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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
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
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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 **Interactive Elements:** - **Check & Submit Answer** button - **Show Approach** link
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
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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