Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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![**Understanding the Equilibrium Constant Expression**
The image presents a task to write the equilibrium constant expression, \( K \), for the given chemical reaction occurring in a dilute aqueous solution.
**Given Reaction:**
\[ \text{HCN (aq) + OH}^- \text{ (aq)} \rightleftharpoons \text{CN}^- \text{ (aq) + H}_2\text{O (l)} \]
**Steps to Write the Equilibrium Constant \( K \):**
1. **Identify the Reactants and Products:**
- Reactants: HCN (aq) and \( \text{OH}^- \) (aq)
- Products: \( \text{CN}^- \) (aq) and \( \text{H}_2\text{O} \) (l)
2. **Expression of the Equilibrium Constant \( K \):**
- The equilibrium constant expression for a reaction is given by the ratio of the product of the concentrations of the products to the product of the concentrations of the reactants, each raised to the power of their respective coefficients in the balanced equation.
3. **Exclude Pure Liquids:**
- Note that \( \text{H}_2\text{O (l)} \) is a pure liquid and its concentration is not included in the equilibrium expression.
4. **Write the Expression:**
\[
K = \frac{[\text{CN}^- \text{ (aq)}]}{[\text{HCN (aq)}][\text{OH}^- \text{ (aq)}]}
\]
In the provided image, the steps to formulate this equilibrium constant \( K \) are visually guided by two rectangular input boxes to fill in the chemical species and a line representing the division in the ratio:
- The top box of the ratio would contain the concentration term for \( \text{CN}^- \) (aq).
- The bottom box of the ratio would contain the product of the concentration terms for HCN (aq) and \( \text{OH}^- \) (aq).
This presentation ensures that learners clearly understand the components and structure of the equilibrium constant expression for the given chemical reaction.](https://content.bartleby.com/qna-images/question/a527ffdc-16df-4a1f-9953-96956a75d05e/a3dec069-a5e1-493b-af77-a79e56245297/i2x3318.png)
Transcribed Image Text:**Understanding the Equilibrium Constant Expression**
The image presents a task to write the equilibrium constant expression, \( K \), for the given chemical reaction occurring in a dilute aqueous solution.
**Given Reaction:**
\[ \text{HCN (aq) + OH}^- \text{ (aq)} \rightleftharpoons \text{CN}^- \text{ (aq) + H}_2\text{O (l)} \]
**Steps to Write the Equilibrium Constant \( K \):**
1. **Identify the Reactants and Products:**
- Reactants: HCN (aq) and \( \text{OH}^- \) (aq)
- Products: \( \text{CN}^- \) (aq) and \( \text{H}_2\text{O} \) (l)
2. **Expression of the Equilibrium Constant \( K \):**
- The equilibrium constant expression for a reaction is given by the ratio of the product of the concentrations of the products to the product of the concentrations of the reactants, each raised to the power of their respective coefficients in the balanced equation.
3. **Exclude Pure Liquids:**
- Note that \( \text{H}_2\text{O (l)} \) is a pure liquid and its concentration is not included in the equilibrium expression.
4. **Write the Expression:**
\[
K = \frac{[\text{CN}^- \text{ (aq)}]}{[\text{HCN (aq)}][\text{OH}^- \text{ (aq)}]}
\]
In the provided image, the steps to formulate this equilibrium constant \( K \) are visually guided by two rectangular input boxes to fill in the chemical species and a line representing the division in the ratio:
- The top box of the ratio would contain the concentration term for \( \text{CN}^- \) (aq).
- The bottom box of the ratio would contain the product of the concentration terms for HCN (aq) and \( \text{OH}^- \) (aq).
This presentation ensures that learners clearly understand the components and structure of the equilibrium constant expression for the given chemical reaction.
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