The following reaction occurs in the Blast furnance where iron ore is reduced to iron metal Fe₂O_3(s) + 3CO_(g) ⇌ Fe₍₁₎ + 3CO_2(g) Using the Le-chatelier's principle, predict which one of the following will not disturb the equilibrium.

The correct option is Addition of Fe₂O₃.

Step-by-Step Explanation:

Le Chatelier's principle states that if a system at equilibrium is disturbed by a change in temperature, pressure, or concentration of one of the components, the system will shift its equilibrium position in a direction that counteracts the disturbance.

Let us consider the given equilibrium reaction:
${\mathrm{Fe}}_2{O}_3\left(s\right)+3\mathrm{CO}\left(g\right)\rightleftharpoons \mathrm{Fe}\left(l\right)+3{\mathrm{CO}}_2\left(g\right)$

To determine which change will not disturb the equilibrium, we evaluate the states of the substances involved:
1. Gaseous reactants and products: CO and CO₂ are gases. According to Le Chatelier's principle, adding or removing a gas changes its concentration and partial pressure, which directly shifts the equilibrium position. Thus, adding CO₂, removing CO, or removing CO₂ will all disturb the equilibrium.
2. Solid reactants: Iron(III) oxide, Fe₂O₃, is present as a pure solid. The concentration (or activity) of a pure solid is constant and does not change regardless of the amount added or removed.

Because the concentration of a pure solid is constant, adding more Fe₂O₃(s) does not alter the reaction quotient or affect the equilibrium. Therefore, the addition of Fe₂O₃ will not disturb the equilibrium.