Question

use the following information to answer the next question. some of the so₂(g) produced from the burning of coal and natural gas can react with no₂(g) in the atmosphere according to the equation so₂(g) + no₂(g) ⇌ no(g) + so₃(g) + energy. 5. the equilibrium concentration of so₂(g) in the reaction could be increased by a. raising the temperature b. adding a catalyst c. removing so₃(g) d. adding no₂(g)

Explanation:

Step1: Recall Le - Chatelier's principle

Le - Chatelier's principle states that when a system at equilibrium is subjected to a change, the system will adjust to counteract the change. For the exothermic reaction \(SO_{2(g)}+NO_{2(g)}
ightleftharpoons NO_{(g)} + SO_{3(g)}+\text{energy}\).

Step2: Analyze option a

Raising the temperature for an exothermic reaction will shift the equilibrium in the reverse direction to absorb the added heat. This will decrease the concentration of \(SO_3\).

Step3: Analyze option b

Adding a catalyst only changes the rate of the forward and reverse reactions equally. It does not affect the position of the equilibrium, so the concentration of \(SO_3\) remains unchanged.

Step4: Analyze option c

Removing \(SO_3\) will cause the equilibrium to shift in the forward direction to replace the removed \(SO_3\), but this is not what the question asks (it asks for increasing the equilibrium concentration).

Step5: Analyze option d

Adding \(NO_2\) will shift the equilibrium in the forward direction according to Le - Chatelier's principle. As the reaction proceeds forward to consume the added \(NO_2\), more \(SO_3\) will be produced, increasing its equilibrium concentration.

Answer:

d. Adding \(NO_{2(g)}\)