(1) If 30.8 kJ of heat are supplied to a mixture of benzene and its vapour at 353 K, one mole of benzene is vaporised. Calculate the change in entropy for this process.
(1) If 30.8 kJ of heat are supplied to a mixture of benzene and its vapour at 353 K, one mole of benzene is vaporised. Calculate the change in entropy for this process.
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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![In each case values of for substances can be obtained by reference to
Table 2.4.
(1) If 30.8 kJ of heat are supplied to a mixture of benzene and its
vapour at 353 K, one mole of benzene is vaporised. Calculate the
change in entropy for this process.
Candicanner
(3) Calculate the standard entropy of copper at 1800 K, given that, for copper,
= 1356 K, C = 24.5 J K¹ mol (assumed constant in the region 298-1800 K),
Im
L
13.0 kJ mol-¹ and AS298 [Cu(s)] = 33.3 J K¹ mol
1
(4)
For the reaction
298 K
TiO₂ (s) + 2Cl₂(g) + C(s)
TiCl4 (1) + CO₂(g)
Calculate: (a) AS298 and (b) AS98, the temperature at which the commercial reaction
is carried out. Between 298 K and 798 K only TiCl4 goes through a transformation and
the molar heat capacities (assumed constant over the temperature range) required are as
follows:
Cl₂(g)
C(s)
TiO₂ (s)
55
TiC14 (g) CO₂ (g)
157
37
40
8.6
Cp (J K¹ mol ¹)
Le = 138.6 kJ mol-1
Tb
= 413 K
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Transcribed Image Text:In each case values of for substances can be obtained by reference to
Table 2.4.
(1) If 30.8 kJ of heat are supplied to a mixture of benzene and its
vapour at 353 K, one mole of benzene is vaporised. Calculate the
change in entropy for this process.
Candicanner
(3) Calculate the standard entropy of copper at 1800 K, given that, for copper,
= 1356 K, C = 24.5 J K¹ mol (assumed constant in the region 298-1800 K),
Im
L
13.0 kJ mol-¹ and AS298 [Cu(s)] = 33.3 J K¹ mol
1
(4)
For the reaction
298 K
TiO₂ (s) + 2Cl₂(g) + C(s)
TiCl4 (1) + CO₂(g)
Calculate: (a) AS298 and (b) AS98, the temperature at which the commercial reaction
is carried out. Between 298 K and 798 K only TiCl4 goes through a transformation and
the molar heat capacities (assumed constant over the temperature range) required are as
follows:
Cl₂(g)
C(s)
TiO₂ (s)
55
TiC14 (g) CO₂ (g)
157
37
40
8.6
Cp (J K¹ mol ¹)
Le = 138.6 kJ mol-1
Tb
= 413 K
Cancer in
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