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One hundred g-moles per hour of liquid n-hexane at 25°C and 7 bar is vaporized and heated to 300°C at constant pressure. Neglecting the effect of pressure on enthalpy, estimate the rate at which heat must be supplied.

One hundred g-moles per hour of liquid n-hexane at 25°C and 7 bar is vaporized and heated to 300°C at constant pressure. Neglecting the effect of pressure on enthalpy, estimate the rate at which heat must be supplied.

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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1 51°F Clear Elementary Principles of Chemica X + File | E:/Elementary%20Principles%20of%20Chemical%20Processes,%204th%20Edition%20(%20PDF Drive%20).pdf Draw (T) Read aloud Example 8.4-2 Solution An energy balance yields ←→ Vaporization and Heating One hundred g-moles per hour of liquid n-hexane at 25°C and 7 bar is vaporized and heated to 300°C at constant pressure. Neglecting the effect of pressure on enthalpy, estimate the rate at which heat must be supplied. Q Search 446 of 695 Q =ΔΗ (W, = ΔΕ, = 0, ΔΕ, ~ 0) Therefore an evaluation of AH will yield the desired value of Q. From the Antoine equation (Table B.4) or the APEx function AntoineT (“n-hexane,” 5250), the temperature at which the vapor pressure of n-hexafe is 7 bar (5250 mm Hg) is 146°C, and this is therefore the temperature at which the vaporization actually occurs. However, Table B.1 lists a value of AĤ, at the normal boiling point of n-hexane, AĤ = 28.85 kJ/mol at 69°C We must therefore find a path that takes hexane from a liquid to a vapor at 69°C, rather than at the true vaporization temperature of 146°C. As noted previously, the change in enthalpy associated with a process may be determined from any convenient path as long as the initial and final points of the chosen path correspond to those of the process. The diagram shown on the following page illustrates several possible paths from liquid hexane at 25°C to hexane vapor at 300°C. State 1 n-C6H₁4(1) 25°C, 7 bar State 2 ETA H State 4 n-C6H₁4(v) 25°C, 7 bar State 5 8.4 Phase-Change Operations 427 State 7 n-C6H₁4(v) 300°C, 7 bar I < Ơ re 80 J VENG Sign in 2:14 AM 5/6/2023 • la + O
Transcribed Image Text:1 51°F Clear Elementary Principles of Chemica X + File | E:/Elementary%20Principles%20of%20Chemical%20Processes,%204th%20Edition%20(%20PDF Drive%20).pdf Draw (T) Read aloud Example 8.4-2 Solution An energy balance yields ←→ Vaporization and Heating One hundred g-moles per hour of liquid n-hexane at 25°C and 7 bar is vaporized and heated to 300°C at constant pressure. Neglecting the effect of pressure on enthalpy, estimate the rate at which heat must be supplied. Q Search 446 of 695 Q =ΔΗ (W, = ΔΕ, = 0, ΔΕ, ~ 0) Therefore an evaluation of AH will yield the desired value of Q. From the Antoine equation (Table B.4) or the APEx function AntoineT (“n-hexane,” 5250), the temperature at which the vapor pressure of n-hexafe is 7 bar (5250 mm Hg) is 146°C, and this is therefore the temperature at which the vaporization actually occurs. However, Table B.1 lists a value of AĤ, at the normal boiling point of n-hexane, AĤ = 28.85 kJ/mol at 69°C We must therefore find a path that takes hexane from a liquid to a vapor at 69°C, rather than at the true vaporization temperature of 146°C. As noted previously, the change in enthalpy associated with a process may be determined from any convenient path as long as the initial and final points of the chosen path correspond to those of the process. The diagram shown on the following page illustrates several possible paths from liquid hexane at 25°C to hexane vapor at 300°C. State 1 n-C6H₁4(1) 25°C, 7 bar State 2 ETA H State 4 n-C6H₁4(v) 25°C, 7 bar State 5 8.4 Phase-Change Operations 427 State 7 n-C6H₁4(v) 300°C, 7 bar I < Ơ re 80 J VENG Sign in 2:14 AM 5/6/2023 • la + O
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