To answer the question of how adding oxygen [tex]\((O_2)\)[/tex] to the reaction
[tex]\[ 2 \;SO_2(g) + O_2(g) \rightleftharpoons 2 \;SO_3(g) \][/tex]
changes the equilibrium, we need to apply Le Chatelier's Principle. Le Chatelier's Principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium moves to counteract the change.
1. Addition of Reactant:
- Adding [tex]\((O_2)\)[/tex] increases the concentration of one of the reactants.
2. Shift in Equilibrium:
- To counteract the increase in [tex]\((O_2)\)[/tex], the system will try to reduce the concentration of [tex]\((O_2)\)[/tex] by shifting the equilibrium to the right, where [tex]\((O_2)\)[/tex] is used up to form more [tex]\((SO_3)\)[/tex].
Correct Answer:
[tex]\[ \boxed{\text{A. The equilibrium shifts right to produce more } SO_3 \text{ molecules.}} \][/tex]
This shift will lead to an increase in the amount of [tex]\(SO_3\)[/tex] produced and a decrease in the amount of [tex]\(SO_2\)[/tex] and [tex]\(O_2\)[/tex] as they are consumed in the reaction.
