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How would the equilibrium change if [tex]$NO_2$[/tex] were added to [tex]$SO_2(g) + NO_2(g) \rightleftharpoons NO(g) + SO_3(g) + \text{heat}$[/tex]?

A. The amount of NO and [tex][tex]$SO_3$[/tex][/tex] would increase.
B. The amount of [tex]$NO_2$[/tex] and [tex]$SO_2$[/tex] would increase.
C. The equilibrium constant would increase.
D. The amount of NO and [tex][tex]$SO_3$[/tex][/tex] would decrease.

Sagot :

GinnyAnsweridn
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.
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