Iron oxide ores are reduced to iron metal by exothermic reaction with carbon monoxide?
$F e O (s) + C O (g) = F e (s) + C O_{2} (g)$ . Which of the following changes in conditions will cause the equilibrium to shift to the right?

Add

C O_{2}

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Add

F e O

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Add

C O

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Raise the temperature

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Solution

The correct option is C Add $C O$

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One of the reactions that takes place in producing steel from iron ore is the reduction of iron (II) oxide by carbon monoxide to give iron metal and CO₂.

FeO (s) + CO (g) Fe (s) + CO₂ (g); K_p= 0.265 at 1050 K.

What are the equilibrium partial pressures of CO and CO₂ at 1050 K if the initial partial pressures are: p_CO = 1.4 atm and = 0.80 atm?

Q. One of the reaction that takes place in producing steel from iron ore is the reduction of iron (II) oxide by carbon monoxide to give iron metal and

C O_{2}

F e O (s) + C O (g) ⇌ F e (s) + C O_{2} (g)

; K_{p} = 0.265

atm at 1050 K.
What are the equilibrium partial pressures of

C O

and

C O_{2}

respectively at 1050 K if the initial partial pressures are:

P_{C O} = 1.4

atm and

P_{C O_{2}} = 0.80

atm?

One of the reactions that takes place in producing steel from iron ore is the reduction of iron (II) oxide by carbon monoxide to give iron metal and CO₂. FeO (s) + CO (g) Fe (s) + CO₂ (g); K_p= 0.265 at 1050 K. What are the equilibrium partial pressures of CO and CO₂ at 1050 K if the initial partial pressures are: p_CO = 1.4 atm and CO₂ = 0.80 atm?