Consider the following elementary reaction: NO2 (g) +O3 (g) →NO3 (g) +O2 (g)Suppose we let k1 stand for the rate constant of this reaction, and k−1 stand for the rate constant of the reverse reaction. Write an expression that gives the equilibrium concentration of NO2 in terms of k1 , k−1 , and the equilibrium concentrations of O3 , NO3 , and O2 .
Consider the following elementary reaction: NO2 (g) +O3 (g) →NO3 (g) +O2 (g)Suppose we let k1 stand for the rate constant of this reaction, and k−1 stand for the rate constant of the reverse reaction. Write an expression that gives the equilibrium concentration of NO2 in terms of k1 , k−1 , and the equilibrium concentrations of O3 , NO3 , and O2 .
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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Consider the following elementary reaction:
NO2
(g)
+O3
(g)
→NO3
(g)
+O2
(g)Suppose we let
k1
stand for the rate constant of this reaction, and
k−1
stand for the rate constant of the reverse reaction.
Write an expression that gives the equilibrium concentration of
NO2
in terms of
k1
,
k−1
, and the equilibrium concentrations of
O3
,
NO3
, and
O2
.
Transcribed Image Text:### Intermolecular Forces of Selected Compounds
#### Table: Intermolecular Forces Acting Between Molecules
| Compound | Intermolecular Forces |
|----------------------|---------------------------------------------------|
| | Dispersion | Dipole | Hydrogen-Bonding |
| **Nitrogen Trifluoride (NF₃)** | ☑ | ☑ | |
| **COS (Carbonyl Sulfide)** | ☑ | ☑ | |
| **Ammonia (NH₃)** | ☑ | ☑ | ☑ |
| **Carbon Tetrafluoride (CF₄)** | ☑ | | |
**Key:**
- **Dispersion:** This is a type of weak intermolecular force also known as London dispersion force.
- **Dipole:** This involves intermolecular forces between molecules that have a separation of positive and negative charges.
- **Hydrogen Bonding:** This is a specific, generally stronger type of dipole-dipole interaction that occurs when hydrogen is bonded to electronegative atoms like nitrogen, oxygen, or fluorine.
#### Explanation:
The table presents a selection of compounds and identifies which intermolecular forces are present between their molecules.
1. **Nitrogen Trifluoride (NF₃):**
- Exhibits both dispersion and dipole intermolecular forces.
- Does not exhibit hydrogen bonding.
2. **Carbonyl Sulfide (COS):**
- Exhibits both dispersion and dipole intermolecular forces.
- Does not exhibit hydrogen bonding.
3. **Ammonia (NH₃):**
- Exhibits dispersion and dipole intermolecular forces.
- Additionally, exhibits hydrogen bonding due to the presence of hydrogen atoms bonded to nitrogen.
4. **Carbon Tetrafluoride (CF₄):**
- Exhibits dispersion forces.
- Does not exhibit dipole or hydrogen bonding forces.
This understanding of intermolecular forces is fundamental in predicting the physical properties and behaviors of these substances in various contexts, including boiling points, melting points, solubility, and vapor pressure.
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