SO₂Cl₂ (g) SO₂(g) + O₂(g) K = 0.520 @ 400 K; X = 0.515 [SO₂Cl₂] = 1.50 M [SO₂] = 0.200 M [Cl₂] = 0.200 M What is the concentration of SO2Cl2 at equilibrium? [SO₂Cl₂] = [?] M [SO,CI₂], M Enter
SO₂Cl₂ (g) SO₂(g) + O₂(g) K = 0.520 @ 400 K; X = 0.515 [SO₂Cl₂] = 1.50 M [SO₂] = 0.200 M [Cl₂] = 0.200 M What is the concentration of SO2Cl2 at equilibrium? [SO₂Cl₂] = [?] M [SO,CI₂], M Enter
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...
Related questions
Concept explainers
Ionic Equilibrium
Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.
Arrhenius Acid
Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.
Bronsted Lowry Base In Inorganic Chemistry
Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.
Question
![### Chemical Equilibrium Problem
#### Given Reaction and Parameters:
\[ \text{SO}_2\text{Cl}_2(g) \rightleftharpoons \text{SO}_2(g) + \text{Cl}_2(g) \]
- **Equilibrium Constant (K):** 0.520 at 400 K
- **Extent of Reaction (X):** 0.515
#### Initial Concentrations:
- \[\text{[SO}_2\text{Cl}_2] = 1.50\text{ M}\]
- \[\text{[SO}_2] = 0.200\text{ M}\]
- \[\text{[Cl}_2] = 0.200\text{ M}\]
#### Objective:
**Determine the concentration of \(\text{SO}_2\text{Cl}_2\) at equilibrium.**
#### Calculation:
1. Utilize the given parameters and initial concentrations to calculate the equilibrium concentration of \(\text{SO}_2\text{Cl}_2\).
#### Answer Submission:
- **[SO_2Cl_2] at Equilibrium:** \(\big[ \text{?} \big] \, \text{M}\)
- **Input Box:** To submit your calculated concentration of \(\text{SO}_2\text{Cl}_2\).
- **Enter Button:** Click to submit your answer.
Submit your answer in the provided input box and then press the "Enter" button to check if your calculated concentration is correct.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Faf34c8cd-64a3-45bc-a064-10a06ef3c764%2F5acfb7f3-ea54-4b59-b299-808f3740b5fa%2F7y6vaww_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Chemical Equilibrium Problem
#### Given Reaction and Parameters:
\[ \text{SO}_2\text{Cl}_2(g) \rightleftharpoons \text{SO}_2(g) + \text{Cl}_2(g) \]
- **Equilibrium Constant (K):** 0.520 at 400 K
- **Extent of Reaction (X):** 0.515
#### Initial Concentrations:
- \[\text{[SO}_2\text{Cl}_2] = 1.50\text{ M}\]
- \[\text{[SO}_2] = 0.200\text{ M}\]
- \[\text{[Cl}_2] = 0.200\text{ M}\]
#### Objective:
**Determine the concentration of \(\text{SO}_2\text{Cl}_2\) at equilibrium.**
#### Calculation:
1. Utilize the given parameters and initial concentrations to calculate the equilibrium concentration of \(\text{SO}_2\text{Cl}_2\).
#### Answer Submission:
- **[SO_2Cl_2] at Equilibrium:** \(\big[ \text{?} \big] \, \text{M}\)
- **Input Box:** To submit your calculated concentration of \(\text{SO}_2\text{Cl}_2\).
- **Enter Button:** Click to submit your answer.
Submit your answer in the provided input box and then press the "Enter" button to check if your calculated concentration is correct.
![**Chemical Equilibrium and Reaction Quotient Calculation**
In this exercise, we will determine the reaction quotient, \( Q \), for the chemical reaction:
\[ \text{H}_2(\text{g}) + \text{CO}_2(\text{g}) \rightleftharpoons \text{CO}(\text{g}) + \text{H}_2\text{O}(\text{g}) \]
Given:
- Equilibrium constant, \( K \), is 0.137 at 823 K.
