The reaction of iron(III) oxide with carbon monoxide occurs in a blast furnace w

Question

The reaction of iron(III) oxide with carbon monoxide occurs in a blast furnace when iron ore is reduced to iron metal:

Fe2O3(s) +   3CO(g)          2Fe(l)   +   3CO2(g)    H = -848 kJ

Suppose that this system is at equilibrium in a 5.0 L flask. Predict the direction in which the reaction will shift (to the left, to the right, no effect) when each of the following occurs. Include a short explanation for each choice.

a. A catalyst is added to the flask _____________________________

b. Some CO2(g)is removed from the flask ____________________________

c. Some (but not all) of the Fe2O3(s)is removed from the flask ____________________________

d. The volume of the flask is doubled _______________________________

e. The temperature of the flask is lowered ____________________________

Explanation / Answer

a] No effect - catalyst only promotes rate of reaction but it doesnt imply any effect on equilibrium.

b] To the right :

According to Le Chatelier, the position of equilibrium will move so that the concentration of CO2 increases again. That means that more Fe2O3 and CO will react to replace the CO2 that has been removed. The position of equilibrium moves to the right.

c] No effect - Adding Fe2O3 doesn't change the concentration of Fe2O3 since it's a solid so there would be no shift in the equilibrium if you added or removed some Fe2O3 .

d] No effect -- since same number of moles of gases are present on both sides .

e] To the right -- Decreasing the temperature of a system in dynamic equilibrium favours the exothermic reaction. The system counteracts the change you have made by producing more heat. -

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