Question

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

Answer #1

we have:

Gof(Fe2O3(s)) = -741.0 KJ/mol

Gof(CO(g)) = -137.3 KJ/mol

Gof(Fe(s)) = 0.0 KJ/mol

Gof(CO2(g)) = -394.4 KJ/mol

we have the Balanced chemical equation as:

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

deltaGo rxn = 2*Gof(Fe(s)) + 3*Gof(CO2(g)) - 1*Gof( Fe2O3(s)) - 3*Gof(CO(g))

deltaGo rxn = 2*(0.0) + 3*(-394.4) - 1*(-741.0) - 3*(-137.3)

deltaGo rxn = -30.3 KJ/mol

Answer: -30.3 KJ/mol

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

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)

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).

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.

Fe2O3(s) + 3C(s) -----> 2Fe(l) +
3CO(g)
(a.) Calculate the mass of iron that can be produced from 1.0
tonne (1.0 t) of Fe2O3 (where 1t =
103kg).
(b.) What mass of carbon is needed for the reduction of
Fe2O3 to produce 500. kg of iron?

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?

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?

Consider the following reaction, which is involved in the
purification of iron from its ores. Some relevant thermodynamic
data is shown below.
Fe2O3 (s) + 3CO(g) → 2Fe(s) + 3 CO2 (g) ΔS° = 15.2 J/K
Substance
∆Hf° (kJ/mol)
S° (J/K/mol)
∆Gf° (kJ/mol)
Fe2O3(s)
–824.2
87.40
??
CO(g)
–110.5
197.6
–137.2
Fe(s)
0
??
0
CO2(g)
–393.5
213.6
–394.4
a) Find ΔH° for the reaction above.
b) Find S° for solid iron.
c) Find ∆Gf° for Fe2O3.
*** I know...

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