· In general, under room temperature, which of the following type(s) of solid(s) would not dissolve in any kind of a solvent? a) network covalent b) ionic or polar molecular c) ionic d) metallic e) polar molecular If at a particular temperature the solubility of oxygen gas in water is 0.771 g/L at an oxygen pressure of around 19.2 atm. What is the Henry's law constant for 02 (in units of L· atm/mol)? 0 = 16.00 amu
· In general, under room temperature, which of the following type(s) of solid(s) would not dissolve in any kind of a solvent? a) network covalent b) ionic or polar molecular c) ionic d) metallic e) polar molecular If at a particular temperature the solubility of oxygen gas in water is 0.771 g/L at an oxygen pressure of around 19.2 atm. What is the Henry's law constant for 02 (in units of L· atm/mol)? 0 = 16.00 amu
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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![### Solubility and Henry's Law
**Question:**
In general, under room temperature, which of the following type(s) of solid(s) would not dissolve in any kind of a solvent?
a) network covalent
b) ionic or polar molecular
c) ionic
d) metallic
e) polar molecular
**Explanation:**
This question probes the solubility characteristics of different types of solids when exposed to solvents under standard room temperature conditions. Understanding why a particular type of solid would or would not dissolve in solvents involves knowledge of intermolecular forces and bonding:
- **Network Covalent**: Typically insoluble in solvents due to strong covalent bonds throughout the entire structure.
- **Ionic or Polar Molecular**: Generally soluble in polar solvents due to ionic/polar interactions.
- **Ionic**: Soluble in polar solvents (e.g., water) due to ion-dipole interactions.
- **Metallic**: Typically insoluble; metallic bonds are not easily disrupted by solvents.
- **Polar Molecular**: Soluble in polar solvents; like dissolves like principle.
**Question:**
If at a particular temperature the solubility of oxygen gas in water is 0.771 g/L at an oxygen pressure of around 19.2 atm. What is the Henry's law constant for \( O_{2} \) (in units of L ⋅ atm/mol)?
Given:
\[ O = 16.00 \, \text{amu} \]
**Explanation:**
To determine Henry's law constant (\( k_H \)), the solubility of the gas in the solvent, and the partial pressure of the gas above the solvent are used. Henry's law is described by the equation:
\[ C = k_H \cdot P \]
where:
- \( C \) is the concentration of the dissolved gas (solubility),
- \( k_H \) is the Henry's law constant,
- \( P \) is the partial pressure of the gas.
Given data:
- Solubility \( C = 0.771 \, \text{g/L} \)
- Partial pressure \( P = 19.2 \, \text{atm} \)
- Molecular weight of \( O_{2} \) = \( 2 \times 16.00 \, \text{amu} = 32.00 \, \text{g/mol} \)
First, convert the sol](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F1243504b-5612-4510-ba6c-7b5ec7c70d6e%2F5521a099-4785-4458-b7ff-7ff66b1cac77%2Fohn9eeq_processed.png&w=3840&q=75)
Transcribed Image Text:### Solubility and Henry's Law
**Question:**
In general, under room temperature, which of the following type(s) of solid(s) would not dissolve in any kind of a solvent?
a) network covalent
b) ionic or polar molecular
c) ionic
d) metallic
e) polar molecular
**Explanation:**
This question probes the solubility characteristics of different types of solids when exposed to solvents under standard room temperature conditions. Understanding why a particular type of solid would or would not dissolve in solvents involves knowledge of intermolecular forces and bonding:
- **Network Covalent**: Typically insoluble in solvents due to strong covalent bonds throughout the entire structure.
- **Ionic or Polar Molecular**: Generally soluble in polar solvents due to ionic/polar interactions.
- **Ionic**: Soluble in polar solvents (e.g., water) due to ion-dipole interactions.
- **Metallic**: Typically insoluble; metallic bonds are not easily disrupted by solvents.
- **Polar Molecular**: Soluble in polar solvents; like dissolves like principle.
**Question:**
If at a particular temperature the solubility of oxygen gas in water is 0.771 g/L at an oxygen pressure of around 19.2 atm. What is the Henry's law constant for \( O_{2} \) (in units of L ⋅ atm/mol)?
Given:
\[ O = 16.00 \, \text{amu} \]
**Explanation:**
To determine Henry's law constant (\( k_H \)), the solubility of the gas in the solvent, and the partial pressure of the gas above the solvent are used. Henry's law is described by the equation:
\[ C = k_H \cdot P \]
where:
- \( C \) is the concentration of the dissolved gas (solubility),
- \( k_H \) is the Henry's law constant,
- \( P \) is the partial pressure of the gas.
Given data:
- Solubility \( C = 0.771 \, \text{g/L} \)
- Partial pressure \( P = 19.2 \, \text{atm} \)
- Molecular weight of \( O_{2} \) = \( 2 \times 16.00 \, \text{amu} = 32.00 \, \text{g/mol} \)
First, convert the sol
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