Calculate the change in entropy of the system for the following process: 10.0g of ice at -10.0°C is converted into water vapour 115.0°C at a constant pressure of 1 bar. Calculate this by dividing this process up into individual steps for heating and each phase transition. The heat capacities and enthalpy changes for H₂O are: Cp (H₂O, solid, 1bar) = 37.6 Cp (H₂O, gas, 1 bar) = 33.6 AHfusion (H₂0, 1bar, Tfus) = 6.01 J mol K J mol K J mol K C„(H₂O, liquid, 1bar) = 75.3 J mol K AHvaporization(H20, 1bar, Trap) = 40.7 J mol K
Calculate the change in entropy of the system for the following process: 10.0g of ice at -10.0°C is converted into water vapour 115.0°C at a constant pressure of 1 bar. Calculate this by dividing this process up into individual steps for heating and each phase transition. The heat capacities and enthalpy changes for H₂O are: Cp (H₂O, solid, 1bar) = 37.6 Cp (H₂O, gas, 1 bar) = 33.6 AHfusion (H₂0, 1bar, Tfus) = 6.01 J mol K J mol K J mol K C„(H₂O, liquid, 1bar) = 75.3 J mol K AHvaporization(H20, 1bar, Trap) = 40.7 J mol K
Chemistry & Chemical Reactivity
9th Edition
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter18: Principles Of Chemical Reactivity: Entropy And Free Energy
Section18.3: Entropy: A Microscopic Understanding
Problem 2RC
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Transcribed Image Text:Calculate the change in entropy of the system for the following process:
10.0g of ice at -10.0°C is converted into water vapour 115.0°C at a constant pressure of 1
bar.
Calculate this by dividing this process up into individual steps for heating and each phase
transition. The heat capacities and enthalpy changes for H₂O are:
Cp (H₂0, solid, 1bar) = 37.6
Cp (H₂O, gas, 1bar) = 33.6
AHfusion (H₂0, 1bar, Tfus) = 6.01
mol K
J
mol K
mol K
C₂(H₂O, liquid, 1bar) = 75.3
mol K
▲Hvaporization (H₂0, 1bar, Tvap) = 40.7
J
mol K
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