The equilibrium constant, Ke, for the following reaction is 6.30 at 723K. 2NH3(g) N2(g) + 3H2(g) If an equilibrium mixture of the three gases in a 14.3 L container at 723K contains 0.318 mol of NH3(g) and 0.364 mol of N2, the equilibrium concentration of H, is М.
The equilibrium constant, Ke, for the following reaction is 6.30 at 723K. 2NH3(g) N2(g) + 3H2(g) If an equilibrium mixture of the three gases in a 14.3 L container at 723K contains 0.318 mol of NH3(g) and 0.364 mol of N2, the equilibrium concentration of H, is М.
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...
Related questions
Question
![### Chemical Equilibrium Calculation
#### Problem Statement
The equilibrium constant, \( K_c \), for the following reaction is **6.30 at 723 K**.
\[
2 \text{NH}_3(g) \rightleftharpoons \text{N}_2(g) + 3 \text{H}_2(g)
\]
If an equilibrium mixture of the three gases in a **14.3 L container at 723 K** contains **0.318 mol of NH\(_3\)(g)** and **0.364 mol of N\(_2\)**, the equilibrium concentration of H\(_2\) is \_\_\_\_\_\_\_ M.
#### Explanation
To solve this problem:
1. **Determine the concentrations** of NH\(_3\) and N\(_2\) at equilibrium:
- Concentration of NH\(_3\): \(\frac{0.318 \text{ mol}}{14.3 \text{ L}}\)
- Concentration of N\(_2\): \(\frac{0.364 \text{ mol}}{14.3 \text{ L}}\)
2. **Set up the expression** for the equilibrium constant \( K_c \):
\[
K_c = \frac{[\text{N}_2][\text{H}_2]^3}{[\text{NH}_3]^2} = 6.30
\]
3. **Plug in** the known concentrations and solve for the concentration of H\(_2\).
#### Visual Explanation
The problem does not contain graphical elements, but solving it involves a straightforward calculation using the given formulae.
This approach ensures that the ratios and equilibrium relations are calculated correctly to find the missing concentration of H\(_2\).](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fbc7db68c-7828-4a06-bc34-18cdd71bf49b%2F3781c46f-57c0-445f-8d8a-cbd73a939cbf%2Fue7zrq_processed.png&w=3840&q=75)
Transcribed Image Text:### Chemical Equilibrium Calculation
#### Problem Statement
The equilibrium constant, \( K_c \), for the following reaction is **6.30 at 723 K**.
\[
2 \text{NH}_3(g) \rightleftharpoons \text{N}_2(g) + 3 \text{H}_2(g)
\]
If an equilibrium mixture of the three gases in a **14.3 L container at 723 K** contains **0.318 mol of NH\(_3\)(g)** and **0.364 mol of N\(_2\)**, the equilibrium concentration of H\(_2\) is \_\_\_\_\_\_\_ M.
#### Explanation
To solve this problem:
1. **Determine the concentrations** of NH\(_3\) and N\(_2\) at equilibrium:
- Concentration of NH\(_3\): \(\frac{0.318 \text{ mol}}{14.3 \text{ L}}\)
- Concentration of N\(_2\): \(\frac{0.364 \text{ mol}}{14.3 \text{ L}}\)
2. **Set up the expression** for the equilibrium constant \( K_c \):
\[
K_c = \frac{[\text{N}_2][\text{H}_2]^3}{[\text{NH}_3]^2} = 6.30
\]
3. **Plug in** the known concentrations and solve for the concentration of H\(_2\).
#### Visual Explanation
The problem does not contain graphical elements, but solving it involves a straightforward calculation using the given formulae.
This approach ensures that the ratios and equilibrium relations are calculated correctly to find the missing concentration of H\(_2\).
Expert Solution

This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
Step by step
Solved in 3 steps with 2 images

Knowledge Booster
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.Recommended textbooks for you

Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning

Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education

Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning

Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning

Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education

Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning

Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education

Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning

Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY