Use the molar bond enthalpy data in the table to estimate the value of ΔH°rxn 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. **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

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Answered: Use the molar bond enthalpy data in the…

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...

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