To understand how the equilibrium of the reaction [tex]\(SO_2(g) + NO_2(g) \rightleftharpoons NO(g) + SO_3(g) + \text{heat}\)[/tex] would change if NO[tex]\(_2\)[/tex] were added, let's analyze the situation step by step:
1. Identify the Reaction Type: This is a reversible reaction in a state of dynamic equilibrium. The forward reaction produces [tex]\(\text{NO}\)[/tex] and [tex]\(\text{SO}_3\)[/tex] and releases heat, while the reverse reaction consumes [tex]\(\text{NO}\)[/tex] and [tex]\(\text{SO}_3\)[/tex] and absorbs heat.
2. Le Chatelier's Principle: According to Le Chatelier's Principle, if a system at equilibrium is disturbed, the system will adjust itself to counteract the disturbance and re-establish equilibrium.
3. Adding [tex]\(NO_2\)[/tex]: Adding [tex]\(NO_2\)[/tex] to the system increases the concentration of one of the reactants. The system will attempt to counter this disturbance by consuming the added [tex]\(NO_2\)[/tex].
4. Shift in Equilibrium: To consume the extra [tex]\(NO_2\)[/tex], the equilibrium will shift to the right—toward the products.
5. Result of the Shift: When the equilibrium shifts to the right, more [tex]\(NO\)[/tex] and [tex]\(SO_3\)[/tex] will be produced.
Conclusion: Therefore, upon adding [tex]\(NO_2\)[/tex], the equilibrium will shift to the right, increasing the amounts of [tex]\(NO\)[/tex] and [tex]\(SO_3\)[/tex].
Thus, the correct answer is:
A. The amount of [tex]\(NO\)[/tex] and [tex]\(\text{SO}_3\)[/tex] would increase.
