Understanding Chemical Equilibrium: The Impact of Removing SO3

In a chemical equilibrium reaction, what happens if SO3 is removed from the system?

• A. The concentration of SO2 increases
• B. The concentration of O2 increases
• C. The concentration of SO2 decreases more than O2
• D. The reaction completely shifts left

Answer: (C)

In a chemical equilibrium, the system strives to maintain a balance between the reactants and products. When a component, such as SO3, is removed from the system, the equilibrium position will shift in a direction that counteracts the change according to Le Chatelier's principle. By removing SO3, the system responds by shifting the equilibrium to the left, which is the direction that produces more SO3 from the available SO2 and O2. This shift will lead to an increase in the concentration of both SO2 and O2, as both are reactants in the reverse reaction. The concentration of SO2 will indeed increase as more of it reacts with O2 to form SO3. However, the phrasing of the correct answer highlights that the concentration of SO2 specifically increases more than that of O2. This can occur because, depending on the stoichiometry of the reaction, the molar ratios of the substances being consumed or produced may vary, leading to a disproportionate increase in one compared to the other. Thus, the response reflects the adjustment of the system towards re-establishing equilibrium after the removal of SO3. In a scenario where SO2 and O2 are utilized in a way that drives the forward reaction, the

When you're knee-deep in chemistry, especially preparing for exams like the ACS Chemistry Exam, getting the hang of concepts like chemical equilibrium can be real head-scratchers. You know what? Understanding these concepts isn't just about rote memorization; it's about really getting how these chemical reactions tick. So let’s dive into a classic problem: what happens when you remove SO3 from a chemical equilibrium reaction?

First up, let’s set the stage. In a chemical equilibrium, reactions are happening at such a pace that the concentrations of reactants and products remain constant. Imagine a finely tuned see-saw; if you add weight on one side, the other will adjust to keep it balanced. This transformation paints a beautiful picture of how chemical systems strive to maintain stability. But what occurs when something is taken away, like SO3 in our case?

Now, when SO3 is yanked out of the equation (literally!), the equilibrium position doesn’t just stand idly by. According to Le Chatelier's principle—a fancy term whispering that systems try to counteract changes—removing SO3 leads the equilibrium to shift left! This shift is the system’s instinctive response to restore balance. Think of it as our see-saw tipping in the opposite direction, favoring the production of our reactants.

Here’s where it gets a tad spicy. As the equilibrium shifts to the left, more of the reactants, which are SO2 and O2 in this case, are used up—leading to their increased concentrations. That’s right! The concentrations of SO2 and O2 increase as they react with each other to form more SO3. But here’s the kicker: the phrasing in the answer suggests that the concentration of SO2 increases more than that of O2. Why is that? Well, it primarily hinges on the stoichiometry of the reaction—the mole ratios of the substances being consumed or produced can differ, causing one concentration to rise disproportionately.

Oh, and by the way, if you’re getting puzzled about stoichiometry, don’t sweat it! It’s just a way of understanding the relationship between the amounts of reactants and products. Picture it as the recipe for a cake; if you double the ingredients for flour and just add a bit of sugar, you might end up with a cake that’s a little more dry than you’d like. It’s all about balance, and chemistry is no different.

So what can we takeaway from this? If you're prepping for your chemistry exam, remember that understanding how reactions respond to changes is crucial. And just like any great experimental journey involves highs and lows, so does grasping these equilibrium concepts. As you look ahead, keep in mind the balance—how systems react to maintain stability—and you’ll be well on your way to mastering the intricacies of chemical equilibrium. Ready to tackle more? There’s always another layer to uncover in the stunning world of chemistry!