Calculate the value of K, in the following reaction if the equilibrium concentrations are [H,S] = 0.25 M, [H,] = 0.88 M, [S,] = 0.44M. 2 H,Se = 2 Hzie) '2(g)

Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
icon
Related questions
Question
### Calculating the Equilibrium Constant (K_eq)

To determine the value of the equilibrium constant (\(K_{eq}\)) for the given reaction, we use the equilibrium concentrations provided.

The reaction in question is:
\[ 2 \text{H}_2\text{S}_{(g)} \rightleftharpoons 2 \text{H}_{2(g)} + \text{S}_{2(g)} \]

The equilibrium concentrations are:
- \([\text{H}_2\text{S}] = 0.25 \, \text{M}\)
- \([\text{H}_2] = 0.88 \, \text{M}\)
- \([\text{S}_2] = 0.44 \, \text{M}\)

### Steps to Calculate \(K_{eq}\)

1. **Write the expression for the equilibrium constant (\(K_{eq}\)):**

   \[
   K_{eq} = \frac{[\text{H}_2]^2 [\text{S}_2]}{[\text{H}_2\text{S}]^2}
   \]

2. **Substitute the equilibrium concentrations into the expression:**

   \[
   K_{eq} = \frac{(0.88)^2 \cdot (0.44)}{(0.25)^2}
   \]

3. **Perform the calculations:**
   
   - Calculate the numerator: \((0.88)^2 \times (0.44) = 0.7744 \times 0.44 = 0.340736\)
   - Calculate the denominator: \((0.25)^2 = 0.0625\)

   \[
   K_{eq} = \frac{0.340736}{0.0625} \approx 5.45
   \]

### Result

The value of the equilibrium constant (\(K_{eq}\)) for the reaction is approximately **5.45**.

### Explanation of Diagrams and Graphs

There are no diagrams or graphs included in this content. The text focuses on presenting and solving a chemical equilibrium problem through mathematical expressions and equilibrium concentrations.
Transcribed Image Text:### Calculating the Equilibrium Constant (K_eq) To determine the value of the equilibrium constant (\(K_{eq}\)) for the given reaction, we use the equilibrium concentrations provided. The reaction in question is: \[ 2 \text{H}_2\text{S}_{(g)} \rightleftharpoons 2 \text{H}_{2(g)} + \text{S}_{2(g)} \] The equilibrium concentrations are: - \([\text{H}_2\text{S}] = 0.25 \, \text{M}\) - \([\text{H}_2] = 0.88 \, \text{M}\) - \([\text{S}_2] = 0.44 \, \text{M}\) ### Steps to Calculate \(K_{eq}\) 1. **Write the expression for the equilibrium constant (\(K_{eq}\)):** \[ K_{eq} = \frac{[\text{H}_2]^2 [\text{S}_2]}{[\text{H}_2\text{S}]^2} \] 2. **Substitute the equilibrium concentrations into the expression:** \[ K_{eq} = \frac{(0.88)^2 \cdot (0.44)}{(0.25)^2} \] 3. **Perform the calculations:** - Calculate the numerator: \((0.88)^2 \times (0.44) = 0.7744 \times 0.44 = 0.340736\) - Calculate the denominator: \((0.25)^2 = 0.0625\) \[ K_{eq} = \frac{0.340736}{0.0625} \approx 5.45 \] ### Result The value of the equilibrium constant (\(K_{eq}\)) for the reaction is approximately **5.45**. ### Explanation of Diagrams and Graphs There are no diagrams or graphs included in this content. The text focuses on presenting and solving a chemical equilibrium problem through mathematical expressions and equilibrium concentrations.
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 3 steps with 1 images

Blurred answer
Knowledge Booster
Chemical Equilibrium
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Similar questions
  • SEE MORE QUESTIONS
Recommended textbooks for you
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY