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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
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) (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: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
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
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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