Questions and Answers of Fundamentals Of Chemical Engineering Thermodynamics

Complete the following for liquid water at T = 100°C.A. Plot fL vs. P, using the Peng-Robinson equation of state to calculate all values of fL.B. Plot fL vs. P, using the Poynting method to
For each of the following compounds, give your best estimate of the vapor pressure at T = 400 K, and your best estimate of the fugacity in the liquid phase at T = 400 K and P = 100 bar.A. BenzeneB.
A compound has a critical point of T = 800 K and P = 45 bar, and an acentric factor of ω = 0.3. Estimate of the vapor pressure at each of the temperatures 300 K, 500 K, and 700 K, using the
You are designing a process that involves mixtures of the compounds n-butane, n-hexane, 1,3-butadiene, and benzene. You are considering whether distillation will be an effective means of separating
You are designing a fermentation process that produces mixtures of water, acetone, ethanol, and 1-butanol. You are considering whether distillation will be an effective means of separating these
Using the data for the benzene (1) + 2-propanol (2) system in Table 9-3, fit the experimental data to an appropriate polynomial equation whose independent variable is the mole fraction of ethanol.
What is the entropy change when you mix 1 mole of 1-propanol with 4 moles of ethanol at 25°C and 1 atm? Assume an ideal solution.
A two-component, two-phase mixture has how many degrees of freedom, according to Gibbs phase rule?
Using the NIST Webbook, estimate the following properties of an equimolar n-pentane + n-hexane mixture at 25°C and 1 atm, assuming an ideal solution: molar enthalpy, molar internal energy, molar
The density of an equal-mass water + ethanol mixture is 0.913 g/cc at 20°C. If the density of water is 0.998 g/cm3 and ethanol is 0.789 g/cm3 with both at 20°C, does this equal-mass mixture possess
The NIST WebBook provides very good estimates of thermodynamic properties for dozens of com pounds at a variety of states (http://webbook.nist. gov/chemistry/fluid/). Using the NIST Webbook, find the
You are in a mentoring program where you help your former high school by answering questions from students taking A.P. Chemistry. A student emails you the following question: “I don’t understand
Experimental data is available that shows the excess molar volume of acetone with three different nor mal alkanes at 298.15 K: n-hexane, n-heptane, and n-octane. Each of the three mixtures shows
Use the Peng-Robinson EOS to estimate each of the following properties of propylene.A. The vapor pressure at T = 25°C.B. The fugacity at the critical point.C. The fugacity of saturated liquid at T =
Consider two atoms: one red and the other blue. There are five locations to place those two atoms. How many microstates exist for this system?
You mix two pure components together (A and B) at the same temperature and pressure, and the mixing process is exothermic. A. If you desire to do the mixing in an adiabatic manner, will the
Consider the following term: (a(nA)) Ā, = a(n.) vrnji Would you call A, the partial molar Helmholtz free energy? Why or why not?
You are a chemical engineer working at Regional Chemical Company. The upper management has done some preliminary cost estimates and is looking to manufacture mixtures of chloroform and methanol.
The molar enthalpy of a mixture of hydrogen fluoride (1) and water (2) at 20°C is given as (Tyner, 1949) H = -1850 - 28240x, +26800x² where II[=] J/mol Calculate the partial molar enthalpy of
In a flow process, you mix 200 g/s of benzene at 308.15 K with 300 g/s of 2-propanol at 298.15 K. Using Figure 9-3, answer the following; A. What is the concentration of the resulting mixture? B.
The molar volume for a mixture of methanol (1) + water (2) at 298.15 K and 1 bar is given asD. Let’s assume you have an equimolar mixture of water and methanol. What will be the molar vol ume of
Consider the following three liquid mixtures. A. Water + n-propane B. n-hexane + benzene C. Ortho-xylene + para-xyleneWhich mixtures, if any, do you expect to behave as an ideal solution and why?
Using the information from Table 9-3, plot the partial molar enthalpies of both components at both temperatures on the same curve as a function of composition. You may have already completed some of
Using tabulated experimental data from the literature for either the excess molar volume or excess molar enthalpy of a system of your choice, provide the following information. A. A plot of the
At 80°F, we mix 10 lbm of sulfuric acid with 20 lbm of water. What is the resulting heat of mixing for this process? Is the heat liberated or absorbed? Use Figure P9-22. H (Btu)/(lb)
A mass of 500 lbm of 40 wt% sulfuric acid solution at 140°F is diluted with 200 lbm of pure water at 100°F. What is the concentration of the resulting solution? What is the heat effect (liberated
Estimate the partial molar enthalpy of sulfuric acid at 140°F at the following two compositions using Figure P9-22. A. 30% by wt sulfuric acid B. 80% by wt sulfuric acid H (Btu)/(lb)
Calculate the van Laar parameters, L12 and L21 , for the benzene (1) + toluene (2) system at 25°C through use of the van der Waals equation of state, What would be the value for the activity
Calculate the van Laar parameters using the Scatchard-Hildebrand approach, M12 and M21 , for the benzene (1) + toluene (2) system at 25°C. What would be the value for the activity coefficients of an
Explain why the integral test for thermodynamic consistency is only a necessary condition, while the direct test is a sufficient condition.
