The vapor pressure of ethanol is 54.68 mm Hg at 25 °C. A nonvolatile, nonelectrolyte that dissolves in ethanol is estrogen. Calculate the vapor pressure of the solution at 25 °C when 12.62 grams of estrogen, C18H2402 (272.4 g/mol), are dissolved in 277.8 grams of ethanol.
The vapor pressure of ethanol is 54.68 mm Hg at 25 °C. A nonvolatile, nonelectrolyte that dissolves in ethanol is estrogen. Calculate the vapor pressure of the solution at 25 °C when 12.62 grams of estrogen, C18H2402 (272.4 g/mol), are dissolved in 277.8 grams of ethanol.
Chemistry & Chemical Reactivity
9th Edition
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter13: Solutions And Their Behavior
Section: Chapter Questions
Problem 75GQ: If a volatile solute is added to a volatile solvent, both substances contribute to the vapor...
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![### Problem Statement
**Objective: Calculating Vapor Pressure of a Solution**
The vapor pressure of **ethanol** is **54.68 mm Hg** at **25 °C**. A nonvolatile, nonelectrolyte that dissolves in ethanol is **estrogen**.
**Task:**
Calculate the vapor pressure of the solution at **25 °C** when **12.62 grams of estrogen** (**C₁₈H₂₄O₂**, molar mass = **272.4 g/mol**), are dissolved in **277.8 grams of ethanol.**
**Data:**
- **ethanol** = **CH₃CH₂OH**
- Molar mass of ethanol = **46.07 g/mol**
- Vapor Pressure (VP) of pure ethanol at 25 °C = **54.68 mm Hg**
**Required Calculation:**
\[ \text{VP(solution)} = \_\_\_\_ \text{ mm Hg} \]
**Answer Entry:**
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### Explanation for Students
To solve this problem, you need to apply the concept of vapor pressure lowering, which is a colligative property. Use the formula that involves the mole fraction of the solvent and the vapor pressure of the pure solvent.
\[
P_{solution} = P_{solvent} \cdot X_{solvent}
\]
Where:
- \( P_{solution} \) is the vapor pressure of the solution
- \( P_{solvent} \) is the vapor pressure of the pure solvent (ethanol here)
- \( X_{solvent} \) is the mole fraction of the solvent (ethanol) in the solution
Steps:
1. Calculate the moles of ethanol and estrogen.
2. Determine the mole fraction of ethanol in the solution.
3. Apply the formula to find the vapor pressure of the solution.
Remember:
- Moles of a substance = Mass / Molar Mass
- Mole Fraction (X) = Moles of component / Total moles of all components in solution](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F60358686-21d1-41ff-a93a-9ba59c7b6516%2F4d054598-5949-4d04-ad69-fe094ecf4b7a%2Fptq0x1c.jpeg&w=3840&q=75)
Transcribed Image Text:### Problem Statement
**Objective: Calculating Vapor Pressure of a Solution**
The vapor pressure of **ethanol** is **54.68 mm Hg** at **25 °C**. A nonvolatile, nonelectrolyte that dissolves in ethanol is **estrogen**.
**Task:**
Calculate the vapor pressure of the solution at **25 °C** when **12.62 grams of estrogen** (**C₁₈H₂₄O₂**, molar mass = **272.4 g/mol**), are dissolved in **277.8 grams of ethanol.**
**Data:**
- **ethanol** = **CH₃CH₂OH**
- Molar mass of ethanol = **46.07 g/mol**
- Vapor Pressure (VP) of pure ethanol at 25 °C = **54.68 mm Hg**
**Required Calculation:**
\[ \text{VP(solution)} = \_\_\_\_ \text{ mm Hg} \]
**Answer Entry:**
- Text box for the answer
- **Submit Answer** button
- **Try Another Version** button
- Notification for remaining attempts (e.g., "10 item attempts remaining")
**Navigation Options:**
- **Previous** button
- **Next** button
### Explanation for Students
To solve this problem, you need to apply the concept of vapor pressure lowering, which is a colligative property. Use the formula that involves the mole fraction of the solvent and the vapor pressure of the pure solvent.
\[
P_{solution} = P_{solvent} \cdot X_{solvent}
\]
Where:
- \( P_{solution} \) is the vapor pressure of the solution
- \( P_{solvent} \) is the vapor pressure of the pure solvent (ethanol here)
- \( X_{solvent} \) is the mole fraction of the solvent (ethanol) in the solution
Steps:
1. Calculate the moles of ethanol and estrogen.
2. Determine the mole fraction of ethanol in the solution.
3. Apply the formula to find the vapor pressure of the solution.
Remember:
- Moles of a substance = Mass / Molar Mass
- Mole Fraction (X) = Moles of component / Total moles of all components in solution
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