The U.S. Food and Drug Administration lists dichloromethane (CH₂Cl₂) and carbon tetrachloride (CCl4) among the many chlorinated organic compounds that are carcinogenic. Consider a solution of 1.50 mol CH₂Cl2 and 1.00 mol of CCl4 at 23.5°C where the vapour pressure of pure dichloromethane and carbon tetrachloride are 0.46 atm and 0.16 atm respectively. a) Calculate the mole fraction of each component in the solution. Mole fraction of CH₂Cl2 Mole fraction of CCl4 b) What is the partial vapour pressure of CH₂Cl2 above the mixture? Partial vapour pressure of CH₂Cl₂ above mixture c) What is the partial vapour pressure of CCl4 above the mixture? Partial vapour pressure of CCl4 above mixture
The U.S. Food and Drug Administration lists dichloromethane (CH₂Cl₂) and carbon tetrachloride (CCl4) among the many chlorinated organic compounds that are carcinogenic. Consider a solution of 1.50 mol CH₂Cl2 and 1.00 mol of CCl4 at 23.5°C where the vapour pressure of pure dichloromethane and carbon tetrachloride are 0.46 atm and 0.16 atm respectively. a) Calculate the mole fraction of each component in the solution. Mole fraction of CH₂Cl2 Mole fraction of CCl4 b) What is the partial vapour pressure of CH₂Cl2 above the mixture? Partial vapour pressure of CH₂Cl₂ above mixture c) What is the partial vapour pressure of CCl4 above the mixture? Partial vapour pressure of CCl4 above mixture
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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![**Exercise: Vapor Pressure and Mole Fractions**
The U.S. Food and Drug Administration lists dichloromethane (CH\(_2\)Cl\(_2\)) and carbon tetrachloride (CCl\(_4\)) among the many chlorinated organic compounds that are carcinogenic. Consider a solution of 1.50 mol CH\(_2\)Cl\(_2\) and 1.00 mol of CCl\(_4\) at 23.5°C where the vapor pressure of pure dichloromethane and carbon tetrachloride are 0.46 atm and 0.16 atm respectively.
**a) Calculate the mole fraction of each component in the solution.**
- Mole fraction of CH\(_2\)Cl\(_2\): [Input Field]
- Mole fraction of CCl\(_4\): [Input Field]
**b) What is the partial vapor pressure of CH\(_2\)Cl\(_2\) above the mixture?**
- Partial vapor pressure of CH\(_2\)Cl\(_2\) above mixture: [Input Field]
**c) What is the partial vapor pressure of CCl\(_4\) above the mixture?**
- Partial vapor pressure of CCl\(_4\) above mixture: [Input Field]
**Guide for Solving:**
1. **Calculate Mole Fractions:**
The mole fraction (\(X_i\)) of a component \(i\) in a solution is calculated using:
\[
X_i = \frac{\text{moles of component } i}{\text{total moles of all components}}
\]
For CH\(_2\)Cl\(_2\):
\[
X_{\text{CH}_2\text{Cl}_2} = \frac{1.50\ \text{mol}}{1.50\ \text{mol} + 1.00\ \text{mol}} = \frac{1.50}{2.50}
\]
For CCl\(_4\):
\[
X_{\text{CCl}_4} = \frac{1.00\ \text{mol}}{1.50\ \text{mol} + 1.00\ \text{mol}} = \frac{1.00}{2.50}
\](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F7f1e4f7e-3ee3-4328-9071-c5dd7af83341%2F0b7239e5-f0d6-44f0-abc3-54467efe11c4%2Ft534gj_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Exercise: Vapor Pressure and Mole Fractions**
The U.S. Food and Drug Administration lists dichloromethane (CH\(_2\)Cl\(_2\)) and carbon tetrachloride (CCl\(_4\)) among the many chlorinated organic compounds that are carcinogenic. Consider a solution of 1.50 mol CH\(_2\)Cl\(_2\) and 1.00 mol of CCl\(_4\) at 23.5°C where the vapor pressure of pure dichloromethane and carbon tetrachloride are 0.46 atm and 0.16 atm respectively.
**a) Calculate the mole fraction of each component in the solution.**
- Mole fraction of CH\(_2\)Cl\(_2\): [Input Field]
- Mole fraction of CCl\(_4\): [Input Field]
**b) What is the partial vapor pressure of CH\(_2\)Cl\(_2\) above the mixture?**
- Partial vapor pressure of CH\(_2\)Cl\(_2\) above mixture: [Input Field]
**c) What is the partial vapor pressure of CCl\(_4\) above the mixture?**
- Partial vapor pressure of CCl\(_4\) above mixture: [Input Field]
**Guide for Solving:**
1. **Calculate Mole Fractions:**
The mole fraction (\(X_i\)) of a component \(i\) in a solution is calculated using:
\[
X_i = \frac{\text{moles of component } i}{\text{total moles of all components}}
\]
For CH\(_2\)Cl\(_2\):
\[
X_{\text{CH}_2\text{Cl}_2} = \frac{1.50\ \text{mol}}{1.50\ \text{mol} + 1.00\ \text{mol}} = \frac{1.50}{2.50}
\]
For CCl\(_4\):
\[
X_{\text{CCl}_4} = \frac{1.00\ \text{mol}}{1.50\ \text{mol} + 1.00\ \text{mol}} = \frac{1.00}{2.50}
\
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