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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Question
![**Title: Equilibrium Constant Expression**
**Text:**
Write the equilibrium constant expression for this reaction:
\[ 2\text{Li}^+ \, (\text{aq}) + \text{CO}_3^{2-} \, (\text{aq}) \rightleftharpoons \text{Li}_2\text{CO}_3 \, (\text{s}) \]
**Equilibrium Constant Expression (K):**
\[ K = \frac{1}{[\text{Li}^+]^2 [\text{CO}_3^{2-}]} \]
**Explanation:**
In this reaction, lithium ions (\(\text{Li}^+\)) and carbonate ions (\(\text{CO}_3^{2-}\)) in aqueous solution combine to form solid lithium carbonate (\(\text{Li}_2\text{CO}_3\)).
Since \(\text{Li}_2\text{CO}_3\) is a solid, its activity is considered to be 1 and does not appear in the equilibrium constant expression. Therefore, the expression for the equilibrium constant (\(K\)) involves only the concentrations of the reactants in the aqueous phase. The square brackets "[ ]" denote concentration.
In this case, the equilibrium constant expression is given as:
\[ K = \frac{1}{[\text{Li}^+]^2 [\text{CO}_3^{2-}]} \]
This indicates that the equilibrium lies heavily to the right when there is a low concentration of \(\text{Li}^+\) and \(\text{CO}_3^{2-}\), favoring the formation of the solid product.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F7c12de76-b007-4fc9-b4e9-4d53c67e07b9%2F18c88f7b-7214-43d1-9b94-ea0399a4af82%2F98exlgn_processed.png&w=3840&q=75)
Transcribed Image Text:**Title: Equilibrium Constant Expression**
**Text:**
Write the equilibrium constant expression for this reaction:
\[ 2\text{Li}^+ \, (\text{aq}) + \text{CO}_3^{2-} \, (\text{aq}) \rightleftharpoons \text{Li}_2\text{CO}_3 \, (\text{s}) \]
**Equilibrium Constant Expression (K):**
\[ K = \frac{1}{[\text{Li}^+]^2 [\text{CO}_3^{2-}]} \]
**Explanation:**
In this reaction, lithium ions (\(\text{Li}^+\)) and carbonate ions (\(\text{CO}_3^{2-}\)) in aqueous solution combine to form solid lithium carbonate (\(\text{Li}_2\text{CO}_3\)).
Since \(\text{Li}_2\text{CO}_3\) is a solid, its activity is considered to be 1 and does not appear in the equilibrium constant expression. Therefore, the expression for the equilibrium constant (\(K\)) involves only the concentrations of the reactants in the aqueous phase. The square brackets "[ ]" denote concentration.
In this case, the equilibrium constant expression is given as:
\[ K = \frac{1}{[\text{Li}^+]^2 [\text{CO}_3^{2-}]} \]
This indicates that the equilibrium lies heavily to the right when there is a low concentration of \(\text{Li}^+\) and \(\text{CO}_3^{2-}\), favoring the formation of the solid product.
![**Chemical Equilibrium Reaction:**
The equilibrium reaction shown is:
\[ \text{Al(OH)}_3 (s) \rightleftharpoons \text{Al}^{3+} (aq) + 3\text{OH}^{-} (aq) \]
This represents the dissociation of aluminum hydroxide in aqueous solution, producing aluminum ions and hydroxide ions.
**Equilibrium Constant Expression:**
The equilibrium constant (\( K \)) for this reaction is given by the expression:
\[ K = \frac{[\text{OH}^{-}]^3}{[\text{Al}^{3+}]} \]
Here, \([\text{OH}^{-}]\) is the concentration of hydroxide ions in the solution, raised to the third power due to its stoichiometric coefficient, and \([\text{Al}^{3+}]\) is the concentration of aluminum ions.
**Additional Interface Options:**
The image includes a toolbar with options that seem to be related to mathematical or scientific formatting, such as formatting for exponents, indices, special characters like delta (δ), and functions like logarithms and cosine. However, these are not directly interacting with the displayed chemical content.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F7c12de76-b007-4fc9-b4e9-4d53c67e07b9%2F18c88f7b-7214-43d1-9b94-ea0399a4af82%2Fig0hpf4_processed.png&w=3840&q=75)
Transcribed Image Text:**Chemical Equilibrium Reaction:**
The equilibrium reaction shown is:
\[ \text{Al(OH)}_3 (s) \rightleftharpoons \text{Al}^{3+} (aq) + 3\text{OH}^{-} (aq) \]
This represents the dissociation of aluminum hydroxide in aqueous solution, producing aluminum ions and hydroxide ions.
**Equilibrium Constant Expression:**
The equilibrium constant (\( K \)) for this reaction is given by the expression:
\[ K = \frac{[\text{OH}^{-}]^3}{[\text{Al}^{3+}]} \]
Here, \([\text{OH}^{-}]\) is the concentration of hydroxide ions in the solution, raised to the third power due to its stoichiometric coefficient, and \([\text{Al}^{3+}]\) is the concentration of aluminum ions.
**Additional Interface Options:**
The image includes a toolbar with options that seem to be related to mathematical or scientific formatting, such as formatting for exponents, indices, special characters like delta (δ), and functions like logarithms and cosine. However, these are not directly interacting with the displayed chemical content.
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