Y Y Part A Given the concentrations, calculate the equilibrium constant for this reaction: 2SO₂(g) + O₂(g) 2SO3(g) At equilibrium, the molar concentrations for reactants and products are found to be [SO₂] -0.48 M. [0₂] -0.40 M, and [SO] 1.12 M What is the equilibrium constant (Ke) for this reaction? Express your answer using two significant figures. ▸ View Available Hint(s) Ke= Submit Part B 15. ΑΣΦ [s0,² [S0₂²10₂ The concentration of SO₂ (g) is increased to 1.48 M, disrupting equilibrium Calculate the new ratio of products to reactants with this higher concentration of sulfur dioxide. Assume that the reaction has not yet regained equilibrium Express your answer using two significant figures. ▸View Available Hint(s) VO → | ΑΣΦ SWIG ? ?
Y Y Part A Given the concentrations, calculate the equilibrium constant for this reaction: 2SO₂(g) + O₂(g) 2SO3(g) At equilibrium, the molar concentrations for reactants and products are found to be [SO₂] -0.48 M. [0₂] -0.40 M, and [SO] 1.12 M What is the equilibrium constant (Ke) for this reaction? Express your answer using two significant figures. ▸ View Available Hint(s) Ke= Submit Part B 15. ΑΣΦ [s0,² [S0₂²10₂ The concentration of SO₂ (g) is increased to 1.48 M, disrupting equilibrium Calculate the new ratio of products to reactants with this higher concentration of sulfur dioxide. Assume that the reaction has not yet regained equilibrium Express your answer using two significant figures. ▸View Available Hint(s) VO → | ΑΣΦ SWIG ? ?
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
![Le Châtelier Principle
Learning Goal:
To use the equilibrium constant and Le Châtelier's
principle to determine how a reaction will respond
to external factors.
A reaction is at equilibrium when the concentrations
of the reactants and products no longer change
over time. This does not mean the reaction is over,
rather, two competing reactions continue to occur
simultaneously at equal rates. The two competing
reactions are the forward reaction (reactants →
products) and the reverse reaction (products →
reactants).
If a reaction at equilibrium is subjected to a stress,
the concentrations of reactants and products adjust
to reestablish equilibrium. This is called Le
Châtelier's principle. A stress might be a change in
the concentration of reactants or products, a
change in the volume of the reaction container, a
change in temperature, or the addition of a catalyst.
0 O
▾
Part A
Given the concentrations, calculate the equilibrium constant for this
reaction:
2SO2(g) +O2(g) = 2SO3(g)
At equilibrium, the molar concentrations for reactants and products are
found to be [SO₂] = 0.48 M. [0₂] -0.40 M, and
[SO3] 1.12 M. What is the equilibrium constant (Ke) for this
reaction?
Express your answer using two significant figures.
▸ View Available Hint(s)
▾
Ke=
Submit
Part B
——| ΑΣΦ
[So, ²
[SO₂]²[0₂]
Submit
The concentration of SO₂ (g) is increased to 1.48 M, disrupting
equilibrium Calculate the new ratio of products to reactants with this
higher concentration of sulfur dioxide. Assume that the reaction has
not yet regained equilibrium.
Express your answer using two significant figures.
View Available Hint(s)
Part D
VO
Part C Complete previous part(s)
ΑΣΦ
Review | Constants | Periodic Table
decrease volume
h
MX... A
The following reaction is at equilibrium in a 2.0-L vessel:
PCh (g) +Ch (g) - PCs (g), Ke=2.4 x 10¹
How do the following actions affect the equilibrium of the reaction?
Drag the appropriate items to their respective bins.
View Available Hint(s)
increase volume
?
4x
?
add catalyst
Rest
add chlorine
7:05 PM](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F7f185ec2-8c2e-4aee-a8f1-0a1f41f71cb3%2Fb6f7fe0f-1b80-40aa-9201-b3122f3f60b6%2Fuuwkdw_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Le Châtelier Principle
Learning Goal:
To use the equilibrium constant and Le Châtelier's
principle to determine how a reaction will respond
to external factors.
A reaction is at equilibrium when the concentrations
of the reactants and products no longer change
over time. This does not mean the reaction is over,
rather, two competing reactions continue to occur
simultaneously at equal rates. The two competing
reactions are the forward reaction (reactants →
products) and the reverse reaction (products →
reactants).
If a reaction at equilibrium is subjected to a stress,
the concentrations of reactants and products adjust
to reestablish equilibrium. This is called Le
Châtelier's principle. A stress might be a change in
the concentration of reactants or products, a
change in the volume of the reaction container, a
change in temperature, or the addition of a catalyst.
0 O
▾
Part A
Given the concentrations, calculate the equilibrium constant for this
reaction:
2SO2(g) +O2(g) = 2SO3(g)
At equilibrium, the molar concentrations for reactants and products are
found to be [SO₂] = 0.48 M. [0₂] -0.40 M, and
[SO3] 1.12 M. What is the equilibrium constant (Ke) for this
reaction?
Express your answer using two significant figures.
▸ View Available Hint(s)
▾
Ke=
Submit
Part B
——| ΑΣΦ
[So, ²
[SO₂]²[0₂]
Submit
The concentration of SO₂ (g) is increased to 1.48 M, disrupting
equilibrium Calculate the new ratio of products to reactants with this
higher concentration of sulfur dioxide. Assume that the reaction has
not yet regained equilibrium.
Express your answer using two significant figures.
View Available Hint(s)
Part D
VO
Part C Complete previous part(s)
ΑΣΦ
Review | Constants | Periodic Table
decrease volume
h
MX... A
The following reaction is at equilibrium in a 2.0-L vessel:
PCh (g) +Ch (g) - PCs (g), Ke=2.4 x 10¹
How do the following actions affect the equilibrium of the reaction?
Drag the appropriate items to their respective bins.
View Available Hint(s)
increase volume
?
4x
?
add catalyst
Rest
add chlorine
7:05 PM
Expert Solution
Step 1
A.) To calculate the Kc, first we have to write an expression for Kc for given equilibrium reaction. Then using the concentration we can calculate Kc.
B.) To calculate the ratio, we have to plug the new concentration of SO2 .
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