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
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...
Related questions
Question
![**Title: Calculating the Change in Entropy for a Phase Transition Process**
**Introduction:**
This section details the steps necessary to calculate the change in entropy as 10.0g of ice at -10.0°C is transformed into water vapor at 115.0°C at a constant pressure of 1 bar. This is achieved by segmenting the process into discrete steps for heating and phase transitions.
**Heat Capacities and Enthalpy Changes for H₂O:**
- **Solid Phase Heat Capacity:**
\[
\bar{C}_p(H_2O, \text{solid}, 1 \text{ bar}) = 37.6 \frac{J}{\text{mol K}}
\]
- **Liquid Phase Heat Capacity:**
\[
\bar{C}_p(H_2O, \text{liquid}, 1 \text{ bar}) = 75.3 \frac{J}{\text{mol K}}
\]
- **Gas Phase Heat Capacity:**
\[
\bar{C}_p(H_2O, \text{gas}, 1 \text{ bar}) = 33.6 \frac{J}{\text{mol K}}
\]
- **Enthalpy of Fusion:**
\[
\Delta H_\text{fusion}(H_2O, 1 \text{ bar}, T_\text{fus}) = 6.01 \frac{J}{\text{mol}}
\]
- **Enthalpy of Vaporization:**
\[
\Delta H_\text{vaporization}(H_2O, 1 \text{ bar}, T_\text{vap}) = 40.7 \frac{J}{\text{mol}}
\]
**Discussion:**
To calculate the total entropy change, consider each step:
1. Heating ice from -10.0°C to 0°C.
2. Melting ice to liquid water at 0°C.
3. Heating water from 0°C to 100°C.
4. Vaporizing water at 100°C.
5. Heating water vapor from 100°C to 115.0°C.
By summing the entropy changes for each step, the overall entropy change can be determined. Each heat capacity value and enthalpy change plays a crucial role in these calculations, highlighting the extensive overlaps between](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Faba5746d-e0e8-46ca-a0bb-ec14000055d1%2F0eaf4992-c4db-401b-b8c5-00c786d2e869%2Fao0bdwj_processed.png&w=3840&q=75)
Transcribed Image Text:**Title: Calculating the Change in Entropy for a Phase Transition Process**
**Introduction:**
This section details the steps necessary to calculate the change in entropy as 10.0g of ice at -10.0°C is transformed into water vapor at 115.0°C at a constant pressure of 1 bar. This is achieved by segmenting the process into discrete steps for heating and phase transitions.
**Heat Capacities and Enthalpy Changes for H₂O:**
- **Solid Phase Heat Capacity:**
\[
\bar{C}_p(H_2O, \text{solid}, 1 \text{ bar}) = 37.6 \frac{J}{\text{mol K}}
\]
- **Liquid Phase Heat Capacity:**
\[
\bar{C}_p(H_2O, \text{liquid}, 1 \text{ bar}) = 75.3 \frac{J}{\text{mol K}}
\]
- **Gas Phase Heat Capacity:**
\[
\bar{C}_p(H_2O, \text{gas}, 1 \text{ bar}) = 33.6 \frac{J}{\text{mol K}}
\]
- **Enthalpy of Fusion:**
\[
\Delta H_\text{fusion}(H_2O, 1 \text{ bar}, T_\text{fus}) = 6.01 \frac{J}{\text{mol}}
\]
- **Enthalpy of Vaporization:**
\[
\Delta H_\text{vaporization}(H_2O, 1 \text{ bar}, T_\text{vap}) = 40.7 \frac{J}{\text{mol}}
\]
**Discussion:**
To calculate the total entropy change, consider each step:
1. Heating ice from -10.0°C to 0°C.
2. Melting ice to liquid water at 0°C.
3. Heating water from 0°C to 100°C.
4. Vaporizing water at 100°C.
5. Heating water vapor from 100°C to 115.0°C.
By summing the entropy changes for each step, the overall entropy change can be determined. Each heat capacity value and enthalpy change plays a crucial role in these calculations, highlighting the extensive overlaps between
Expert Solution
Trending now
This is a popular solution!
Step by step
Solved in 9 steps
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Recommended textbooks for you
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY