpy=
+12.5 kJ)

Iron(III) oxide reacts with carbon monoxide according to the
equation: Fe2O3(s)+3CO(g)→2Fe(s)+3CO2(g) A reaction mixture
initially contains 22.95 g Fe2O3 and 14.26 g CO.
Once the reaction has occurred as completely as possible, what
mass (in g) of the excess reactant is left?

3)From the following data at 25C ∆Hreaction (kJ
mol-1)
Fe2O3(s) + 3C(graphite) → 2Fe(s) + 3CO(g) 492.6
FeO(s) + C(graphite) → Fe(s) + CO(g) 155.8
C(graphite) + O2(g) → CO2(g)
-393.51
CO(g) + 1⁄2 O2(g) → CO2(g) -282.98
Calculate the standard enthalpy of formation of FeO(s) and of
Fe2O3(s).

Iron(III) oxide reacts with carbon monoxide according to the
equation:
Fe2O3(s)+3CO(g)→2Fe(s)+3CO2(g)
A reaction mixture initially contains 23.00 g Fe2O3and 15.66 g
CO.
Once the reaction has occurred as completely as possible, what
mass (in g) of the excess reactant is left?

From the following data calculate the ΔHrxn for the following
reaction:
2 C(s) + 2 H2O(g) CH4(g) + CO2(g) ΔHrxn = ________
Use the following reactions and given ΔH’s and show your
work.
CO(g) + H2(g) → C(s) + H2O(g) ΔHrxn = −131.3 kJ
CO(g) + H2O(g) → CO2(g) + H2(g) ΔHrxn = −41.2 kJ
CO(g) + 3 H2(g) → CH4(g) + H2O(g) ΔHrxn = −206.1 kJ

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