Consider the following experimental data in Table E11-11 for the ethanol (1) + 2, 2, 4-tri methyl pentane (2) system at 333.15.Considering the values of the activity coefficients, you know that this
An experiment on the vapor-liquid equilibrium for the methanol (1) + dimethyl carbonate (2) system at 337.35 K provides the following information (S. Yunhai et al., 2005):x1 50.0, y1 50.0 and P
Resolve Example Problem 11.1, but now include the nitrogen gas into the system. Note the Henry’s Law constants for nitrogen in water in Table P11-15: TABLE E11-11 Vapor-liquid equilibrium data
Which system provided here, if any, would be best modeled by an ideal solution? If any of the solutions are non-ideal, discuss whether the Scatchard Hildebrand approach would be appropriate to model
A binary liquid containing mostly component 2 is in equilibrium with a vapor phase containing both components 1 and 2. The pressure of this two-phase system is 1 bar; the temperature is 25°C.
Provide an estimate of the composition of N2 dissolved in water at 298 K. Assume A = 6.52 for the 1-parameter Margules equation for this system and the partial pressure of the Nitrogen is 44.5 atm at
A liquid mixture of 20% by mole benzene and the rest 2-propanol is in equilibrium with its vapor at 69°C. Estimate the equilibrium pressure and the composition of the vapor phase. Assume the 1-
You are interested in finding the pressure at which the first bubble of vapor will form from a liquid mixture of methanol (1) and 2-methyl 1-propanol (2) (49% by mole methanol) at 50°C. The Margules
For a chloroform (1) + ethanol (2) system at 55°C, a Margules equation has been written as GE/RT = (0.5579x1 + 1.5254x2) x1 x2 (Gmehling and Onken, 1977). Calculate the pressure and vapor-phase
The azeotrope of a binary mixture, being an important point on a mixture phase diagram, is often used for parameter estimation. To that end, use the azeotropic information for the acetone (1) +
Consider the experimental data in Table P11 21 for the ethyl acetate (1) + cyclohexane (2) system at 293.15 K. Please fit this system to the 2-parameter Margules equation and plot the Pxy curve for
In the sizing of separation equipment, you need to know the vapor–liquid equilibrium for the benzene (1) + acetonitrile (2) system. You have data for this system at 293.15 K, but not at your
You are interested in finding the pressure at which the first bubble of vapor will form from a liquid mixture of ethanol (1) and benzene (2) (49% by mole ethanol) at 313 K. The Margules parameters
You are interested in evaluating how well you can predict the phase-behavior of a system using an excess molar Gibbs free energy model. Here, use the van Laar predictions (from the VDW-defined
Compare the van Laar predictions if using VDW-defined parameters relative to those from Scatchard-Hildebrand in order to calculate the Pxy diagram of the benzene (1) + m-xylene (2) system at 310.15 K
In a process analysis application, you are working with the di-n-propyl ether (1) and 2-propanol (2) system at 25°C. You think you have an error in the spread sheet you have been working with, but
Your company needs to evaluate the separation of an equimolar mixture of ethanol (1) + n-hexane (2) at 318.15 K. While looking at some company notebooks, you find data for this system at 318.15 K as
In a process you need to evaluate the flash separation of an equimolar mixture of 1,3-dioxolane (1) + n-heptane (2) at 70°C. However, you can only find experimental data at 40°C. From your
You desire to flash 20 moles/min of a liquid mixture containing 20% by mole chloroform (1) and 80% by mole ethanol (2) at 332.4 K in a flash distillation unit operating at 70 kPa. You do not know a
You desire to flash separate 10 mol/s of an equimolar liquid mixture of 1-butene (1) + n-heptane (2) at 100 kPa and 0 C. If your f lash distillation unit operates at 50 kPa and 0 C, what is the f low
You have found a set of thermodynamic data in the literature for benzene (1) + 2-propanol (2) at 298.15 K that you need to evaluate for a particular process. However, you want to verify the quality
Consider an equimolar mixture of n-butane (1) + 1-butanol (2) at 50°C. Calculate the second-virial coefficient of the mixture using Equation 12.24.Equation 12.24. Η Η Η
Derive Equation 12.31, which is the expression for the mixture fugacity coefficient of component 1 in a binary mixture described by the virial equation.Equation 12.31. In (+₁) = P RT [B'₁₁ +
For an equimolar acetone (1) + methyl ethyl ketone (2) mixture, calculate the van der Waals and Peng-Robinson equation of state parameters at 35°C. H₂C Lov CH3 Acetone H3C- CH3 Methyl ethyl ketone
Calculate the mixture fugacity coefficient for both components of a n-butane (1) + propane (2) mixture at 50°C using the virial equation. Provide the result at five compositions:A. x1 = 0 B. x1 =
For an equimolar mixture of water (1) + chloroform (2) mixture at 200°C and 5 bar, estimate the molar volume of the mixture three ways: A. Ideal gas law B. van der Waals equation of state C.
