plus) [References] Isopropyl alcohol is the main ingredient in rubbing alcohol. It can decompose into acetone (the main ingredient in nail polish remover) and hydrogen gas according to the following reaction: C3H,OH(g) = C2H,CO(g)+ H2(g) At 180°C, the equilibrium constant for the decomposition is 0.45. If 43 mL (d = 0.785 g/mL) of isopropyl alcohol is placed in a 2.0 L vessel and heated to 180°C, what percentage remains undissociated at equilibrium?
plus) [References] Isopropyl alcohol is the main ingredient in rubbing alcohol. It can decompose into acetone (the main ingredient in nail polish remover) and hydrogen gas according to the following reaction: C3H,OH(g) = C2H,CO(g)+ H2(g) At 180°C, the equilibrium constant for the decomposition is 0.45. If 43 mL (d = 0.785 g/mL) of isopropyl alcohol is placed in a 2.0 L vessel and heated to 180°C, what percentage remains undissociated at equilibrium?
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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![**Chemical Decomposition of Isopropyl Alcohol**
**Introduction**
Isopropyl alcohol is the main ingredient in rubbing alcohol. It can decompose into acetone (the main ingredient in nail polish remover) and hydrogen gas according to the following reaction:
\[ \text{C}_3\text{H}_7\text{OH}(g) \rightarrow \text{C}_2\text{H}_6\text{CO}(g) + \text{H}_2(g) \]
**Problem Statement**
At 180°C, the equilibrium constant for the decomposition is 0.45. If 43 mL (density = 0.785 g/mL) of isopropyl alcohol is placed in a 2.0 L vessel and heated to 180°C, what percentage remains undissociated at equilibrium?
**Solution Approach**
To solve this problem, you'll need to follow these steps:
1. **Determine the initial moles of isopropyl alcohol:**
- Calculate the mass of isopropyl alcohol using its volume and density.
- Use the molecular weight of isopropyl alcohol to convert mass to moles.
2. **Set up the ICE (Initial, Change, Equilibrium) table:**
- Write initial concentrations.
- Express changes in concentration in terms of a variable.
- Write equilibrium concentrations in terms of the initial concentrations and the variable.
3. **Apply the equilibrium constant expression:**
- Substitute the equilibrium concentrations into the expression for the equilibrium constant and solve for the variable.
4. **Calculate the percentage of isopropyl alcohol that remains undissociated:**
- Use the obtained values to determine the undissociated part and convert it to a percentage.
This detailed approach ensures that you correctly determine how much of the isopropyl alcohol remains undissociated at the given conditions.
**Interactive Component**
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**Note:** This problem tests the understanding of chemical equilibrium concepts and the ability to apply them to a practical scenario.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fdba2aaf3-9d4f-48e5-a260-55d7aa0dddc9%2Fce8d3693-01f7-4154-b96c-78974f3fa3aa%2F7o2szub_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Chemical Decomposition of Isopropyl Alcohol**
**Introduction**
Isopropyl alcohol is the main ingredient in rubbing alcohol. It can decompose into acetone (the main ingredient in nail polish remover) and hydrogen gas according to the following reaction:
\[ \text{C}_3\text{H}_7\text{OH}(g) \rightarrow \text{C}_2\text{H}_6\text{CO}(g) + \text{H}_2(g) \]
**Problem Statement**
At 180°C, the equilibrium constant for the decomposition is 0.45. If 43 mL (density = 0.785 g/mL) of isopropyl alcohol is placed in a 2.0 L vessel and heated to 180°C, what percentage remains undissociated at equilibrium?
**Solution Approach**
To solve this problem, you'll need to follow these steps:
1. **Determine the initial moles of isopropyl alcohol:**
- Calculate the mass of isopropyl alcohol using its volume and density.
- Use the molecular weight of isopropyl alcohol to convert mass to moles.
2. **Set up the ICE (Initial, Change, Equilibrium) table:**
- Write initial concentrations.
- Express changes in concentration in terms of a variable.
- Write equilibrium concentrations in terms of the initial concentrations and the variable.
3. **Apply the equilibrium constant expression:**
- Substitute the equilibrium concentrations into the expression for the equilibrium constant and solve for the variable.
4. **Calculate the percentage of isopropyl alcohol that remains undissociated:**
- Use the obtained values to determine the undissociated part and convert it to a percentage.
This detailed approach ensures that you correctly determine how much of the isopropyl alcohol remains undissociated at the given conditions.
**Interactive Component**
- **Submit Answer:** Click this button to submit your calculated answer.
- **Try Another Version:** Click this button if you want to attempt another version of the problem.
- **Attempts Remaining:** This count shows how many attempts you have left to answer the question.
**Note:** This problem tests the understanding of chemical equilibrium concepts and the ability to apply them to a practical scenario.
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