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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States of Matter
The substance that constitutes everything in the universe is known as matter. Matter comprises atoms which in turn are composed of electrons, protons, and neutrons. Different atoms combine together to give rise to molecules that act as a foundation for all kinds of substances. There are five states of matter based on their energies of attraction, namely solid, liquid, gases, plasma, and BEC (Bose-Einstein condensates).
Chemical Reactions and Equations
When a chemical species is transformed into another chemical species it is said to have undergone a chemical reaction. It consists of breaking existing bonds and forming new bonds by changing the position of electrons. These reactions are best explained using a chemical equation.
Question
![### Educational Resource on Trouton's Rule
**Understanding Trouton's Rule**
Trouton's rule states that the molar enthalpy of vaporization (ΔH_vap) of a liquid that lacks strong molecular interactions (such as hydrogen bonding or ion-ion attractions) can be estimated using the relationship:
\[ \Delta H_{\text{vap}} = \left( 85 \: \text{J} \cdot \text{K}^{-1} \cdot \text{mol}^{-1} \right) T_b \]
where:
- \( \Delta H_{\text{vap}} \) is the molar enthalpy of vaporization.
- \( T_b \) is the normal boiling point of the liquid in kelvins (K).
### Data Table
The table below lists the chemical formulas, molar enthalpies of vaporization (ΔH_vap), boiling points (in K), and molar enthalpies of fusion (ΔH_fus) for different compounds:
| Compound | Chemical formula | \( \Delta H_{\text{vap}} \) (kJ·mol\(^{-1}\)) | Boiling point (K) | \( \Delta H_{\text{fus}} \) (kJ·mol\(^{-1}\)) |
|----------------------|-------------------|----------------------------------|-------------------|---------------------------------|
| chloromethane | CH\(_3\)Cl | 21.40 | 249.06 | 6.43 |
| water | H\(_2\)O | 40.65 | 373.15 | 6.01 |
| hydrogen sulfide | H\(_2\)S | 18.67 | 213.60 | 18.67 |
### Applying Trouton's Rule
To estimate the value of \( \Delta H_{\text{vap}} \) for chloromethane using Trouton's rule, substitute the normal boiling point (\( T_b \)) of chloromethane into the equation:
\[ \Delta H_{\text{vap}} = ( 85 \: \text{J} \cdot \text{K}^{-1} \cdot \text{mol}^{-1} ) \times T_b \]
Given:
- \( T_b \) for chloromethane = 249.06 K
Therefore](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ff00f8b75-2bac-4335-a200-62a4fa07a89d%2F8ae7424b-ab27-496c-9562-447b9b1b22f4%2Fbp8zuj3_processed.png&w=3840&q=75)
Transcribed Image Text:### Educational Resource on Trouton's Rule
**Understanding Trouton's Rule**
Trouton's rule states that the molar enthalpy of vaporization (ΔH_vap) of a liquid that lacks strong molecular interactions (such as hydrogen bonding or ion-ion attractions) can be estimated using the relationship:
\[ \Delta H_{\text{vap}} = \left( 85 \: \text{J} \cdot \text{K}^{-1} \cdot \text{mol}^{-1} \right) T_b \]
where:
- \( \Delta H_{\text{vap}} \) is the molar enthalpy of vaporization.
- \( T_b \) is the normal boiling point of the liquid in kelvins (K).
### Data Table
The table below lists the chemical formulas, molar enthalpies of vaporization (ΔH_vap), boiling points (in K), and molar enthalpies of fusion (ΔH_fus) for different compounds:
| Compound | Chemical formula | \( \Delta H_{\text{vap}} \) (kJ·mol\(^{-1}\)) | Boiling point (K) | \( \Delta H_{\text{fus}} \) (kJ·mol\(^{-1}\)) |
|----------------------|-------------------|----------------------------------|-------------------|---------------------------------|
| chloromethane | CH\(_3\)Cl | 21.40 | 249.06 | 6.43 |
| water | H\(_2\)O | 40.65 | 373.15 | 6.01 |
| hydrogen sulfide | H\(_2\)S | 18.67 | 213.60 | 18.67 |
### Applying Trouton's Rule
To estimate the value of \( \Delta H_{\text{vap}} \) for chloromethane using Trouton's rule, substitute the normal boiling point (\( T_b \)) of chloromethane into the equation:
\[ \Delta H_{\text{vap}} = ( 85 \: \text{J} \cdot \text{K}^{-1} \cdot \text{mol}^{-1} ) \times T_b \]
Given:
- \( T_b \) for chloromethane = 249.06 K
Therefore
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