1. For benzaldehyde, AvapH = 43.44 kJ/mol at 452.7 K (this is the standard boiling point). The heat capacity (in J/mol-K) of benzaldehyde vapor can be modeled for 400 < T< 600 K by 5.5456 x 106 Cp vapor (T) = 115.476 +0.164216 T T² (a) If AvapH = 43.8 kJ/mol at 424 K, and Cplia, the heat capacity of liquid benzaldehyde, is constant between 424 and 452.7 K, what is its value in J/mol.K? (b) Use the information from part (a) to find AvapH (in kJ/mol) at 400 K and 500 K.
1. For benzaldehyde, AvapH = 43.44 kJ/mol at 452.7 K (this is the standard boiling point). The heat capacity (in J/mol-K) of benzaldehyde vapor can be modeled for 400 < T< 600 K by 5.5456 x 106 Cp vapor (T) = 115.476 +0.164216 T T² (a) If AvapH = 43.8 kJ/mol at 424 K, and Cplia, the heat capacity of liquid benzaldehyde, is constant between 424 and 452.7 K, what is its value in J/mol.K? (b) Use the information from part (a) to find AvapH (in kJ/mol) at 400 K and 500 K.
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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![**Transcription for Educational Website:**
1. For benzaldehyde, \( \Delta_{\text{vap}}H = 43.44 \, \text{kJ/mol} \) at 452.7 K (this is the standard boiling point). The heat capacity (in J/mol·K) of benzaldehyde vapor can be modeled for \( 400 < T < 600 \, \text{K} \) by
\[
C_p^{\text{vapor}}(T) = 115.476 + 0.164216 \, T - \frac{5.5456 \times 10^6}{T^2}
\]
(a) If \( \Delta_{\text{vap}}H = 43.8 \, \text{kJ/mol} \) at 424 K, and \( C_p^{\text{liq}} \), the heat capacity of liquid benzaldehyde, is constant between 424 and 452.7 K, what is its value in J/mol·K?
(b) Use the information from part (a) to find \( \Delta_{\text{vap}}H \) (in kJ/mol) at 400 K and 500 K.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F3c924432-5356-4d2a-9799-f03f3a53c4ab%2F766e4ded-efa1-48fc-81e1-e197e0046e10%2Febzu0yc_processed.png&w=3840&q=75)
Transcribed Image Text:**Transcription for Educational Website:**
1. For benzaldehyde, \( \Delta_{\text{vap}}H = 43.44 \, \text{kJ/mol} \) at 452.7 K (this is the standard boiling point). The heat capacity (in J/mol·K) of benzaldehyde vapor can be modeled for \( 400 < T < 600 \, \text{K} \) by
\[
C_p^{\text{vapor}}(T) = 115.476 + 0.164216 \, T - \frac{5.5456 \times 10^6}{T^2}
\]
(a) If \( \Delta_{\text{vap}}H = 43.8 \, \text{kJ/mol} \) at 424 K, and \( C_p^{\text{liq}} \), the heat capacity of liquid benzaldehyde, is constant between 424 and 452.7 K, what is its value in J/mol·K?
(b) Use the information from part (a) to find \( \Delta_{\text{vap}}H \) (in kJ/mol) at 400 K and 500 K.
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