Calculate the change in entropy of a 1kg of He gas at the normal boiling point of He when it all condenses isothermally to 1L of liquid He.TABLE 17.4 Heats of Fusion and VaporizationNormal MeltingPolntNormal BollingHeat ofHeat ofPolntFuslon, L4(J/kg)Vaportzation, I(J/kg)SubstanceKK"CHelium4.216-268.9320.9 x 10'Hydrogen13.84-259.3158.6 x 1020.26-252.89452 x 10Nitrogen63.18-209.9725.5 x 1077.34-195.8201 x 10Oxygen54.36-218.7913.8 x 1090.18-183.0213 х 10°Elhanol854 x 10199-114104.2 x 1035178Mercury234-3911.8 x 10630357272 x 10Water273.150.00334 x 10373.15100.002256 x 10Sulfur39211938.1 x 10717.75444,60326 x 10Lead600.5327.324.5 x 1020231750871 x 10Antimony903.65630.50165 x 1017131440S61 x 10Silver1233.95960.8088.3 x 10246621932336 x 10Gold1336.151063.0064.5 x 10293326601578 x 10'Соррer13561083134 x 10146011875069 x 10"A pressure in excess of 25 atmospheres is required to make helium solidify. At I atmosphere pressure, helium remainsa liquid down to absolute zero.

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Calculate the change in entropy of a 1kg of He gas at the normal boiling point of He when it all condenses isothermally to 1L of liquid He. TABLE 17.4 Heats of Fusion and Vaporization Normal Melting Polnt Normal Bolling Polnt Heat of Fuslon, L4 (J/kg) Heat of Vaportzation, I (J/kg) Substance K "C K "C Helium 4.216 -268.93 20.9 × 10' Hydrogen 13.84 -259.31 58.6 x 10 20.26 -252.89 452 x 10 Nitrogen 63.18 -209.97 25.5 x 10 77.34 -195.8 201 x 10 Oxygen 54.36 -218.79 13.8 x 10 90.18 -183.0 213 x 10 Eihanol 199 -114 104.2 x 10 351 ואר 854 x 10 Mercury 234 -39 11.8 x 10 630 357 272 x 10 Water 273.15 0.00 334 x 10 373.15 100.00 2256 x 10 Sulfur 392 119 38.1 x 10' 717.75 444,60 326 x 10 Lead 600.5 327.3 24.5 x 10 2023 1750 871 x 10 Antimony 90365 630.50 165 x 10 1713 1440 561 x 10 Silver 123395 960.80 883 x 10 2466 2193 2336 x 10 Gold 1336.15 1063.00 64.5 x 10 2933 2660 1578 x 10 Copper 1356 1083 134 x 10 1460 1187 5069 x 10' "A pressure in excess of 25 atmospheres is required to make helium solidify. At I atmosphere pressure, helium remains a liquid down to absolute zero.

Calculate the change in entropy of a 1kg of He gas at the normal boiling point of He when it all condenses isothermally to 1L of liquid He. TABLE 17.4 Heats of Fusion and Vaporization Normal Melting Polnt Normal Bolling Polnt Heat of Fuslon, L4 (J/kg) Heat of Vaportzation, I (J/kg) Substance K "C K "C Helium 4.216 -268.93 20.9 × 10' Hydrogen 13.84 -259.31 58.6 x 10 20.26 -252.89 452 x 10 Nitrogen 63.18 -209.97 25.5 x 10 77.34 -195.8 201 x 10 Oxygen 54.36 -218.79 13.8 x 10 90.18 -183.0 213 x 10 Eihanol 199 -114 104.2 x 10 351 ואר 854 x 10 Mercury 234 -39 11.8 x 10 630 357 272 x 10 Water 273.15 0.00 334 x 10 373.15 100.00 2256 x 10 Sulfur 392 119 38.1 x 10' 717.75 444,60 326 x 10 Lead 600.5 327.3 24.5 x 10 2023 1750 871 x 10 Antimony 90365 630.50 165 x 10 1713 1440 561 x 10 Silver 123395 960.80 883 x 10 2466 2193 2336 x 10 Gold 1336.15 1063.00 64.5 x 10 2933 2660 1578 x 10 Copper 1356 1083 134 x 10 1460 1187 5069 x 10' "A pressure in excess of 25 atmospheres is required to make helium solidify. At I atmosphere pressure, helium remains a liquid down to absolute zero.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Dissolution of ionic compounds generally involves an increase in entropy (+ΔS°), but for a few specific metal ions, dissolution of the ionic compound can lead to a decrease in entropy. For example, the dissolution of magnesium chloride (MgCl2) has a ΔS° = -115 J K-1 mol-1. Explain this decrease in entropy
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