Homework Help is Here – Start Your Trial Now!
Science
Chemistry
4. In a container at 2000°C, carbon dioxide decomposes into carbon monoxide and oxygen gas. The equilibrium constant, K, is 6.40 x 107. When the system is analyzed, the concentrations are found to be as follows: [CO] is 0.220 mol/L. [CO] is 3.0 x 102 mol/L, and [O2(g)] is 2.8 x 10 mol/L. Determine whether the system is at equilibrium (i.e. comparing Q to K), and if it is not, predict the direction in which the reaction will proceed to reach equilibrium.

4. In a container at 2000°C, carbon dioxide decomposes into carbon monoxide and oxygen gas. The equilibrium constant, K, is 6.40 x 107. When the system is analyzed, the concentrations are found to be as follows: [CO] is 0.220 mol/L. [CO] is 3.0 x 102 mol/L, and [O2(g)] is 2.8 x 10 mol/L. Determine whether the system is at equilibrium (i.e. comparing Q to K), and if it is not, predict the direction in which the reaction will proceed to reach equilibrium.

Chemistry for Engineering Students
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter12: Chemical Equilibrium
Section: Chapter Questions
Problem 12.41PAE: Because calcium carbonate is a sink for CO32- in a lake, the student in Exercise 12.39 decides to go...
See similar textbooks
icon
Related questions
Question

Plz complete this question, thanks

4. In a container at 2000˚C, carbon dioxide decomposes into carbon monoxide and oxygen gas. The equilibrium constant, K, is 6.40 x 107. When the system is analyzed, the concentrations are found to be as follows: [CO] is 0.220 mol/L. [CO] is 3.0 x 102 mol/L, and [O2(g)] is 2.8 x 10³ mol/L. Determine whether the system is at equilibrium (i.e. comparing Q to K), and if it is not, predict the direction in which the reaction will proceed to reach equilibrium.
Transcribed Image Text:4. In a container at 2000˚C, carbon dioxide decomposes into carbon monoxide and oxygen gas. The equilibrium constant, K, is 6.40 x 107. When the system is analyzed, the concentrations are found to be as follows: [CO] is 0.220 mol/L. [CO] is 3.0 x 102 mol/L, and [O2(g)] is 2.8 x 10³ mol/L. Determine whether the system is at equilibrium (i.e. comparing Q to K), and if it is not, predict the direction in which the reaction will proceed to reach equilibrium.
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 4 steps

SEE SOLUTIONCheck out a sample Q&A here
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 for Engineering Students
Chemistry for Engineering Students
Chemistry
ISBN:
9781337398909
Author:
Lawrence S. Brown, Tom Holme
Publisher:
Cengage Learning
Chemistry: The Molecular Science
Chemistry: The Molecular Science
Chemistry
ISBN:
9781285199047
Author:
John W. Moore, Conrad L. Stanitski
Publisher:
Cengage Learning
Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
Chemistry
ISBN:
9781337399074
Author:
John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:
Cengage Learning
Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
Chemistry
ISBN:
9781133949640
Author:
John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:
Cengage Learning
Introductory Chemistry: A Foundation
Introductory Chemistry: A Foundation
Chemistry
ISBN:
9781337399425
Author:
Steven S. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
SEE MORE TEXTBOOKS