a) Calculate the heat evolved (in J) when 100.0 g of pure H₂SO4 is added to 100.0 g of H₂O. b) Calculate the heat evolved (in J) when the solution prepared in part (a) is diluted with an additional 100 g of H₂O. c) Calculate the heat evolved (in J) when 100.0 g of a 60 wt% solution of H₂SO4 is mixed with 75.0 g of a 25 wt% solution of H₂SO4.
a) Calculate the heat evolved (in J) when 100.0 g of pure H₂SO4 is added to 100.0 g of H₂O. b) Calculate the heat evolved (in J) when the solution prepared in part (a) is diluted with an additional 100 g of H₂O. c) Calculate the heat evolved (in J) when 100.0 g of a 60 wt% solution of H₂SO4 is mixed with 75.0 g of a 25 wt% solution of H₂SO4.
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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Transcribed Image Text:1) (Note that Figure 8.1-1 will be useful in solving this problem) The molar
integral heat of solution AH is defined as the change in enthalpy that results when
1.00 mole of solute (component 1) is isothermally mixed with N₂ moles of solvent
(component 2) and is given by the following
AsH is easily measured in an isothermal calorimeter by monitoring the heat evolved
or absorbed on successive additions of solvent to a given amount of solute. The
table below gives the integral heat-of-solution data for 1.00 mol of sulfuric acid
(H2SO4) in water at 25 °C. Note, the negative sign indicates that heat is evolved in
the dilution process.
N₂
-ASH
(moles H₂O) (J/1.00 mole acid)
8242
28200
34980
44690
54440
Enthalpy, (kJ/kg) of mixture including vapor
450
a) Calculate the heat evolved (in J) when 100.0 g of pure H₂SO4 is added to 100.0
g of H₂O.
400
b) Calculate the heat evolved (in J) when the solution prepared in part (a) is diluted
with an additional 100 g of H₂O.
350
c) Calculate the heat evolved (in J) when 100.0 g of a 60 wt % solution of H₂SO4
is mixed with 75.0 g of a 25 wt% solution of H₂SO4.
300
250
200
150
100
50
0
-50
-100
-150
AsH = (1 + N₂)H mix − H₁ − N₂H₂ = Ħ₁ + N₂H₂ − H₁ − N₂H₂ .
-
-200
-250
0.250
1.00
1.50
2.33
4.00
-300
-350
0
100°C
104.4°C
110°C
Boiling point at 0.1 MPa
20
115.6°C
121.1°C
148.9°C
0°℃
21.1°C
37.8°C
65.6°C
176.7°C
204.4°C
232.2°C
260°C
287.8°C
Liquid +
Vapor
93.3°C
Liquid
N₂
(moles H₂O)
121.1°C
40
60
Wt. percentage H₂SO4
148.9°C
80
5.44
9.00
10.1
19.0
20.0
Boiling point at 0.1 MPa -
176.7°C
100
-A,H
(J/ 1.00 mole acid)
58370
62800
64850
70710
71970
287.8°C
260°C
232.2°C
Transcribed Image Text:10
@a) -59,560 J released
(b)-7140 J released
(c) -2970 J must be removed.
(d) see figure
answers may vary
slightly from those
listed here
→ H₁-H₁ = -46,000 J/mol
F₁₂-H₂2₂ = -2300J/mol
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