Show all your work to receive full credit. 1. An equilibrium involving the carbonate and bicarbonate ions exists in natural waters. HCO3 (a9) = H†(ag) + CO3²¯(ag) Assuming that the reactions in both directions are elementary processes, do the following. (a) Write rate expressions for the forward and reverse reactions. Forward rate = k+1 %3D Reverse rate = k-1 (b) (b) Write an expression for the equilibrium constant based on the rates of the forward and reverse reactions.
Show all your work to receive full credit. 1. An equilibrium involving the carbonate and bicarbonate ions exists in natural waters. HCO3 (a9) = H†(ag) + CO3²¯(ag) Assuming that the reactions in both directions are elementary processes, do the following. (a) Write rate expressions for the forward and reverse reactions. Forward rate = k+1 %3D Reverse rate = k-1 (b) (b) Write an expression for the equilibrium constant based on the rates of the forward and reverse reactions.
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...
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An equilibrium involving the carbonate and bicarbonate ions exist in natural waters.
HCO3-(aq) -> H+(ag) + CO32-(aq)
Assuming that the reactions in both directions are elementary processes, do the following write rate expressions for the forward and reverse reactions.
![**Problem Solving Chapter 12**
Show all your work to receive full credit.
1. An equilibrium involving the carbonate and bicarbonate ions exists in natural waters.
\[ \text{HCO}_3^- (aq) \rightleftharpoons \text{H}^+ (aq) + \text{CO}_3^{2-} (aq) \]
Assuming that the reactions in both directions are elementary processes, do the following:
(a) Write rate expressions for the forward and reverse reactions.
- Forward rate = \( k_1 \)
- Reverse rate = \( k_{-1} \)
(b) Write an expression for the equilibrium constant based on the rates of the forward and reverse reactions.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F862d597a-ccd1-4202-ba0c-cb7527992470%2F6151e593-8443-4b55-9d2b-285bcd0799c2%2Fkbl3u09.jpeg&w=3840&q=75)
Transcribed Image Text:**Problem Solving Chapter 12**
Show all your work to receive full credit.
1. An equilibrium involving the carbonate and bicarbonate ions exists in natural waters.
\[ \text{HCO}_3^- (aq) \rightleftharpoons \text{H}^+ (aq) + \text{CO}_3^{2-} (aq) \]
Assuming that the reactions in both directions are elementary processes, do the following:
(a) Write rate expressions for the forward and reverse reactions.
- Forward rate = \( k_1 \)
- Reverse rate = \( k_{-1} \)
(b) Write an expression for the equilibrium constant based on the rates of the forward and reverse reactions.
![**Problem Solving Chapter 12**
**Instructions:**
Show all your work to receive full credit.
**1. An equilibrium involving the carbonate and bicarbonate ions exists in natural waters.**
\[ \text{HCO}_3^{- (aq)} \rightleftharpoons \text{H}^+_{(aq)} + \text{CO}_3^{2- (aq)} \]
Assuming that the reactions in both directions are elementary processes, do the following:
(a) Write rate expressions for the forward and reverse reactions.
- **Forward rate = k+1**: [Space for student work]
- **Reverse rate = k−1**: [Space for student work]
(b) Write an expression for the equilibrium constant based on the rates of the forward and reverse reactions.
- [Space for student work]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F862d597a-ccd1-4202-ba0c-cb7527992470%2F6151e593-8443-4b55-9d2b-285bcd0799c2%2Fh952hvq.jpeg&w=3840&q=75)
Transcribed Image Text:**Problem Solving Chapter 12**
**Instructions:**
Show all your work to receive full credit.
**1. An equilibrium involving the carbonate and bicarbonate ions exists in natural waters.**
\[ \text{HCO}_3^{- (aq)} \rightleftharpoons \text{H}^+_{(aq)} + \text{CO}_3^{2- (aq)} \]
Assuming that the reactions in both directions are elementary processes, do the following:
(a) Write rate expressions for the forward and reverse reactions.
- **Forward rate = k+1**: [Space for student work]
- **Reverse rate = k−1**: [Space for student work]
(b) Write an expression for the equilibrium constant based on the rates of the forward and reverse reactions.
- [Space for student work]
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