The vapor pressure of benzene is 73.03 mm Hg at 25 °C. A nonvolatile, nonelectrolyte that dissolves in benzene is cholesterol. Calculate the vapor pressure of the solution at 25 °C when 10.28 grams of cholesterol, C27H460 (386.6 g/mol), are dissolved in 268.4 grams of benzene. benzene = C,H = 78.12 g/mol. VP(solution) = mm Hg
The vapor pressure of benzene is 73.03 mm Hg at 25 °C. A nonvolatile, nonelectrolyte that dissolves in benzene is cholesterol. Calculate the vapor pressure of the solution at 25 °C when 10.28 grams of cholesterol, C27H460 (386.6 g/mol), are dissolved in 268.4 grams of benzene. benzene = C,H = 78.12 g/mol. VP(solution) = mm Hg
Chemistry
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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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![### Calculating the Vapor Pressure of a Solution
The vapor pressure of **benzene** is **73.03 mm Hg** at **25 °C**. A nonvolatile, nonelectrolyte that dissolves in benzene is **cholesterol**.
Calculate the vapor pressure of the solution at **25 °C** when **10.28 grams** of **cholesterol**, **C₇₂H₄₆O (386.6 g/mol)**, are dissolved in **268.4 grams** of **benzene**.
#### Given Data:
- **Benzene** (C₆H₆): **78.12 g/mol**
- **Vapor pressure of pure benzene**: **73.03 mm Hg**
- **Mass of cholesterol (C₂₇H₄₆O)**: **10.28 grams**
- **Molar mass of cholesterol**: **386.6 g/mol**
- **Mass of benzene**: **268.4 grams**
#### Formula to Calculate:
\[ \text{VP(solution)} = \square \text{ mm Hg} \]
To solve the problem, use the data given and the appropriate equations related to vapor pressure lowering due to a solute.
### Steps to Solve:
1. **Calculate the moles of Benzene (C₆H₆)**:
\[ \text{Moles of Benzene} = \frac{\text{mass}}{\text{molar mass}} = \frac{268.4 \, \text{g}}{78.12 \, \text{g/mol}} \]
2. **Calculate the moles of Cholesterol (C₂₇H₄₆O)**:
\[ \text{Moles of Cholesterol} = \frac{10.28 \, \text{g}}{386.6 \, \text{g/mol}} \]
3. **Calculate the mole fraction of Benzene**:
- The mole fraction of the solvent (benzene) can be determined by finding the total moles of the solution and using the formula:
\[ \text{Mole fraction of Benzene} = \frac{\text{Moles of Benzene}}{\text{Moles of Benzene} + \text{Moles of Cholesterol}} \]
4. **Calculate the Vapor Pressure of the Solution**:
- Use Raoult’s](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fedee5435-55e0-4ec8-aecd-101c845dd6aa%2F4171d695-1625-4ce5-aa29-159debc0b247%2Fheji1l_processed.png&w=3840&q=75)
Transcribed Image Text:### Calculating the Vapor Pressure of a Solution
The vapor pressure of **benzene** is **73.03 mm Hg** at **25 °C**. A nonvolatile, nonelectrolyte that dissolves in benzene is **cholesterol**.
Calculate the vapor pressure of the solution at **25 °C** when **10.28 grams** of **cholesterol**, **C₇₂H₄₆O (386.6 g/mol)**, are dissolved in **268.4 grams** of **benzene**.
#### Given Data:
- **Benzene** (C₆H₆): **78.12 g/mol**
- **Vapor pressure of pure benzene**: **73.03 mm Hg**
- **Mass of cholesterol (C₂₇H₄₆O)**: **10.28 grams**
- **Molar mass of cholesterol**: **386.6 g/mol**
- **Mass of benzene**: **268.4 grams**
#### Formula to Calculate:
\[ \text{VP(solution)} = \square \text{ mm Hg} \]
To solve the problem, use the data given and the appropriate equations related to vapor pressure lowering due to a solute.
### Steps to Solve:
1. **Calculate the moles of Benzene (C₆H₆)**:
\[ \text{Moles of Benzene} = \frac{\text{mass}}{\text{molar mass}} = \frac{268.4 \, \text{g}}{78.12 \, \text{g/mol}} \]
2. **Calculate the moles of Cholesterol (C₂₇H₄₆O)**:
\[ \text{Moles of Cholesterol} = \frac{10.28 \, \text{g}}{386.6 \, \text{g/mol}} \]
3. **Calculate the mole fraction of Benzene**:
- The mole fraction of the solvent (benzene) can be determined by finding the total moles of the solution and using the formula:
\[ \text{Mole fraction of Benzene} = \frac{\text{Moles of Benzene}}{\text{Moles of Benzene} + \text{Moles of Cholesterol}} \]
4. **Calculate the Vapor Pressure of the Solution**:
- Use Raoult’s
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