Question

At 1000 K, *K*p = 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.

Answer #1

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

Initial -------- 0,904atm ------ 0atm

Change ------- -X ------- +X

Equilibrium -------- 0,904-Xat ------ X

K_{p}= (PCO_{2})^{3}/ (PCO)^{3}
(Solids and liquids are not affected by pressure)

==> 9,19= X^{3}/(0,904-X)^{3} (replace the
patrial pressures in equilibrium and solve for X)

==> ?9,19 = X/0,904-X

==>2,7098(0,904-x) = X

==>2,4497 -3,7098X = 0

==>-3,7098X = -2,4497

==>X=-2,4497/-3,7098

==> X=0,6603

Pressure of CO in eqiulibrium =0,904-0,6603 ==> 0,2437atm

Pressure of CO_{2} in equilibrium = X ==>
0,6603atm

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 ?

The reaction of iron(III) oxide with carbon monoxide is
important in making steel. At 1200 K, Kp=19.9 for the following
reaction: Fe2O3(s)+3CO(g)⇌2Fe(l)+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 0.908 atm? Express your answers
in atmospheres to three significant figures separated by a
comma.

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

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

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)

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?

The equilibrium constant Kp for the reaction
C(s)+H2O(g)?CO(g)+H2(g) is 2.44
at 1000 K. What are the equilibrium partial pressures of H2O, CO,
and H2 if the initial partial pressures are PCO= 1.25 atm,
and PH2= 1.60 atm?
What is the equilibrium partial pressure of H2O?
What is the equilibrium partial pressure of CO?
What is the equilibrium partial pressure of H2?

Consider the following reaction: A(g)⇌2B(g) Find the equilibrium
partial pressures of A and B for each of the following different
values of Kp. Assume that the initial partial pressure of B in each
case is 1.0 atm and that the initial partial pressure of A is 0.0
atm. Make any appropriate simplifying assumptions.
Part A
Kp= 1.6
Enter your answers numerically separated by a comma. Express
your answer using two significant figures.
Part B
Kp= 2.0×10−4
Enter your answers numerically...

Consider the following reaction: A(g)⇌2B(g) Find the equilibrium
partial pressures of A and B for each of the following different
values of Kp. Assume that the initial partial pressure of B in each
case is 1.0 atm and that the initial partial pressure of A is 0.0
atm. Make any appropriate simplifying assumptions.
A) Kp= 2.0×10−4
Enter your answers numerically separated by a comma. Express
your answer using two significant figures.
B) Kp= 1.8×105
Enter your answers numerically separated by...

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

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