Calculate the entropy change associated with transforming 30.0 g of steam at -110.°C to ice at -10.0°C. For H20: kJ (at 0°C) kJ ;(at 100°C) AHfus = 6.008 AHfap = 40.656 mol mol Assume constant heat capacities: CH20(s) = 2.108 J = 4.186 CH20(1) CH20(g) = 1.996 g- K g- K g- K

Calculate the entropy change associated with transforming 30.0 g of steam at -110.°C to ice at -10.0°C. For H20: kJ (at 0°C) kJ ;(at 100°C) AHfus = 6.008 AHfap = 40.656 mol mol Assume constant heat capacities: CH20(s) = 2.108 J = 4.186 CH20(1) CH20(g) = 1.996 g- K g- K g- K

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter16: Thermodynamics: Directionality Of Chemical Reactions

Section16.3: Measuring Dispersal Of Energy: Entropy

Problem 16.1PSP: A chemical reaction transfers 30.8 kJ to a thermal reservoir that has a temperature of 45.3 C before...

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Question

All decimal places should be shown in the solution.
Problem 1.
Calculate the entropy change associated with transforming 30.0 g of steam at -110.°C to ice at -10.0°C.
For H20:
kJ
(at 0°C)
kJ
(at 100°C)
mol
AHfus
= 6.008
AHap
= 40.656-
mol
Assume constant heat capacities:
J
J
CH20(s) = 2.108-
g- K
CH20(1) = 4.186-
g - K
J
= 1.996-
g- K
CH20(g)

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