McQuarrie Rock Gallogly presented by Macmillan Learning Use the molar bond enthalpy data in the table to estimate the Bond kJ mol-1 Bond kJ mol-1 value of AHn for the equation. O-H 464 C=N 890 0-0 142 N-H 390 NH, (g) + 20,(g) HNO,(g) + H,O(g) С-О 351 N-O 201 The bonding in the molecules is shown. O=0 502 N=N 418 O=O C=0 730 N=O 607 С-С 347 F-F 155 С-С 615 Cl-CI 243 C=C 811 Br-Br 192 С-Н 414 Н-Н 435 С-F 439 Н-F 565 331 H-Cl 431 Cr-Cl С-Br 276 Н-Br 368 С-N 293 H-S 364 615 S-S 225 C=N kJ-mol-! AHxn = Question Source: MRG - General Chemistry Pubisher: U
McQuarrie Rock Gallogly presented by Macmillan Learning Use the molar bond enthalpy data in the table to estimate the Bond kJ mol-1 Bond kJ mol-1 value of AHn for the equation. O-H 464 C=N 890 0-0 142 N-H 390 NH, (g) + 20,(g) HNO,(g) + H,O(g) С-О 351 N-O 201 The bonding in the molecules is shown. O=0 502 N=N 418 O=O C=0 730 N=O 607 С-С 347 F-F 155 С-С 615 Cl-CI 243 C=C 811 Br-Br 192 С-Н 414 Н-Н 435 С-F 439 Н-F 565 331 H-Cl 431 Cr-Cl С-Br 276 Н-Br 368 С-N 293 H-S 364 615 S-S 225 C=N kJ-mol-! AHxn = Question Source: MRG - General Chemistry Pubisher: U
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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![### Estimating the Enthalpy Change of Reaction (\(\Delta H_{\text{rxn}}\))
**Objective:** Use the molar bond enthalpy data in the table to estimate the value of \(\Delta H_{\text{rxn}}\) for the given chemical equation.
**Chemical Equation:**
\[
\text{NH}_3(g) + 2 \text{O}_2(g) \rightarrow \text{HNO}_3(g) + \text{H}_2\text{O}(g)
\]
**Molecular Bonding Diagrams:**
- **Reactants:**
- \(\text{NH}_3\): Displays three N-H bonds.
- \(\text{O}_2\): Exhibits a double bond (O=O).
- **Products:**
- \(\text{HNO}_3\): Contains N=O, N-O, and O-H bonds.
- \(\text{H}_2\text{O}\): Shows two O-H bonds.
**Bond Enthalpy Table:**
| Bond | kJ·mol\(^{-1}\) | Bond | kJ·mol\(^{-1}\) |
|--------|----------------|-------|----------------|
| O–H | 464 | C≡N | 890 |
| O=O | 142 | N–H | 390 |
| C=O | 351 | N–O | 201 |
| O–O | 502 | N≡N | 418 |
| C≡O | 730 | O=O | 607 |
| 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 |](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F78ccc9d3-408e-4529-84dd-3dc261702da6%2F652b6305-c14b-4266-b53a-2de9da6bfe2a%2Fvft2ekt_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Estimating the Enthalpy Change of Reaction (\(\Delta H_{\text{rxn}}\))
**Objective:** Use the molar bond enthalpy data in the table to estimate the value of \(\Delta H_{\text{rxn}}\) for the given chemical equation.
**Chemical Equation:**
\[
\text{NH}_3(g) + 2 \text{O}_2(g) \rightarrow \text{HNO}_3(g) + \text{H}_2\text{O}(g)
\]
**Molecular Bonding Diagrams:**
- **Reactants:**
- \(\text{NH}_3\): Displays three N-H bonds.
- \(\text{O}_2\): Exhibits a double bond (O=O).
- **Products:**
- \(\text{HNO}_3\): Contains N=O, N-O, and O-H bonds.
- \(\text{H}_2\text{O}\): Shows two O-H bonds.
**Bond Enthalpy Table:**
| Bond | kJ·mol\(^{-1}\) | Bond | kJ·mol\(^{-1}\) |
|--------|----------------|-------|----------------|
| O–H | 464 | C≡N | 890 |
| O=O | 142 | N–H | 390 |
| C=O | 351 | N–O | 201 |
| O–O | 502 | N≡N | 418 |
| C≡O | 730 | O=O | 607 |
| 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 |
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