4. The vapor pressures of CCI4 (A) and C2HCI3 (B) between T= 350 and 360 K, can be determined empirically by the formulas PA In 1 bar 2790.78 = 9.2199 (T-46.75) PB* In 1 bar 2345.4 = 8.3922 (T-80.45) where T is given in K, and the vapor pressures will be in units of bars. Assuming that these two substances form an ideal solution in this temperature range, in all proportions, find the mole fraction of CCI4 (component A) in both the liquid and vapor phases at T= 355 K, and an ambient pressure of 1.0 bar.
4. The vapor pressures of CCI4 (A) and C2HCI3 (B) between T= 350 and 360 K, can be determined empirically by the formulas PA In 1 bar 2790.78 = 9.2199 (T-46.75) PB* In 1 bar 2345.4 = 8.3922 (T-80.45) where T is given in K, and the vapor pressures will be in units of bars. Assuming that these two substances form an ideal solution in this temperature range, in all proportions, find the mole fraction of CCI4 (component A) in both the liquid and vapor phases at T= 355 K, and an ambient pressure of 1.0 bar.
Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
Section: Chapter Questions
Problem 1.1P
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![**Vapor Pressure Determination for CCl₄ and C₂HCl₃**
**Problem Statement:**
The vapor pressures of carbon tetrachloride (CCl₄, denoted as component A) and trichloroethylene (C₂HCl₃, denoted as component B) between temperatures T = 350 K and 360 K can be determined empirically by the following formulas:
\[ \ln\left(\frac{P_A^*}{1 \text{ bar}}\right) = 9.2199 - \frac{2790.78}{T - 46.75} \]
\[ \ln\left(\frac{P_B^*}{1 \text{ bar}}\right) = 8.3922 - \frac{2345.4}{T - 80.45} \]
where \( T \) is the temperature in Kelvin (K), and the vapor pressures are expressed in bars.
**Task:**
Assuming CCl₄ and C₂HCl₃ form an ideal solution in this temperature range and in all proportions, find the mole fraction of CCl₄ (component A) in both the liquid and vapor phases at T = 355 K, with an ambient pressure of 1.0 bar.
**Instructions and Explanation:**
- **Empirical Equations for Vapor Pressures:**
- The equations relate the natural logarithm of the pressure ratio to temperature for each component of the mixture. For component A (CCl₄), the equation involves constants 9.2199 and 2790.78, and a temperature correction of 46.75. For component B (C₂HCl₃), the constants are 8.3922 and 2345.4, with a temperature correction of 80.45.
- **Ideal Solution Assumption:**
- An ideal solution implies that the interactions between different molecules are similar to those between like molecules, allowing the application of Raoult's Law.
- **Calculation Objectives:**
- Determine vapor pressures using the given empirical formulas.
- Calculate mole fractions in both phases considering the given temperature and total pressure.
**Note:** This calculation will help in understanding how the vapor-liquid equilibrium is influenced by temperature and composition under ideal conditions.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F43ecea6c-19da-4f1a-84b7-58dbdadda41b%2Fc5fb84fd-433d-4cb0-b135-6d2782435195%2F5reagok_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Vapor Pressure Determination for CCl₄ and C₂HCl₃**
**Problem Statement:**
The vapor pressures of carbon tetrachloride (CCl₄, denoted as component A) and trichloroethylene (C₂HCl₃, denoted as component B) between temperatures T = 350 K and 360 K can be determined empirically by the following formulas:
\[ \ln\left(\frac{P_A^*}{1 \text{ bar}}\right) = 9.2199 - \frac{2790.78}{T - 46.75} \]
\[ \ln\left(\frac{P_B^*}{1 \text{ bar}}\right) = 8.3922 - \frac{2345.4}{T - 80.45} \]
where \( T \) is the temperature in Kelvin (K), and the vapor pressures are expressed in bars.
**Task:**
Assuming CCl₄ and C₂HCl₃ form an ideal solution in this temperature range and in all proportions, find the mole fraction of CCl₄ (component A) in both the liquid and vapor phases at T = 355 K, with an ambient pressure of 1.0 bar.
**Instructions and Explanation:**
- **Empirical Equations for Vapor Pressures:**
- The equations relate the natural logarithm of the pressure ratio to temperature for each component of the mixture. For component A (CCl₄), the equation involves constants 9.2199 and 2790.78, and a temperature correction of 46.75. For component B (C₂HCl₃), the constants are 8.3922 and 2345.4, with a temperature correction of 80.45.
- **Ideal Solution Assumption:**
- An ideal solution implies that the interactions between different molecules are similar to those between like molecules, allowing the application of Raoult's Law.
- **Calculation Objectives:**
- Determine vapor pressures using the given empirical formulas.
- Calculate mole fractions in both phases considering the given temperature and total pressure.
**Note:** This calculation will help in understanding how the vapor-liquid equilibrium is influenced by temperature and composition under ideal conditions.
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