2. Toluene has a vapor pressure of 40.4 mm Hg at 4.4°C and 3166.0 mm Hg at 55.2°C. Solve for the AHvap of toluene. At what temperature will toluene have a vapor pressure of 700.0 mm Hg? goitonib
2. Toluene has a vapor pressure of 40.4 mm Hg at 4.4°C and 3166.0 mm Hg at 55.2°C. Solve for the AHvap of toluene. At what temperature will toluene have a vapor pressure of 700.0 mm Hg? goitonib
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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![### Problem Statement on Vapor Pressure of Toluene
**Problem 2:**
Toluene has a vapor pressure of 40.4 mm Hg at 4.4°C and 316.0 mm Hg at 52.2°C. Solve for the ΔHvap (enthalpy of vaporization) of toluene. At what temperature will toluene have a vapor pressure of 700.0 mm Hg?
---
**Explanation:**
This problem involves determining the enthalpy of vaporization (ΔHvap) for toluene using the Clausius-Clapeyron equation and subsequently solving for the temperature at which toluene will achieve a specified vapor pressure.
Ensure to follow the steps of using the Clausius-Clapeyron equation:
1. **Identify the given data:**
- Vapor pressure (P1) = 40.4 mm Hg at T1 = 4.4°C
- Vapor pressure (P2) = 316.0 mm Hg at T2 = 52.2°C
- Desired vapor pressure (P3) = 700.0 mm Hg
2. **Convert temperatures from Celsius to Kelvin:**
- T1 = 4.4 + 273.15 = 277.55 K
- T2 = 52.2 + 273.15 = 325.35 K
3. **Use the Clausius-Clapeyron equation:**
\[
\ln \left( \frac{P2}{P1} \right) = \frac{\Delta H_{vap}}{R} \left( \frac{1}{T1} - \frac{1}{T2} \right)
\]
- Where R is the universal gas constant (8.314 J/mol·K).
4. **Rearrange the equation to solve for ΔHvap:**
\[
\Delta H_{vap} = \frac{ \ln \left( \frac{P2}{P1} \right) \times R }{ \left( \frac{1}{T1} - \frac{1}{T2} \right) }
\]
5. **Once ΔHvap is determined, use it to find the new temperature (T3) for P3 using the Clausius-Clapeyron equation again:**
\[
\](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ff2609b9a-bccc-4ea0-ab3c-7cfd8cf7907c%2F41d27530-bb26-43aa-99db-abe9c30ef3ea%2F760z84_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Problem Statement on Vapor Pressure of Toluene
**Problem 2:**
Toluene has a vapor pressure of 40.4 mm Hg at 4.4°C and 316.0 mm Hg at 52.2°C. Solve for the ΔHvap (enthalpy of vaporization) of toluene. At what temperature will toluene have a vapor pressure of 700.0 mm Hg?
---
**Explanation:**
This problem involves determining the enthalpy of vaporization (ΔHvap) for toluene using the Clausius-Clapeyron equation and subsequently solving for the temperature at which toluene will achieve a specified vapor pressure.
Ensure to follow the steps of using the Clausius-Clapeyron equation:
1. **Identify the given data:**
- Vapor pressure (P1) = 40.4 mm Hg at T1 = 4.4°C
- Vapor pressure (P2) = 316.0 mm Hg at T2 = 52.2°C
- Desired vapor pressure (P3) = 700.0 mm Hg
2. **Convert temperatures from Celsius to Kelvin:**
- T1 = 4.4 + 273.15 = 277.55 K
- T2 = 52.2 + 273.15 = 325.35 K
3. **Use the Clausius-Clapeyron equation:**
\[
\ln \left( \frac{P2}{P1} \right) = \frac{\Delta H_{vap}}{R} \left( \frac{1}{T1} - \frac{1}{T2} \right)
\]
- Where R is the universal gas constant (8.314 J/mol·K).
4. **Rearrange the equation to solve for ΔHvap:**
\[
\Delta H_{vap} = \frac{ \ln \left( \frac{P2}{P1} \right) \times R }{ \left( \frac{1}{T1} - \frac{1}{T2} \right) }
\]
5. **Once ΔHvap is determined, use it to find the new temperature (T3) for P3 using the Clausius-Clapeyron equation again:**
\[
\
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