The Equilibrium Constant - Online Tutor, Practice Problems & Exam Prep

The Equilibrium Constant Concept 1

Hey guys, in this brand new video, we're going to take a look at the equilibrium constant. Now, we're going to say that the variable we use to illustrate our equilibrium constant is the variable k. We're going to say k is a number equal to the ratio of products to reactants at a given temperature. Why do I say at a given temperature? Because we're going to say that temperature directly affects our equilibrium constant k. Increasing the temperature will increase our k value. Decreasing the temperature will decrease our k value. Now, we're going to say it's a ratio of products to reactants, so we're going to say here that \( k = \frac{\text{products}}{\text{reactants}} \). Now, we're going to say that k is important because its magnitude tells us how far to the left or to the right our chemical reaction is at a given temperature. So we're going to say if \( k > 1 \), then products are favored over reactants. Think about it. This makes sense because we said \( k = \frac{\text{products}}{\text{reactants}} \). So let's say our products are 10 and our reactants are 1. \( k = 10 \), definitely greater than 1. We're going to say when products are favored over our reactants, that means we're making more products. How do we make more products? By going in the forward direction. So the forward direction would be favored. Now in the opposite way, if \( k < 1 \), so let's say we have in this case, products are 1 but our reactants are 10. We'd have a \( k < 1 \). So in this case, if \( k < 1 \), then reactants are favored over products, which means our reaction is heading in the reverse direction. So the reverse direction would be favored. Just remember these two differences, when \( k > 1 \) and when \( k < 1 \). Now, what if we say \( k = 1 \)? We know that this is products over reactants, so that means that our products and reactants would have to be equal. Let's say they're both 10. \( \frac{10}{10} = 1 \). So when \( k = 1 \), we're going to say both our reactant and our product amounts are equal to one another. Now we're going to say the equilibrium constant \( k \) takes into account all the states of matter except 2. It doesn't look at solids and it doesn't look at liquids. It ignores those 2 states of matter.

The Equilibrium Constant Example 1

So it looks at, it only cares about really gases and also aqueous. Aqueous just means that the solvent is water, so a compound is dissolved in water. It would be aqueous. Now, knowing this, let's take a look at the following example. It says, Write the equilibrium expression for the following reaction. Here we have N2O5 (aqueous) gives us 4NO2 (aqueous) plus O2 (aqueous). It's important to look at the phases because remember if it's a solid or a liquid, we ignore it. Now we're going to say here k= products over reactants. So we're going to have our products as NO₂ and remember, you have to use the coefficients in these calculations. The number in front of NO₂ is a 4, so that 4 will become the power. So it's going to be NO₂ to the 4 times O₂. O₂ just has a coefficient of 1 in front of it, which we don't have to show. Divided by N₂O₅. Again, the coefficient in front of N₂O₅ is a 2, so that becomes the power. So we would say that this represents our equilibrium expression or our equilibrium equation. Same thing. Equilibrium expression, equilibrium equation. Now that we've seen this one, let's look at B.

For B, we're going to say here, we're going to ignore this compound because it's a solid and we're going to ignore this compound because it's a solid. Here we're going to say k= products over reactants like before. But here's the thing, we're going to say we don't have any products available. But you have to put something on top. We're going to say it's equal to 1. Solids and liquids are ignored and in place of them, we're going to put 1. We're going to say this because things such as pressure don't really affect solids and liquids like they do gases and aqueous compounds. That's why they're equal to 1 because their number is being held constant. So we're going to replace solids and liquids with the number 1. And on the bottom we'd have O2. Now, a different way your professor could give you this is, we know there's a one here, so this could also be O2-1. So be aware of both types of answers. Both are correct. Both are saying the same thing. Inverse 1 just means 1 over whatever it is.