Starting with Equation 11.124 and assuming the combining rule in Equation 11.126, derive Equation 11.127Equation 11.124.Equation 11.126.Equation 11.127. ²q²x²x+¹²q²x²³x + ²q²x³²x +
For a binary mixture you desire to produce a Txy diagram from an equation of state. List the equations needed and the unknown variables.
You are interested in the location of the azeotrope for the acetonitrile (1) + benzene (2) system at 346.85 K. However, you only have that information for this system at 318.15 K. At that state
In Example 12-2 in this chapter, you evaluated two equation of state approaches for the prediction of the phase behavior for the propane (1) + n-butane (2) system at 323.15 K. Once you completed this
In Problem 12-18 in this section, you used a gamma-phi modeling approach for the pentafluoroethane [R-125] (1) + isobutane (2) system at 30°C. There (if you solved that problem), you realized the
Use a - approach to model the vapor-liquid equilibrium of an ethyne [acetylene] (1) + 1, 1 difluoro ethane {R-152a] (2) system at 303.2 K. Treat theliquid using the 2-parameter Margules equation and
N-formylmorpholine can be used as a solvent in an extraction process for producing high-purity aromatic compounds. To that end, liquid–liquid equilibrium data has been prepared for this compound
For an ethylene glycol n-butyl ether (1) + water (2) system at 360 K with 70% by mass water, determine if the system is one stable liquid phase or two stable liquid phases at equilibrium. If the
Chopade and co-workers in 2003 reported the vapor–liquid, liquid–liquid, and vapor–liquid–liquid equilibrium for the system 2-methyl-1, 3 dioxolane (1) + water (2) system at 1 atm. They
In 1924, Gilbert Lewis and Merle Randall published Thermodynamics and the Free Energy of Chemical Substances (1st Edition, McGraw-Hill Book Co., Inc., New York). On page 225 these authors state,
Produce the SLE phase diagram for the p-xylene (1) + m-xylene system. Treat the liquid phase as an ideal solution and the solid phase as im miscible. Please plot your phase diagram using the p-xylene
Example 14-6 examined the thermal decomposition of butane forming propylene:C4 H10 ↔ C3 H6 + CH4But a competing thermal decomposition reaction forming ethylene and ethane is also possible: C4
Predict the Pxy behavior for a mixture of cyclohexane (1) + 1-butanol (2) at 383.15 K using the Peng-Robinson equation of state. Compare the predictions to the experimental data given in Table
Predict the Pxy behavior for a mixture of acetone (1) + 2-propanol (2) at 328.15 K using the Peng-Robinson equation of state. Compare the predictions to the experimental data given in Table P12-26.
The infinite dilution activity coefficients for the methanol (1) + n-heptane (2) mixture at 30°C are Ý1 = 84.20 (Wobst et al., 1992) and Ý2 = 35.10 (Gmehling et al., 1986). You know that this
When you learned about the solubility parameters (₰) from the Scatchard-Hildebrand approach in Chapter 11, it was discussed that the difference in the values of the solubility parameters between
Estimate the pressure and composition for VLLE for the diethyl ether (1) + water (2) system at 35°C. Assume the liquid can be modeled by the 2-parameter Margules equation where A12 = 4.62 and A21 =
At 108C, n-pentane (1) + water (2) shows a miscibility gap. The composition of the phases in equilibrium is as follows: x1a = 0.00107 and x2β = 0.0184, where “a” is for the water-rich phase and
Produce the SLE phase diagram for the m- chloronitrobenzene (1) + p-chloronitrobenzene (2) system at 1 atm. Treat the liquid phase as an ideal solution and the solid phase as immiscible. On each
Produce the SLE phase diagram for the p- dichlorobenzene (1) + p-dibromobenzene system at 1 atm. You will do the modeling in two ways and answer each part of the question. Some helpful data are
Determine the equilibrium constant at T = 298.15 K for each of the following reactions: A. Formation of ethanol from ethylene and water:B. Dehydrogenation of cyclohexane to form benzene: C.
