Calculate the entropy change when a gas condenses at its boiling point. Calculate the entropy change when when 2.47 moles of methane condenses at its boiling point of -162°C. The heat of vaporization of CH4 is 8.2 kJ/mol. AS = J/K Check & Submit Answer Show Approach
Calculate the entropy change when a gas condenses at its boiling point. Calculate the entropy change when when 2.47 moles of methane condenses at its boiling point of -162°C. The heat of vaporization of CH4 is 8.2 kJ/mol. AS = J/K Check & Submit Answer Show Approach
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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Could use some help on these two please
![**Problem Description:**
Calculate the entropy change when a gas condenses at its boiling point.
**Given:**
Calculate the entropy change when 2.47 moles of methane condenses at its boiling point of -162°C. The heat of vaporization of CH₄ is 8.2 kJ/mol.
**Solution:**
ΔS = ____ J/K
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Transcribed Image Text:**Problem Description:**
Calculate the entropy change when a gas condenses at its boiling point.
**Given:**
Calculate the entropy change when 2.47 moles of methane condenses at its boiling point of -162°C. The heat of vaporization of CH₄ is 8.2 kJ/mol.
**Solution:**
ΔS = ____ J/K
**Interactive Elements:**
- **Check & Submit Answer** button
- **Show Approach** link
![Predict the sign and calculate ΔS° for a reaction.
**Consider the reaction**
\[2\text{CO}(g) + 2\text{NO}(g) \rightarrow 2\text{CO}_2(g) + \text{N}_2(g)\]
Based upon the stoichiometry of the reaction, the sign of ΔS°\(_{\text{rxn}}\) should be __.
Using standard thermodynamic data (*in the Chemistry References*), calculate ΔS°\(_{\text{rxn}}\) at 25°C.
ΔS°\(_{\text{rxn}}\) = __ J/K·mol](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F03536715-3e1d-4765-9555-fb0adbd33776%2Fb77eda85-be61-4626-a6a0-88aae1c92bd2%2F3v88ljo_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Predict the sign and calculate ΔS° for a reaction.
**Consider the reaction**
\[2\text{CO}(g) + 2\text{NO}(g) \rightarrow 2\text{CO}_2(g) + \text{N}_2(g)\]
Based upon the stoichiometry of the reaction, the sign of ΔS°\(_{\text{rxn}}\) should be __.
Using standard thermodynamic data (*in the Chemistry References*), calculate ΔS°\(_{\text{rxn}}\) at 25°C.
ΔS°\(_{\text{rxn}}\) = __ J/K·mol
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