Question

Given the following data:

2Fe(s) + 3CO |
ΔH° = 23.0 kJ |

3FeO(s) + CO |
ΔH° = -18.0 kJ |

3Fe |
ΔH° = -39.0 kJ |

Calculate ΔH° for the reaction:

Fe(s) + CO_{2}(g) → FeO(s) + CO(g)

Answer #1

Lets number the reaction as 1, 2, 3, 4 from top to bottom

required reaction should be written in terms of other reaction

This is Hess Law

required reaction can be written as:

reaction 4 = (1/2) * (reaction 1) - (1/3) * (reaction 2) + (1/6) * (reaction 3)

So, deltaHo rxn for required reaction will be:

deltaHo rxn = (1/2) * deltaHo rxn(reaction 1) -(1/3) * deltaHo rxn(reaction 2) + (1/6) * deltaHo rxn(reaction 3)

= (1/2) * (23.0) - (1/3) * (-18.0) +(1/6) * (-39.0)

= 11.0 KJ

Answer: 11.0 KJ

Calculate ΔHrxn for the following reaction:
Fe2O3(s)+3CO(g)→2Fe(s)+3CO2(g)
Use the following reactions and given ΔH′s.
2Fe(s)+3/2O2(g)→Fe2O3(s), ΔH =
-824.2 kJ
CO(g)+1/2O2(g)→CO2(g), ΔH =
-282.7 kJ

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

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).

Calculate the ΔH for the following
reaction:
Fe2O3
+ 3 CO → 2 Fe + 3
CO2
based on the reactions below.
3Fe2O3
+
CO→2Fe3O4
+ CO2
ΔH=−48.5kJ
Fe+CO2
→FeO+CO.
ΔH=−11.0kJ
Fe3O4
+CO→3FeO+CO2
ΔH=+22.0kJ

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)

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 ?

You are given the following thermodynamic data. 2 Fe(s) + 3/2
O2(g) → Fe2O3(s) ΔH° = -823 kJ 3 Fe(s) + 2 O2(g) → Fe3O4(s) ΔH° =
-1120. kJ Calculate the ΔH° for the following reaction. 3 Fe2O3(s)
→ 2 Fe3O4(s) + ½ O2(g)

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.

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?

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