Consider the following gas reaction of A 2 ( shaded spheres) and B 2 ( unshaded spheres) A 2 (g) + B 2 (g) ⇌ 2 AB (g) Which container proceeds more to completion?

Hey guys, let's take a look at the practice question that was left for you at the bottom of the page. So here it says, consider the following gas reaction of A2. A2 are the shaded spheres and B are the unshaded spheres. Which container proceeds more to completion? So, first things first, we're going to say that the shaded spheres are the one that look like this. A2 looks like this. B2 are the unshaded spheres, so 2 b's together look like that and then a, b would be 1 shaded, one not shaded. Now, the key to this question was realizing what do we mean by the one that moves more to completion. Since we're talking about equilibrium here, we're talking about the k value. So really what I was asking was, which one has a larger equilibrium constant? The larger your k value, the more to the right the reaction proceeds. The more to the right it proceeds, the more product you make. Completion is based on how much product are you be able to isolate. Now, since we're talking about k here, we need to know the equilibrium expression for our equation. So, if we take a look, k would equal products over reactants. Since everything is a gas, we can keep everything. So, it would equal ab2 because remember whatever the coefficient is that becomes the power, divided by a2xb2. That's our equilibrium expression and that's what we would use for each one of these containers. The one that would give me the larger k value would be my answer. So here we'd say k equals, now ab, remember, is 1 shaded, one not shaded. Here there's only one of those kinds. So here it's going to be 1 squared, divided by, you have 3 that are shaded, those are a2s, and there's 3 of them. And then you have 3 that are not shaded, those are your b2s. So, you work that out, k equals 1 over 9. So, we just found the equilibrium constant for the first one. We do the same exact thing for the next one. K equals ab2 and we have 3 ab's here. So, it'd be 3 squared divided by a2, there's 2 of them, times b2, there's 2 of them. So this would equal 9 over 4. So we can just punch this into our calculator if we if we want. But obviously, 9 over 4 is definitely a number greater than 1. Whereas, onenine is a number less than 1. So here, since container B has a larger equilibrium constant, it proceeds more to completion than container a. So our answer here would be container b. B. Container B has a bigger k constant, therefore goes more to completion. That was the key to this question and just make note of this. When When we talk about completion, we're talking about equilibrium. We're just talking about the k value.

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1. The Chemical World9m
- The Scientific Method
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2. Measurement and Problem Solving2h 19m
3. Matter and Energy2h 15m
4. Atoms and Elements2h 33m
5. Molecules and Compounds1h 50m
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8. Quantities in Chemical Reactions1h 8m
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11 Gases2h 7m
12. Liquids, Solids, and Intermolecular Forces1h 11m
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15. Chemical Equilibrium1h 27m
16. Oxidation and Reduction1h 33m
17. Radioactivity and Nuclear Chemistry53m

15. Chemical Equilibrium

Le Chatelier's Principle

Introduction to Chemistry

15. Chemical Equilibrium

Le Chatelier's Principle

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Multiple Choice

Consider the following gas reaction of A₂ ( shaded spheres) and B₂ ( unshaded spheres)
A₂ (g) + B₂(g) ⇌ 2 AB (g)
Which container proceeds more to completion?

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Verified step by step guidance

Identify the reactants and products in the given chemical reaction: A2 (shaded spheres) and B2 (unshaded spheres) are the reactants, and 2 AB (one shaded and one unshaded sphere) is the product.

Examine the images of containers A and B. Count the number of A2, B2, and AB molecules in each container.

In container A, count the number of A2 and B2 molecules that have not reacted and the number of AB molecules formed.

In container B, count the number of A2 and B2 molecules that have not reacted and the number of AB molecules formed.

Compare the extent of reaction in both containers by evaluating the number of AB molecules formed relative to the initial number of A2 and B2 molecules. The container with more AB molecules indicates a reaction that has proceeded more to completion.