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Ph (s. 25°C, 1 atm) Ph (s. 42.5°C, 1 atm) Ph (1, 42.5°C, 1 atm) Ph (1, 181.4°C, 1 atm) Ph=phenol(C,H,OH) (True path) AR கர் AR₂ AR, AR₂ Ph (v. 300.0°C, 3 atm) AR Ph (v. 300.0°C, 1 atm) AR₁ Ph (v. 181.4°C, 1 atm)

Ph (s. 25°C, 1 atm) Ph (s. 42.5°C, 1 atm) Ph (1, 42.5°C, 1 atm) Ph (1, 181.4°C, 1 atm) Ph=phenol(C,H,OH) (True path) AR கர் AR₂ AR, AR₂ Ph (v. 300.0°C, 3 atm) AR Ph (v. 300.0°C, 1 atm) AR₁ Ph (v. 181.4°C, 1 atm)

Introduction to Chemical Engineering Thermodynamics
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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Calculate enthalpies 1 through 6.  For calculating enthalpies 1, 3, 5, and 6, use the method of deltaH = VdeltaP.

For calculating enthalpies 2 and 4, use the method of phase changes.  Calculate these enthalpies for the solid, liquid, and vapor states of phenol.  

X + PDF *Elementary Principles of Chemic X b My Questions | bartleby File | E:/Elementary%20Principles%20of%20Chemical%20Processes,%204th%20Edition%20(%20PDF Drive%20).pdf Draw (T) Read aloud of 695 3 its mole fraction in the mixture). A state property does not depend on how the species reached its state. Consequently, when a species passes from one state to another, both ▲Û and ▲H for the process are independent of the path taken from the first state to the second one. ←→ 425 In most of this chapten and in Chapter 9, you will learn how to calculate internal energy and enthalpy changes associated with certain processes: specifically, Changes in P at constant T and state of aggregation (Section 8.2). 2. Changes in T at constant P and state of aggregation (Section 8.3). 3. Phase changes at constant T and P-melting, solidifying, vaporizing, condensing, sublimating (Section 8.4). 4. Mixing of two liquids or dissolving of a gas or a solid in a liquid at constant T and P (Section 8.5). 5. Chemical reaction at constant T and P (Chapter 9). Q Search For example, compressing hydrogen gas from 1 atm to 300 atm at 25°C is a Type 1 process; melting ice at 0°C and then heating the liquid water to 30°C, all at 1 atm, is a Type 3 process followed by a Type 2 process; mixing sulfuric acid and water at a constant temperature of 20°C and a constant pressure of 1 atm is a Type 4 process. Once we know how to calculate AU and AH for these five types of processes, we can calculate these quantities for any process by taking advantage of the fact that Û and Ĥ are state properties. The procedure is to construct a hypothetical process path from the initial state to the final state consisting of a series of steps of the given five types. Having done this, we calculate AĤ for each of the steps, and then add the AA's for the steps to calculate AĤ for the total process. Since Ĥ is a state property, AĤ calculated for the hypothetical process path-which we constructed for convenience is the same as AĤ for the path actually followed by the process. The same procedure can be followed to calculate AU for any process. Suppose, for example, that we wish to calculate AĤ for a process in which solid phenol at 25°C and I atm is converted to phenol vapor at 300°C and 3 atm. If we had a table of enthalpies for phenol, we could simply subtract Ĥ at the initial state from Ĥ at the final state, or AĤ = Ĥ(vapor, 300°C, 3 atm) - Ĥ(solid, 25°C, 1 atm) However, we do not have such a table. Our task is then to construct a hypothetical process path from the solid at 25°C and 1 atm to the vapor at 300°C and 3 atm. To do so, we will look ahead a bit and note that Table B.1 gives enthalpy changes for the melting of phenol at 1 atm and 42.5°C (the normal melting point of phenol) and for the vaporization of phenol at 1 atm and 181.4°C (the normal boiling point of phenol). We therefore choose the following hypothetical process path: Phnhenol(C₂H-OH). {" J 63 50 ENG Sign in I ● 5:53 AM 5/8/2023 + O {0}
Transcribed Image Text:X + PDF *Elementary Principles of Chemic X b My Questions | bartleby File | E:/Elementary%20Principles%20of%20Chemical%20Processes,%204th%20Edition%20(%20PDF Drive%20).pdf Draw (T) Read aloud of 695 3 its mole fraction in the mixture). A state property does not depend on how the species reached its state. Consequently, when a species passes from one state to another, both ▲Û and ▲H for the process are independent of the path taken from the first state to the second one. ←→ 425 In most of this chapten and in Chapter 9, you will learn how to calculate internal energy and enthalpy changes associated with certain processes: specifically, Changes in P at constant T and state of aggregation (Section 8.2). 2. Changes in T at constant P and state of aggregation (Section 8.3). 3. Phase changes at constant T and P-melting, solidifying, vaporizing, condensing, sublimating (Section 8.4). 4. Mixing of two liquids or dissolving of a gas or a solid in a liquid at constant T and P (Section 8.5). 