Using bond energies provided below, calculate the AHrxn: Report answer to three significant figures without units and pay attention to the sign of enthalpy. The structure for C2H4 contains a C=C bond while the structure for C2H6 contains a C-C bond. C2H4(g) + H2(g) → C2H6g) C-C 347 kJ/mol C=C 611 kJ/mol C-H 414 kJ/mol H-H 436 kJ/mol
Using bond energies provided below, calculate the AHrxn: Report answer to three significant figures without units and pay attention to the sign of enthalpy. The structure for C2H4 contains a C=C bond while the structure for C2H6 contains a C-C bond. C2H4(g) + H2(g) → C2H6g) C-C 347 kJ/mol C=C 611 kJ/mol C-H 414 kJ/mol H-H 436 kJ/mol
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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![**Topic: Calculating Enthalpy Changes Using Bond Energies**
**Objective:**
Calculate the change in enthalpy (\( \Delta H_{\text{rxn}} \)) for the formation of ethane (\( \text{C}_2\text{H}_6 \)) from ethene (\( \text{C}_2\text{H}_4 \)) and hydrogen (\( \text{H}_2 \)) using bond energies.
**Introduction:**
For the reaction:
\[
\text{C}_2\text{H}_4(g) + \text{H}_2(g) \rightarrow \text{C}_2\text{H}_6(g)
\]
The structure of \( \text{C}_2\text{H}_4 \) includes a C=C bond, while \( \text{C}_2\text{H}_6 \) contains only C-C bonds.
**Bond Energy Data:**
- **C–C**: 347 kJ/mol
- **C=C**: 611 kJ/mol
- **C–H**: 414 kJ/mol
- **H–H**: 436 kJ/mol
**Instructions:**
1. **Break Bonds:** Calculate the energy required to break the bonds in the reactants.
- Break 1 C=C bond in \( \text{C}_2\text{H}_4 \).
- Break 1 H–H bond in \( \text{H}_2 \).
2. **Form Bonds:** Calculate the energy released in forming the bonds of the product.
- Form 1 C–C bond and 2 C–H bonds in \( \text{C}_2\text{H}_6 \).
3. **Calculate \( \Delta H_{\text{rxn}} \):**
\[
\Delta H_{\text{rxn}} = \text{(Energy required to break bonds)} - \text{(Energy released in forming bonds)}
\]
**Output:**
Provide the answer to three significant figures and ensure the correct sign for enthalpy change, indicating whether the reaction is endothermic or exothermic.
**Note:**
Emphasize the importance of using bond energies correctly and reporting the sign and magnitude accurately as this greatly affects the interpretation of chemical reactions in educational contexts.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F269cfda5-f8f7-4d34-b214-f5bad582f65d%2F3c2cffb6-8d9a-4d71-8c91-b8d84ac589a9%2Fjqaos1d_processed.png&w=3840&q=75)
Transcribed Image Text:**Topic: Calculating Enthalpy Changes Using Bond Energies**
**Objective:**
Calculate the change in enthalpy (\( \Delta H_{\text{rxn}} \)) for the formation of ethane (\( \text{C}_2\text{H}_6 \)) from ethene (\( \text{C}_2\text{H}_4 \)) and hydrogen (\( \text{H}_2 \)) using bond energies.
**Introduction:**
For the reaction:
\[
\text{C}_2\text{H}_4(g) + \text{H}_2(g) \rightarrow \text{C}_2\text{H}_6(g)
\]
The structure of \( \text{C}_2\text{H}_4 \) includes a C=C bond, while \( \text{C}_2\text{H}_6 \) contains only C-C bonds.
**Bond Energy Data:**
- **C–C**: 347 kJ/mol
- **C=C**: 611 kJ/mol
- **C–H**: 414 kJ/mol
- **H–H**: 436 kJ/mol
**Instructions:**
1. **Break Bonds:** Calculate the energy required to break the bonds in the reactants.
- Break 1 C=C bond in \( \text{C}_2\text{H}_4 \).
- Break 1 H–H bond in \( \text{H}_2 \).
2. **Form Bonds:** Calculate the energy released in forming the bonds of the product.
- Form 1 C–C bond and 2 C–H bonds in \( \text{C}_2\text{H}_6 \).
3. **Calculate \( \Delta H_{\text{rxn}} \):**
\[
\Delta H_{\text{rxn}} = \text{(Energy required to break bonds)} - \text{(Energy released in forming bonds)}
\]
**Output:**
Provide the answer to three significant figures and ensure the correct sign for enthalpy change, indicating whether the reaction is endothermic or exothermic.
**Note:**
Emphasize the importance of using bond energies correctly and reporting the sign and magnitude accurately as this greatly affects the interpretation of chemical reactions in educational contexts.
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