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: McGraw-Hill Education
expand_more
expand_more
format_list_bulleted
Related questions
Question
![**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.](https://content.bartleby.com/qna-images/question/43ecea6c-19da-4f1a-84b7-58dbdadda41b/c5fb84fd-433d-4cb0-b135-6d2782435195/5reagok_processed.jpeg)
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.
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
Step by stepSolved in 6 steps
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemical-engineering and related others by exploring similar questions and additional content below.Similar questions
- Complete the property table for water below. Use only the Thermodynamic Property Table for Water referring to the Smith, Van Ness and Abbot Thermodynamics textbook. P [kPa] V [m³/kg] H[ kJ/kg] T[°C] Phase Description X 500 Saturated liquid 171 2044.5 300 0.8 Note that x refers to the "quality" or the mass fraction of the water in vapor phase. If the system is composed of pure liquid water, x = 0. If the system is composed of pure gaseous steam, x = 1. The volume of a liquid/vapor system can be determined using the following equation. V = Vj + x(Vg-Vj) V - volume of saturated liquid water Va - volume of saturated gaseous steam Similar calculation can be done for other properties such as internal energy, entropy, and enthalpy. H = HỊ + x(Hg-H) Under phase description, indicate whether the system is composed of saturated liquid, saturated vapor, superheated vapor, or liquid-vapor mixture. Also note that when pressure is given, it is more advisable to use the Superheated Steam Table than…arrow_forward(a)Using the compressibility chart, determine the compression factor (Z). Express your final answers in 3 significant figures (b)What would be the corresponding state of carbon dioxide? (Pc = 72.9 atm, Tc = 304.2 K) T (K) 200 P (atm) Tс (К) Pc (atm) Gas Argon 23.0 150.7 48.0 1.1 1.0 T- 2.00 0.9 I=1.50 0.8 Tx =1.30 0.7 to 0.6 T=1.20 0.5 T-1.10 0.4 Legend: X Methane O Ethylene A Ethane O Propane O n-Butane Iso-pentane • n-Heptane A Nitrogen T =1.00 0.3 Carbon dioxide Water 0.2 Average curve based on data on hydrocarbons 0.1 0.5 1.0 1.5 2.0 2.5 3.0 3.5 4.0 4.5 5.0 5.5 6.0 6.5 7.0 Reduced pressure P x of xarrow_forwardPHYSICAL CHEMISTRY:Calculate the pressure exerted by 1.0 mol C2H6 at 1000 K in 100 cm3 using (a) the ideal gas equation and (b) the van der Waals equation. The van der Waals constant for C2H6 are: a = 5.562 bar dm6 mol-2 ; b = 0.06380 dm3 mol-1 answer:[831; 1.72 x 10-3]arrow_forward
- (a) The ideal gas equation of state is a fairly simple expression of the relationship between the physical properties of a gas. In Module 4, we will consider some other equations of states, one of which is the van der Waals equation of state, (? + a n2/ v2) (V-nb)=nRT where a and b are constant coefficients for a given substance, and P, V, T, and n have their usual meaning. Find the partial derivative (P/T)v for this equation of state . b) Mathematically, it is known that for three variables that are related to one another (as P, Vm, and Tare here) by a function (or equation of state), one can show (??/??)z (??/??)x (??/??)y =−1 (note the cyclic variation of the three variables).Using this relationship, and the definitions of kT(coefficient of isothermal compressibility) and a (coefficient of isobaric thermal expansibility), find a simple equation relating the van der Waals parameter, b, to Vm, a, and kT. (For a discussion of this sort of…arrow_forwardIn a vessel at 200 kN/m² and 310 K, the relative humidity of water vapor in air is 52 %. The partial pressure of water vapor when air is saturated with vapor at 310 K is 6.3 kN/m?. Calculate the moisture content of the air (humidity). H = 0.6207 × Hmarrow_forwardThe following equation of state is found to describes the behavior of a particular gas with reasonable accuracy. Z = 1 + (a - b/T)P/RT where a=15x10-6 m3/mol and b= 0.06 (m3.K)/mol. Show that the residual enthalpy and residual entropy take the form: (H^r)/RT =(A-2B) and (S^r)/R = -B where A =(aP)/RT and B = (bP)/(RT^2)arrow_forward
- Partial derivatives. Use Helmholtz a P =T² (1) %3D av ƏT T V and the ideal gas equation of state to show that the internal energy, U, of an ideal gas does not depend on the volume, V.arrow_forwardmolar mass of ethanol: 46.094w = 0.645Tc = 513.9 KVc = 167cm^3/molTn = 351.4 K a.) Calculate the molar volume V (in cm3/mol) and compressibility factor Z of saturated liquid ethanol at T = 368 K.b.) Calculate the molar volume V (in cm3/mol) and compressibility factor Z of saturated vapor ethanol at T = 368 K.c.) Calculate the molar volume and compressibility factor Z of ethanol vapor at T = 462.5 K and P = 24.6 bar.arrow_forwardExample2 A lecture hall of the size 9m x 5m x 5m is filled with an air-water vapour mixture of 38° C, atmospheric pressure of 1 bar and RH 70%. The mass of air will be?? (assume Ps at 38° C = 0.06624 bar): %3D If Pa and Pw are the partial pressure of dry air and water vapour respectively, then by Dalton's law: P =Pa + Pw Given: Ø = 70 %, ps = 0.06624 bar, Patm = 1 bar. T= 38° =311 K Yolume =9 my 5 %3Darrow_forward
arrow_back_ios
arrow_forward_ios
Recommended textbooks for you
- Introduction to Chemical Engineering Thermodynami...Chemical EngineeringISBN:9781259696527Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark SwihartPublisher:McGraw-Hill Education
Elementary Principles of Chemical Processes, Bind...Chemical EngineeringISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY
Elements of Chemical Reaction Engineering (5th Ed...Chemical EngineeringISBN:9780133887518Author:H. Scott FoglerPublisher:Prentice Hall 
Industrial Plastics: Theory and ApplicationsChemical EngineeringISBN:9781285061238Author:Lokensgard, ErikPublisher:Delmar Cengage Learning
Unit Operations of Chemical EngineeringChemical EngineeringISBN:9780072848236Author:Warren McCabe, Julian C. Smith, Peter HarriottPublisher:McGraw-Hill Companies, The
Introduction to Chemical Engineering Thermodynami...
Chemical Engineering
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:McGraw-Hill Education
Elementary Principles of Chemical Processes, Bind...
Chemical Engineering
ISBN:9781118431221
Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:WILEY
Elements of Chemical Reaction Engineering (5th Ed...
Chemical Engineering
ISBN:9780133887518
Author:H. Scott Fogler
Publisher:Prentice Hall
Industrial Plastics: Theory and Applications
Chemical Engineering
ISBN:9781285061238
Author:Lokensgard, Erik
Publisher:Delmar Cengage Learning
Unit Operations of Chemical Engineering
Chemical Engineering
ISBN:9780072848236
Author:Warren McCabe, Julian C. Smith, Peter Harriott
Publisher:McGraw-Hill Companies, The