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Based on the calculated Δ?vap values, arrange the liquid samples in order from most ordered to least ordered. CH3OH  C6H6 C4H10

Based on the calculated Δ?vap values, arrange the liquid samples in order from most ordered to least ordered. CH3OH  C6H6 C4H10

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
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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Based on the calculated Δ?vap values, arrange the liquid samples in order from most ordered to least ordered.

CH3OH 

C6H6

C4H10

### Heat of Vaporization and Entropy of Vaporization Three liquid samples of known masses are heated to their boiling points using a heater rated at 525.0 W. Once the boiling points of each sample are reached, the samples are heated for an additional 3.60 minutes, which results in the vaporization of some of each sample. After 3.60 minutes, the samples are cooled and the masses of the remaining liquids are determined. The process is performed at constant pressure. The results are recorded in the table below. | Liquid | Boiling point (°C) | Initial mass (g) | Final mass (g) | |-----------|--------------------|------------------|----------------| | CH<sub>3</sub>OH | 64.5 | 407.65 | 312.53 | | C<sub>4</sub>H<sub>10</sub> | -1.00 | 410.2 | 105.08 | | C<sub>6</sub>H<sub>6</sub> | 80.1 | 593.3 | 331.18 | **Objective:** Calculate the molar enthalpy of vaporization, ΔH<sub>vap</sub>, and the molar entropy of vaporization, ΔS<sub>vap</sub>, for each sample. Assume that all of the heat from the heater goes into the sample. **Calculations:** 1. **ΔH<sub>vap</sub> of CH<sub>3</sub>OH**: - Input box for calculation result (kJ/mol) 2. **ΔS<sub>vap</sub> of CH<sub>3</sub>OH**: - Input box for calculation result (J/mol·K)
Transcribed Image Text:### Heat of Vaporization and Entropy of Vaporization Three liquid samples of known masses are heated to their boiling points using a heater rated at 525.0 W. Once the boiling points of each sample are reached, the samples are heated for an additional 3.60 minutes, which results in the vaporization of some of each sample. After 3.60 minutes, the samples are cooled and the masses of the remaining liquids are determined. The process is performed at constant pressure. The results are recorded in the table below. | Liquid | Boiling point (°C) | Initial mass (g) | Final mass (g) | |-----------|--------------------|------------------|----------------| | CH<sub>3</sub>OH | 64.5 | 407.65 | 312.53 | | C<sub>4</sub>H<sub>10</sub> | -1.00 | 410.2 | 105.08 | | C<sub>6</sub>H<sub>6</sub> | 80.1 | 593.3 | 331.18 | **Objective:** Calculate the molar enthalpy of vaporization, ΔH<sub>vap</sub>, and the molar entropy of vaporization, ΔS<sub>vap</sub>, for each sample. Assume that all of the heat from the heater goes into the sample. **Calculations:** 1. **ΔH<sub>vap</sub> of CH<sub>3</sub>OH**: - Input box for calculation result (kJ/mol) 2. **ΔS<sub>vap</sub> of CH<sub>3</sub>OH**: - Input box for calculation result (J/mol·K)
### Thermodynamic Properties of Various Compounds In the context of phase changes, particularly vaporization, we often examine the enthalpy (\( \Delta H \)) and entropy (\( \Delta S \)) of vaporization. Below is a table format into which data for the various compounds can be filled. #### Methanol (\( \text{CH}_3\text{OH} \)) - **Entropy of Vaporization (\( \Delta S_{\text{vap}} \))** of \( \text{CH}_3\text{OH} \)): - Input your value here: `_________________` J/mol·K #### Butane (\( \text{C}_4\text{H}_{10} \)) - **Enthalpy of Vaporization (\( \Delta H_{\text{vap}} \))** of \( \text{C}_4\text{H}_{10} \)): - Input your value here: `_________________` kJ/mol - **Entropy of Vaporization (\( \Delta S_{\text{vap}} \))** of \( \text{C}_4\text{H}_{10} \)): - Input your value here: `_________________` J/mol·K #### Benzene (\( \text{C}_6\text{H}_6 \)) - **Enthalpy of Vaporization (\( \Delta H_{\text{vap}} \))** of \( \text{C}_6\text{H}_6 \)): - Input your value here: `_________________` kJ/mol - **Entropy of Vaporization (\( \Delta S_{\text{vap}} \))** of \( \text{C}_6\text{H}_6 \)): - Input your value here: `_________________` J/mol·K ### Measurement Units - **Enthalpy of vaporization (\( \Delta H_{\text{vap}} \))** is measured in kilojoules per mole (kJ/mol). - **Entropy of vaporization (\( \Delta S_{\text{vap}} \))** is measured in joules per mole per kelvin (J/mol·K). These values are essential for understanding the energy requirements and changes associated with phase transitions from liquid to gas for these compounds.
Transcribed Image Text:### Thermodynamic Properties of Various Compounds In the context of phase changes, particularly vaporization, we often examine the enthalpy (\( \Delta H \)) and entropy (\( \Delta S \)) of vaporization. Below is a table format into which data for the various compounds can be filled. #### Methanol (\( \text{CH}_3\text{OH} \)) - **Entropy of Vaporization (\( \Delta S_{\text{vap}} \))** of \( \text{CH}_3\text{OH} \)): - Input your value here: `_________________` J/mol·K #### Butane (\( \text{C}_4\text{H}_{10} \)) - **Enthalpy of Vaporization (\( \Delta H_{\text{vap}} \))** of \( \text{C}_4\text{H}_{10} \)): - Input your value here: `_________________` kJ/mol - **Entropy of Vaporization (\( \Delta S_{\text{vap}} \))** of \( \text{C}_4\text{H}_{10} \)): - Input your value here: `_________________` J/mol·K #### Benzene (\( \text{C}_6\text{H}_6 \)) - **Enthalpy of Vaporization (\( \Delta H_{\text{vap}} \))** of \( \text{C}_6\text{H}_6 \)): - Input your value here: `_________________` kJ/mol - **Entropy of Vaporization (\( \Delta S_{\text{vap}} \))** of \( \text{C}_6\text{H}_6 \)): - Input your value here: `_________________` J/mol·K ### Measurement Units - **Enthalpy of vaporization (\( \Delta H_{\text{vap}} \))** is measured in kilojoules per mole (kJ/mol). - **Entropy of vaporization (\( \Delta S_{\text{vap}} \))** is measured in joules per mole per kelvin (J/mol·K). These values are essential for understanding the energy requirements and changes associated with phase transitions from liquid to gas for these compounds.
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