Use the molar bond enthalpy data in the table to estimate the value of AHxn for the equation C,H,(g) + HBr(g) → C,H,Br(g) The bonding in the molecules is shown. H. H Br C: + H-Br H-Ć- -C-H H' H.
Use the molar bond enthalpy data in the table to estimate the value of AHxn for the equation C,H,(g) + HBr(g) → C,H,Br(g) The bonding in the molecules is shown. H. H Br C: + H-Br H-Ć- -C-H H' H.
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...
Related questions
Concept explainers
Thermochemistry
Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.
Exergonic Reaction
The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.
Question
100%
![Use the molar bond enthalpy data in the table to estimate the value of ΔH°<sub>rxn</sub> for the equation
\[ \text{C}_2\text{H}_4(\text{g}) + \text{HBr}(\text{g}) \rightarrow \text{C}_2\text{H}_5\text{Br}(\text{g}) \]
The bonding in the molecules is shown.
**Diagram Explanation:**
- **Reactants:**
- Ethylene (C₂H₄) is shown with a carbon-carbon double bond. Each carbon is bonded to two hydrogen atoms.
- Hydrogen bromide (HBr) is shown with a single bond between hydrogen and bromine.
- **Products:**
- Ethyl bromide (C₂H₅Br) is shown with a carbon-carbon single bond. The first carbon is bonded to three hydrogens, and the second carbon is bonded to two hydrogens and one bromine.
The reaction involves breaking the C=C double bond in ethylene and the H–Br bond, and forming new C–C, C–H, and C–Br bonds in ethyl bromide. Use the given bond enthalpy values to calculate the reaction enthalpy change.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F28113ec2-37ac-45d1-a0e9-7ed3588453b7%2F94bf76bb-c07c-469c-ad9a-b93173219c2b%2Fe0d1o2e_processed.png&w=3840&q=75)
Transcribed Image Text:Use the molar bond enthalpy data in the table to estimate the value of ΔH°<sub>rxn</sub> for the equation
\[ \text{C}_2\text{H}_4(\text{g}) + \text{HBr}(\text{g}) \rightarrow \text{C}_2\text{H}_5\text{Br}(\text{g}) \]
The bonding in the molecules is shown.
**Diagram Explanation:**
- **Reactants:**
- Ethylene (C₂H₄) is shown with a carbon-carbon double bond. Each carbon is bonded to two hydrogen atoms.
- Hydrogen bromide (HBr) is shown with a single bond between hydrogen and bromine.
- **Products:**
- Ethyl bromide (C₂H₅Br) is shown with a carbon-carbon single bond. The first carbon is bonded to three hydrogens, and the second carbon is bonded to two hydrogens and one bromine.
The reaction involves breaking the C=C double bond in ethylene and the H–Br bond, and forming new C–C, C–H, and C–Br bonds in ethyl bromide. Use the given bond enthalpy values to calculate the reaction enthalpy change.
Transcribed Image Text:**Average Molar Bond Enthalpies (\(H_{\text{bond}}\))**
This table provides a list of average molar bond enthalpies for various chemical bonds, expressed in kilojoules per mole (\( \text{kJ} \cdot \text{mol}^{-1} \)).
| Bond | \( \text{kJ} \cdot \text{mol}^{-1} \) | Bond | \( \text{kJ} \cdot \text{mol}^{-1} \) |
|------|-----------------------|------|---------------------|
| O–H | 464 | C≡N | 890 |
| O–O | 142 | N–H | 390 |
| C–O | 351 | N–N | 159 |
| O=O | 502 | N=N | 418 |
| C=O | 730 | N≡N | 945 |
| C–C | 347 | F–F | 155 |
| C=C | 615 | Cl–Cl| 243 |
| C≡C | 811 | Br–Br| 192 |
| C–H | 414 | H–H | 435 |
| C–F | 439 | H–F | 565 |
| C–Cl | 331 | H–Cl | 431 |
| C–Br | 276 | H–Br | 368 |
| C–N | 293 | H–S | 364 |
| C=N | 615 | S–S | 225 |
**Explanation:**
- The table contains two columns of bond types, each paired with their respective bond enthalpies.
- Bond enthalpy, or bond dissociation energy, is the energy required to break one mole of bonds in a gaseous substance.
- Higher bond enthalpies indicate stronger bonds, as they require more energy to break.
- For example, the bond enthalpy of a nitrogen triple bond (N≡N) is 945 kJ/mol, which is much stronger than that of a nitrogen single bond (N–N) at 159 kJ/mol
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution!
Trending now
This is a popular solution!
Step by step
Solved in 2 steps with 2 images
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Recommended textbooks for you
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY