The equilibrium constant, Kc, for the following reaction is 57.6 at 277 K. 2CH₂Cl2 (9) CH4 (9) + CCl4 (9) When a sufficiently large sample of CH₂Cl₂ (g) is introduced into an evacuated vessel at 277 K, the equilibrium concentration of CC14 (g) is found to be 0.383 M. Calculate the concentration of CH₂Cl2 in the equilibrium mixture. [CH₂ Cl₂] = M
The equilibrium constant, Kc, for the following reaction is 57.6 at 277 K. 2CH₂Cl2 (9) CH4 (9) + CCl4 (9) When a sufficiently large sample of CH₂Cl₂ (g) is introduced into an evacuated vessel at 277 K, the equilibrium concentration of CC14 (g) is found to be 0.383 M. Calculate the concentration of CH₂Cl2 in the equilibrium mixture. [CH₂ Cl₂] = M
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
![The equilibrium constant, \( K_c \), for the following reaction is 57.6 at 277 K.
\[ 2 \text{CH}_2\text{Cl}_2 (g) \rightleftharpoons \text{CH}_4 (g) + \text{CCl}_4 (g) \]
When a sufficiently large sample of \(\text{CH}_2\text{Cl}_2 (g)\) is introduced into an evacuated vessel at 277 K, the equilibrium concentration of \(\text{CCl}_4 (g)\) is found to be 0.383 M.
Calculate the concentration of \(\text{CH}_2\text{Cl}_2\) in the equilibrium mixture.
\[
[\text{CH}_2\text{Cl}_2] = \boxed{\,\,} \,\, \text{M}
\]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F6e7279b6-864f-464c-a490-1592f397f56d%2Fde8005ae-d373-4d28-8f86-a5ea6f675e4d%2F5toy6cr_processed.png&w=3840&q=75)
Transcribed Image Text:The equilibrium constant, \( K_c \), for the following reaction is 57.6 at 277 K.
\[ 2 \text{CH}_2\text{Cl}_2 (g) \rightleftharpoons \text{CH}_4 (g) + \text{CCl}_4 (g) \]
When a sufficiently large sample of \(\text{CH}_2\text{Cl}_2 (g)\) is introduced into an evacuated vessel at 277 K, the equilibrium concentration of \(\text{CCl}_4 (g)\) is found to be 0.383 M.
Calculate the concentration of \(\text{CH}_2\text{Cl}_2\) in the equilibrium mixture.
\[
[\text{CH}_2\text{Cl}_2] = \boxed{\,\,} \,\, \text{M}
\]
![**Equilibrium Constant Calculation**
The equilibrium constant, \( K_c \), for the following reaction is \(1.80 \times 10^{-4}\) at 298 K.
\[ \text{NH}_4\text{HS} (s) \rightleftharpoons \text{NH}_3 (g) + \text{H}_2\text{S} (g) \]
**Problem Statement:**
Calculate the equilibrium concentration of \(\text{H}_2\text{S}\) when 0.525 moles of \(\text{NH}_4\text{HS} (s)\) are introduced into a 1.00 L vessel at 298 K.
\[[\text{H}_2\text{S}] = \_\_\_\_\_ \, \text{M} \]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F6e7279b6-864f-464c-a490-1592f397f56d%2Fde8005ae-d373-4d28-8f86-a5ea6f675e4d%2F7wv2qs_processed.png&w=3840&q=75)
Transcribed Image Text:**Equilibrium Constant Calculation**
The equilibrium constant, \( K_c \), for the following reaction is \(1.80 \times 10^{-4}\) at 298 K.
\[ \text{NH}_4\text{HS} (s) \rightleftharpoons \text{NH}_3 (g) + \text{H}_2\text{S} (g) \]
**Problem Statement:**
Calculate the equilibrium concentration of \(\text{H}_2\text{S}\) when 0.525 moles of \(\text{NH}_4\text{HS} (s)\) are introduced into a 1.00 L vessel at 298 K.
\[[\text{H}_2\text{S}] = \_\_\_\_\_ \, \text{M} \]
Expert Solution
Step 1: Defining equilibrium constant!
Answer:
For any reaction, value of equilibrium constant KC is equal to the ratio of molar concentration of products and reactants at equilibrium.
Step by step
Solved in 4 steps with 9 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