Consider the following equilibrium: 2 H 2 (g) + S 2 (g) ⇌ 2 H 2 S(g) K c = 1.08 × 10 7 at 700°C (b) Does the equilibrium mixture contain mostly H 2 and S 2 or mostly H 2 S?

hey everyone in this example, we need to figure out which of the below statement is correct for the given reaction. So the first thing we should notice about this given reaction is that this is the equilibrium constant value or the equilibrium value and we want to recognize that it's a very small value. We have times 10 to the negative 20th power. And so we would say that the equilibrium constant is much smaller than the number one. It's a very low and negative number. And whenever we have the equilibrium constant being a low negative number, less than one, this means that the reactant are favored and we also want to recall that when we have an equilibrium constant, that is much greater than one. That means products are favored. Now in this case, based on this equilibrium constant value, we would go ahead, go ahead and confirm that our Equilibrium constant is much smaller than one. And so reactant are favored. And so we would be able to agree with answer choice A which states that there is a higher concentration of reactant that equilibrium than compared to the products. And that is correct again, because we determined our equilibrium constant is less than one and so reactant our favorite. So their concentration will be higher. Now, statement B says, once the equilibrium state is attained, the concentration of reactant become zero, that's going to also be ruled that's going to be ruled out in this case. And that's because at equilibrium we should have some reactant and some product so be would not make sense. Moving on to see it says the concentration of the reactant and the products are equal at equilibrium. Now, in this case, we know that this is not true and that's because we are given an equilibrium constant that favors reactant. And so the concentration of the reactant and products are not equal according to this reaction. So we would rule out c lastly we would rule out deep because again, we determined that A agrees with the fact that the reactant are favored based on our equilibrium constant value for the reaction. So A is the final answer to complete this example. I hope that everything we reviewed was clear. But if you have any questions, please leave them down below and I will see everyone in the next practice video.

Ch.15 - Chemical Equilibrium

Brown - Chemistry: The Central Science 15th Edition

Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Not the one you use?Change textbook

All textbooks

Brown 15th Edition

Ch.15 - Chemical Equilibrium

Problem 24b

Chapter 15, Problem 24b

Consider the following equilibrium: 2 H₂(g) + S₂(g) ⇌ 2 H₂S(g) K_c = 1.08 × 10⁷ at 700°C (b) Does the equilibrium mixture contain mostly H₂ and S₂ or mostly H₂S?

Verified step by step guidance

Understand the equilibrium expression: The equilibrium constant (Kc) is given for the reaction 2 H2(g) + S2(g) ⇌ 2 H2S(g). It is a measure of the ratio of the concentration of products to reactants at equilibrium.

Write the expression for Kc: The equilibrium constant expression for the reaction is Kc = [H2S]^2 / ([H2]^2 * [S2]).

Analyze the value of Kc: The given Kc value is 1.08 × 10^7, which is a very large number. This indicates that at equilibrium, the concentration of the products (H2S) is much greater than the concentration of the reactants (H2 and S2).

Interpret the equilibrium position: Since Kc is significantly greater than 1, the equilibrium position is heavily shifted towards the products, meaning the equilibrium mixture contains mostly H2S.

Conclude the analysis: Based on the large Kc value, the equilibrium mixture will predominantly consist of H2S rather than H2 and S2.

Verified video answer for a similar problem:

This video solution was recommended by our tutors as helpful for the problem above.

Video duration:

Was this helpful?

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Chemical Equilibrium

Chemical equilibrium occurs when the rates of the forward and reverse reactions are equal, resulting in constant concentrations of reactants and products. In this state, the system is dynamic, meaning that reactions continue to occur, but there is no net change in the concentrations. Understanding this concept is crucial for analyzing how changes in conditions affect the position of equilibrium.

Equilibrium Constant (Kc)

The equilibrium constant, Kc, quantifies the ratio of the concentrations of products to reactants at equilibrium, raised to the power of their stoichiometric coefficients. A large Kc value, such as 1.08 × 107, indicates that at equilibrium, the concentration of products is much greater than that of reactants, suggesting that the reaction favors the formation of products.

Le Chatelier's Principle

Le Chatelier's Principle states that if a system at equilibrium is subjected to a change in concentration, temperature, or pressure, the system will adjust to counteract that change and restore a new equilibrium. This principle helps predict how the equilibrium position will shift in response to changes, such as adding or removing reactants or products.

Consider the following equilibrium: 2 H2(g) + S2(g) ⇌ 2 H2S(g) Kc = 1.08 × 107 at 700°C (b) Does the equilibrium mixture contain mostly H2 and S2 or mostly H2S?

Verified video answer for a similar problem:

Key Concepts

Chemical Equilibrium

Equilibrium Constant (K<sub>c</sub>)

Le Chatelier's Principle

Consider the following equilibrium: 2 H₂(g) + S₂(g) ⇌ 2 H₂S(g) K_c = 1.08 × 10⁷ at 700°C (b) Does the equilibrium mixture contain mostly H₂ and S₂ or mostly H₂S?