**Initial Conditions:**
- Partial pressure of Hydrogen (\( P_{\text{H}_2} \)) = 0.50 atm
- Partial pressure of Carbon Dioxide (\( P_{\text{CO}_2} \)) = 0.75 atm
- Partial pressure of Carbon Monoxide (\( P_{\text{CO}} \)) = 1.0 atm
- Partial pressure of Water (\( P_{\text{H}_2\text{O}} \)) = 2.0 atm
**Question:**
What is the reaction quotient, \( Q \), based on the given initial conditions?
**Reaction Quotient calculation:**
The reaction quotient \( Q \) is calculated using the formula:
\[ Q = \frac{P_{\text{CO}} \cdot P_{\text{H}_2\text{O}}}{P_{\text{H}_2} \cdot P_{\text{CO}_2}} \]
Substituting the given values:
\[ Q = \frac{(1.0 \, \text{atm}) \cdot (2.0 \, \text{atm})}{(0.50 \, \text{atm}) \cdot (0.75 \, \text{atm})} \]
**Enter the Reaction Quotient:**
There is an input field where the value of \( Q \) should be calculated and entered.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Faf34c8cd-64a3-45bc-a064-10a06ef3c764%2F5acfb7f3-ea54-4b59-b299-808f3740b5fa%2Fp71b8x_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Chemical Equilibrium and Reaction Quotient Calculation**
In this exercise, we will determine the reaction quotient, \( Q \), for the chemical reaction:
\[ \text{H}_2(\text{g}) + \text{CO}_2(\text{g}) \rightleftharpoons \text{CO}(\text{g}) + \text{H}_2\text{O}(\text{g}) \]
Given:
- Equilibrium constant, \( K \), is 0.137 at 823 K.
**Initial Conditions:**
- Partial pressure of Hydrogen (\( P_{\text{H}_2} \)) = 0.50 atm
- Partial pressure of Carbon Dioxide (\( P_{\text{CO}_2} \)) = 0.75 atm
- Partial pressure of Carbon Monoxide (\( P_{\text{CO}} \)) = 1.0 atm
- Partial pressure of Water (\( P_{\text{H}_2\text{O}} \)) = 2.0 atm
**Question:**
What is the reaction quotient, \( Q \), based on the given initial conditions?
**Reaction Quotient calculation:**
The reaction quotient \( Q \) is calculated using the formula:
\[ Q = \frac{P_{\text{CO}} \cdot P_{\text{H}_2\text{O}}}{P_{\text{H}_2} \cdot P_{\text{CO}_2}} \]
Substituting the given values:
\[ Q = \frac{(1.0 \, \text{atm}) \cdot (2.0 \, \text{atm})}{(0.50 \, \text{atm}) \cdot (0.75 \, \text{atm})} \]
**Enter the Reaction Quotient:**
There is an input field where the value of \( Q \) should be calculated and entered.
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 2 steps with 1 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 for Engineering Students
Chemistry
ISBN:
9781337398909
Author:
Lawrence S. Brown, Tom Holme
Publisher:
Cengage Learning
Chemistry: Principles and Practice
Chemistry
ISBN:
9780534420123
Author:
Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry for Engineering Students
Chemistry
ISBN:
9781337398909
Author:
Lawrence S. Brown, Tom Holme
Publisher:
Cengage Learning
Chemistry: Principles and Practice
Chemistry
ISBN:
9780534420123
Author:
Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry: An Atoms First Approach
Chemistry
ISBN:
9781305079243
Author:
Steven S. Zumdahl, Susan A. Zumdahl
Publisher:
Cengage Learning
Introduction to General, Organic and Biochemistry
Chemistry
ISBN:
9781285869759
Author:
Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres
Publisher:
Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:
9781337399074
Author:
John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:
Cengage Learning