You are tasked with determining a good estimate of the pressure and vapor–phase composition for a vapor–liquid–liquid equilibrium system of benzene (1) + water (2) at two temperatures: 303.15 K
A sealed container (Figure 14-1) initially contains 1.0 mole of ethane, 0.5 mole of eth ylene, and 0.5 mole of hydrogen. The vessel is maintained at a constant T = 25°C and P = 1 bar, as the
The chemical reaction:is carried out at P = 1 bar and T = 25°C. Derive an equilibrium expression for this reaction in which the only unknowns are the mole fractions of the three gases. C₂H₂(g)
The steam reforming of natural gas into syngas features the gas phase reaction: which has an equilibrium constant K1000 = 26.6 (Lu, 2010). This reaction is to be carried out in a sealed reaction
For each of the three reactions listed in Exercise 14-3, use the shortcut van’t Hoff equation to compute the equilibrium constant at T = 600 K.Exercise 14-3.Determine the equilibrium constant at T
Ethyl acetate can be formed from ethanol and acetic acid, by the liquid phase reaction A liquid phase reactor (Figure 14-6) with a constant temperature T = 298.15 K initially contains 5 moles each
For each of the following cases, construct a stoichiometric table that describes the reaction: 2SO2 (g) + O2 (g) ↔ 2SO3 (g)Your table should show expressions for the mole fraction y of each gas in
The compound chloromethane can be synthesized by the chemical reaction: This reaction progresses by a free-radical mechanism and typically requires high temperatures. The reaction is carried out in
Butadiene can be formed by dehydrogenation of n-butane: C4 H10 ↔ C4 H6 + 2H2 This reaction is carried out in the gas phase.A. Calculate the equilibrium constant of this reaction at K298.15. B.
Example 14-8 illustrated the chlorination of methane to form chloromethane: Example 14-8 also revealed that at equilibrium, the products were strongly favored. However, the substitution of chlorine
Ethylene can be formed by cracking of propane: C3 H8 ↔C2 H4 + CH4 This reaction is carried out in the gas phase. A. Calculate the equilibrium constant of this reaction at K298.15. B. 1000
The reaction 2A + 4B↔C + 3D is carried out in the liquid phase, in a closed-system reactor at T + 400 K and P + 1 bar. At these conditions, the equilibrium constant is K400 = 12.5, and the reaction
The reaction A13B↔C+2D is carried out in the gas phase, in a steady-state re actor at T = 500 K and P = 1 bar. At these conditions, the equilibrium constant is K500 = 0.2500. The reacting mixture
For the following liquid phase reaction, 1 - pentene + water ↔1 - pentanol A. Find the equilibrium constant at T = 300°C using the shortcut van ’t Hoff approach. B. Find the equilibrium
The motivational example demonstrated that the reaction: C2 H6 (g) ↔ C2 H4 (g) + H2 (g) strongly favors the reactant ethane at equilibrium—so strongly that the amount of product is barely
Ethyl acetate is synthesized from ethanol and acetic acid by the liquid phase esterification reaction shown in Figure 15-3..C2 H5 OH + CH3 COOH ↔ H2 O + CH3 COOC2 H5 Ethanol + acetic acid ↔
This problem revisits Example 15-3, part B. Re-do the problem three times, changing the amount of water to the following. A. 25 moles B. 100 moles C. 500 moles D. Use graphs or tables to compare
This problem revisits Example 15-4. Re-do the problem three times, changing the volume of the system to the following. A. 300 L B. 1000 L C. 1500 L D. Use graphs or tables to compare the results
At ambient conditions, nitrogen dioxide and dinitrogen tetraoxide form a vapor phase equilibrium mixture with each other: 2NO2 (g) ↔ N2 O4 (g)A. 10 moles of nitrogen dioxide are placed in a
This problem considers the ammonia synthesis process described in Example 15-5, part B. The fresh air and hydrogen each enter the process at T = 25°C and P = 1 bar, and need to be compressed to P
This problem re-examines Example 15-5 by considering the effect of changing the pressure.A. Re-do Example 15-5. Use P = 49 bar for all pressures throughout the system, assume all mixtures are ideal
30 mol/s of hydrogen gas and 15 mol/s of air, each compressed to 25 bar, enter a steady state reactor as shown in Figure 15-5, where the nitrogen in the air reacts with the hydrogen to form
For an ethylene glycol n-butyl ether (1) + water (2) system at 310 K with 70% by mass water, determine if the system is one stable liquid phase or two stable liquid phases at equilibrium. If the

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