Chemistry
Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Question

Use the molar bond enthalpy data in the table to estimate the value of Delta H°rxn for the equation:

CCI4(g) + 2 F2(g) = CF4(g) + 2 Cl2(g) 

 

**Bond Enthalpy Calculation for Reaction** ### Reaction Equation: To estimate the value of the enthalpy change (\( \Delta H_{\text{rxn}} \)) for the reaction: \[ \text{CCl}_4 (g) + 2 \text{F}_2 (g) \rightarrow \text{CF}_4 (g) + 2 \text{Cl}_2 (g) \] ### Molecular Structures: - **CCl\(_4\):** A central carbon atom bonded to four chlorine atoms. - **F\(_2\):** Two fluorine atoms bonded together. - **CF\(_4\):** A central carbon atom bonded to four fluorine atoms. - **Cl\(_2\):** Two chlorine atoms bonded together. ### Table of Average Molar Bond Enthalpies (\(H_{\text{bond}}\)): | **Bond** | **kJ·mol\(^{-1}\)** | **Bond** | **kJ·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 | ### Explanation for Educational Purpose: This setup allows students to calculate the reaction enthalpy by considering the bonds broken and formed during the chemical
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Transcribed Image Text:**Bond Enthalpy Calculation for Reaction** ### Reaction Equation: To estimate the value of the enthalpy change (\( \Delta H_{\text{rxn}} \)) for the reaction: \[ \text{CCl}_4 (g) + 2 \text{F}_2 (g) \rightarrow \text{CF}_4 (g) + 2 \text{Cl}_2 (g) \] ### Molecular Structures: - **CCl\(_4\):** A central carbon atom bonded to four chlorine atoms. - **F\(_2\):** Two fluorine atoms bonded together. - **CF\(_4\):** A central carbon atom bonded to four fluorine atoms. - **Cl\(_2\):** Two chlorine atoms bonded together. ### Table of Average Molar Bond Enthalpies (\(H_{\text{bond}}\)): | **Bond** | **kJ·mol\(^{-1}\)** | **Bond** | **kJ·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 | ### Explanation for Educational Purpose: This setup allows students to calculate the reaction enthalpy by considering the bonds broken and formed during the chemical
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