5. Chemical reaction at constant T and P (Chapter 9). Q Search For example, compressing hydrogen gas from 1 atm to 300 atm at 25°C is a Type 1 process; melting ice at 0°C and then heating the liquid water to 30°C, all at 1 atm, is a Type 3 process followed by a Type 2 process; mixing sulfuric acid and water at a constant temperature of 20°C and a constant pressure of 1 atm is a Type 4 process. Once we know how to calculate AU and AH for these five types of processes, we can calculate these quantities for any process by taking advantage of the fact that Û and Ĥ are state properties. The procedure is to construct a hypothetical process path from the initial state to the final state consisting of a series of steps of the given five types. Having done this, we calculate AĤ for each of the steps, and then add the AA's for the steps to calculate AĤ for the total process. Since Ĥ is a state property, AĤ calculated for the hypothetical process path-which we constructed for convenience is the same as AĤ for the path actually followed by the process. The same procedure can be followed to calculate AU for any process. Suppose, for example, that we wish to calculate AĤ for a process in which solid phenol at 25°C and I atm is converted to phenol vapor at 300°C and 3 atm. If we had a table of enthalpies for phenol, we could simply subtract Ĥ at the initial state from Ĥ at the final state, or AĤ = Ĥ(vapor, 300°C, 3 atm) - Ĥ(solid, 25°C, 1 atm) However, we do not have such a table. Our task is then to construct a hypothetical process path from the solid at 25°C and 1 atm to the vapor at 300°C and 3 atm. To do so, we will look ahead a bit and note that Table B.1 gives enthalpy changes for the melting of phenol at 1 atm and 42.5°C (the normal melting point of phenol) and for the vaporization of phenol at 1 atm and 181.4°C (the normal boiling point of phenol). We therefore choose the following hypothetical process path: Phnhenol(C₂H-OH). {" J 63 50 ENG Sign in I ● 5:53 AM 5/8/2023 + O {0}
||! PDF *Elementary Principles of Chemic X + 60°F Clear File | E:/Elementary%20Principles%20of%20Chemical%20Processes,%204th%20Edition%20(%20PDF Drive%20).pdf Draw 2 T Read aloud 406 CHAPTER 8 Balances on Nonreactive Processes Test Yourself 426 of 695 OD However, we do not have such a table. Our task is then to construct a hypothetical process path from the solid at 25°C and 1 atm to the vapor at 300°C and 3 atm. To do so, we will look ahead a bit and note that Table B.1 gives enthalpy changes for the melting of phenol at 1 atm and 42.5°C (the normal melting point of phenol) and for the vaporization of phenol at 1 atm and 181.4°C (the normal boiling point of phenol). We therefore choose the following hypothetical process path: Ph (s, 25°C, 1 atm) Q Search Ph (s, 42.5°C, 1 atm) Ph (1, 42.5°C, 1 atm) Ph (1, 181.4°C, 1 atm) Ph=phenol(C,H,OH) (True path) AĤ AĤ₁ ΔΗ͂, AĤ3 ΔΗ͂Α Ph (v. 300.0°C, 3 atm) AĤ6 Ph (v, 300.0°C, 1 atm) Δῆς Ph (v, 181.4°C, 1 atm) Notice that in this path, the first, third, and fifth steps are Type 2 (change in T at constant P), the second and fourth steps are Type 3 (change in phase at constant T and P), and the sixth step is Type 1 (change in P at constant T). Also notice that the phase changes were made to occur at the conditions for which tabulated enthalpy changes are available. The next step in the calculation would be to determine the values of AĤ for Steps 1, 3, 5, and 6 using methods to be given in Section 8.2; read the values of AH₂ and AĤ4 from Table B.1; and then use the fact that enthalpy is a state property to calculate the desired AĤ (AĦ for the upper dashed line in the figure) as AĤ = AĤ₁ + AĤ₂ + AĤ3 + AĤ4 + AĤ5 + AĤ6 Construct a process nath for each of the following processes consisting of sequential stens of the {" J 63 50 ^ ENG Sign in I 00 3:40 AM 5/8/2023 + ☐ {0}
Transcribed Image Text:||! PDF *Elementary Principles of Chemic X + 60°F Clear File | E:/Elementary%20Principles%20of%20Chemical%20Processes,%204th%20Edition%20(%20PDF Drive%20).pdf Draw 2 T Read aloud 406 CHAPTER 8 Balances on Nonreactive Processes Test Yourself 426 of 695 OD However, we do not have such a table. Our task is then to construct a hypothetical process path from the solid at 25°C and 1 atm to the vapor at 300°C and 3 atm. To do so, we will look ahead a bit and note that Table B.1 gives enthalpy changes for the melting of phenol at 1 atm and 42.5°C (the normal melting point of phenol) and for the vaporization of phenol at 1 atm and 181.4°C (the normal boiling point of phenol). We therefore choose the following hypothetical process path: Ph (s, 25°C, 1 atm) Q Search Ph (s, 42.5°C, 1 atm) Ph (1, 42.5°C, 1 atm) Ph (1, 181.4°C, 1 atm) Ph=phenol(C,H,OH) (True path) AĤ AĤ₁ ΔΗ͂, AĤ3 ΔΗ͂Α Ph (v. 300.0°C, 3 atm) AĤ6 Ph (v, 300.0°C, 1 atm) Δῆς Ph (v, 181.4°C, 1 atm) Notice that in this path, the first, third, and fifth steps are Type 2 (change in T at constant P), the second and fourth steps are Type 3 (change in phase at constant T and P), and the sixth step is Type 1 (change in P at constant T). Also notice that the phase changes were made to occur at the conditions for which tabulated enthalpy changes are available. The next step in the calculation would be to determine the values of AĤ for Steps 1, 3, 5, and 6 using methods to be given in Section 8.2; read the values of AH₂ and AĤ4 from Table B.1; and then use the fact that enthalpy is a state property to calculate the desired AĤ (AĦ for the upper dashed line in the figure) as AĤ = AĤ₁ + AĤ₂ + AĤ3 + AĤ4 + AĤ5 + AĤ6 Construct a process nath for each of the following processes consisting of sequential stens of the {" J 63 50 ^ ENG Sign in I 00 3:40 AM 5/8/2023 + ☐ {0}
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