Consider the following elementary reaction: CFC1₂(g) → CFC1₂(g) +Cl(g) Suppose we let k₁ stand for the rate constant of this reaction, and k₁ stand for the rate constant of the reverse reaction. Write an expression that gives the equilibrium concentration of CFC13 in terms of k₁, k₁, and the equilibrium concentrations of CFC1₂ and Cl. [CFCI,]= X olo 9 5
Consider the following elementary reaction: CFC1₂(g) → CFC1₂(g) +Cl(g) Suppose we let k₁ stand for the rate constant of this reaction, and k₁ stand for the rate constant of the reverse reaction. Write an expression that gives the equilibrium concentration of CFC13 in terms of k₁, k₁, and the equilibrium concentrations of CFC1₂ and Cl. [CFCI,]= X olo 9 5
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Question
Consider the following elementary reaction:
CFCl3
(g)
→CFCl2
(g)
+Cl
(g)Suppose we let
k1
stand for the rate constant of this reaction, and
k−1
stand for the rate constant of the reverse reaction.
Write an expression that gives the equilibrium concentration of
CFCl3
in terms of
k1
,
k−1
, and the equilibrium concentrations of
CFCl2
and
Cl
.
![### Elementary Reaction Analysis
Consider the following elementary reaction:
\[ \text{CFCl}_3(g) \rightarrow \text{CFCl}_2(g) + \text{Cl}(g) \]
Suppose we let \( k_1 \) stand for the rate constant of this reaction, and \( k_{-1} \) stand for the rate constant of the reverse reaction.
#### Task
Write an expression that gives the equilibrium concentration of \(\text{CFCl}_3\) in terms of \( k_1 \), \( k_{-1} \), and the equilibrium concentrations of \(\text{CFCl}_2\) and \(\text{Cl}\).
##### Solution
\[ [\text{CFCl}_3] = \]
The interface indicated allows you to enter the mathematical expressions using provided tools, such as symbols for square root, superscripts, and other common mathematical notations.
By considering the rates of the forward and reverse reactions and using the principles of chemical equilibrium, you can derive an expression for the equilibrium concentration of \(\text{CFCl}_3\).](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F9757754f-3312-4a82-9461-9956fc98753f%2F602809a2-f848-46ce-a0ac-447628b076a1%2F5wfrpec_processed.png&w=3840&q=75)
Transcribed Image Text:### Elementary Reaction Analysis
Consider the following elementary reaction:
\[ \text{CFCl}_3(g) \rightarrow \text{CFCl}_2(g) + \text{Cl}(g) \]
Suppose we let \( k_1 \) stand for the rate constant of this reaction, and \( k_{-1} \) stand for the rate constant of the reverse reaction.
#### Task
Write an expression that gives the equilibrium concentration of \(\text{CFCl}_3\) in terms of \( k_1 \), \( k_{-1} \), and the equilibrium concentrations of \(\text{CFCl}_2\) and \(\text{Cl}\).
##### Solution
\[ [\text{CFCl}_3] = \]
The interface indicated allows you to enter the mathematical expressions using provided tools, such as symbols for square root, superscripts, and other common mathematical notations.
By considering the rates of the forward and reverse reactions and using the principles of chemical equilibrium, you can derive an expression for the equilibrium concentration of \(\text{CFCl}_3\).
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