For the next one, again we ignore solids. The only thing that we don't ignore is this gas. Here, k= products over reactants, so just equal Xe3 because of the 3 over 1. But we don't need to put the one because anything over 1 is the same exact thing. So that would be our equilibrium C. We ignore the solids and the liquids.

Now that you've seen this, I want you guys to attempt to answer a question that follows this one, the practice one. Here, I want you to tell me who's greater in amount? Is it products or is it reactants? From that, you have to remember what do we say about K. When it's greater than 1, who's favored? When it's less than 1, who's favored? When it's equal to 1 who's favored. Remembering that will be a great way for you to approach this problem. Good luck, guys.

State which is greater in amount: reactants or products, based on the given equilibrium constant, K.

a) N₂ (g) + O₂ (g) ⇌ 2 NO (g) K = 1.0 x 10²⁰

b) 2 CO (g) + O₂ (g) ⇌ 2 CO₂ (g) K = 2.2 x 10^-22

c) 2 BrCl (g) ⇌ Br₂ (g) + Cl₂ (g) K = 1

• A. a) products, b) products, c) reactants
• B. a) reactants, b) products, c) reactants
• C. a) products, b) reactants, c) equal
• D. a) reactants, b) products, c) equal

The decomposition of nitrogen monoxide can be achieved under high temperatures to create the products of nitrogen and oxygen gas. 

6 NO(aq) ⇌ 3 N₂(aq) + 3 O₂(aq) 

a) What is the equilibrium equation for the reaction above?

b) What is the equilibrium expression for the reverse reaction. 

• A.
• B.
• C.
• D.

The equilibrium constant, K, for 2 NO (g) + O₂ (g) ⇌ 2 NO₂ (g) is 6.9 x 10². 

What is the [NO] in an equilibrium mixture of gaseous NO, O₂, and NO₂ at 500 K that contains 1.5 x 10 ^–2 M O₂ and 4.3 x 10 ^–3 M NO₂?

• A. 4.15 x 10^-4 M
• B. 1.34 x 10^-3 M
• C. 2.04 x 10^-2 M
• D. 1.80 x 10^-6 M

Here’s what students ask on this topic:

What is the equilibrium constant and how is it calculated?

The equilibrium constant, denoted as K, is a number that represents the ratio of the concentrations of products to reactants at equilibrium for a given chemical reaction at a specific temperature. It is calculated using the formula:

$K=\frac{\mathrm{[products]}}{\mathrm{[reactants]}}$

Here, the concentrations of the products and reactants are raised to the power of their respective coefficients in the balanced chemical equation. Note that solids and liquids are not included in this ratio.

How does temperature affect the equilibrium constant?

Temperature has a direct effect on the equilibrium constant (K). If the temperature increases, the value of K will also increase for endothermic reactions, meaning the reaction favors the formation of products. Conversely, for exothermic reactions, an increase in temperature will decrease the value of K, favoring the formation of reactants. Therefore, the equilibrium constant is temperature-dependent, and any change in temperature can shift the position of equilibrium.

What does it mean if the equilibrium constant (K) is greater than 1?

If the equilibrium constant (K) is greater than 1, it indicates that the concentration of products is greater than the concentration of reactants at equilibrium. This means that the reaction favors the formation of products, and the forward reaction is predominant. For example, if K = 10, the products are ten times more concentrated than the reactants.

Why are solids and liquids not included in the equilibrium constant expression?

Solids and liquids are not included in the equilibrium constant expression because their concentrations do not change during the reaction. The concentration of a pure solid or liquid is constant and does not affect the equilibrium position. Therefore, only the concentrations of gases and aqueous solutions are considered when calculating the equilibrium constant.

What happens when the equilibrium constant (K) is equal to 1?

When the equilibrium constant (K) is equal to 1, it means that the concentrations of products and reactants are equal at equilibrium. This indicates that neither the forward nor the reverse reaction is favored, and the system is in a state of dynamic balance. For example, if both the products and reactants have a concentration of 10, then K = 10/10 = 1.