Monofluorination of methane is
H3C-H + F-F ------------> H3C-F + H-F
ΔHo = BDE of reactants - BDE of products [ BDE = Bond dissociation energy]
= BDE of [ H3C-H + F-F] - BDE [ H3C-F + H-F]
= 105 kcal/mol + 38 kcal/mol - [ 110 kcal/mol + 136 kcal/mol]
= -103 kcal/mol
Therefore,
ΔHo = -103 kcal/mol
Use the bond dissociation energies listed below to calculate the Delta H degree for the halogenations...
Given the following: O2 (g) + 2F2 (g)------> 2OF2 (g) delta H=+24.5 kJ/mol Bond dissociation energies: F2= 159 kJ/mol; O2 (double bond) = 498 kJ/mol Calculate the bond strength of the O-F bonds in OF2.
Calculate the enthalpy for the reaction below using the following bond dissociation energies. • H-H 436 kJ/mol O-H 460 kJ/mol 0-0 180 kJ/mol • 0=0 498 kJ/mol H -774 kJ/mol -654 kJ/mol 654 kJ/mol 774 kJ/mol
1. Bond Dissociation Energies and Free Radicals Bond Bond Dissociation Energies (kJ/mol) Bond BDE Bond BDE (kJ/mol) (kJ/mol) H-H 436 CH3-H 439 H-F 570 CH3CH2-H 432 H-CI 432 (CH3CH2 413 BDE Bond (kJ/mol) 10-N 350 0-0 180 F-F O-H 0-C O-F 460 BDE (kJ/mol) | 200 180 159 | H-Br H-I 366 298 404 350 O-C1200 O-Br (CH3)3C-H C-C (sigma) C=C(pi) 210 C1-C1243 Br-Br 193 243 0 -I 220 I-I | 151 A. The enzyme methane monooxygenase catalyzes a remarkably...
8.10 Explain the value of bond dissociation energies and use bond dissociation energies in calculations 1. Explain how bond dissociation energies are used to determine the enthalpy change in a reaction. 2. Understand the limitations of using average bond dissociation energy values. 3. Calculate reaction enthalpies from bond dissociation energies
H2C=CH2 + CI H2C=CH + HCI Use the table of bond dissociation energies above to calculate AH for this reaction, the first step in the free radical chlorination of ethene. Table of Bond Dissociation Enthalpies Bond BDE (kJ/mol) H2C=CH-H 464 H-I 297 H-Br 368 H-C1 431 H-F 568 ΔΗ: kJ/mol This reaction is:
Shown below is an alternative mechanism for the photochemical chain radical chlorination of methane: Cl_2 + CH_4 right arrow CH_3CI + HCL Step 1 (initiation): CI_2 right arrow 2CI- Step 2 (propagation, part 1): CI +CH_4 right arrow CH_3CI + H Step 3 (propagation, part 2): H + CI_2 right arrow HCI +CI. Using the data provided below(bond dissociation energies, BDE), calculate delta Hdegree for each of the two propagation steps of the alternative mechanism. BDE: C-H bond, 104kcal/mol; C-Cl...
Question 1a. (0.5 point) Consider the bond dissociation energies listed below in kcal/mol CH3 – Br 70 CH3CH2 – Br 68 (CH3)2CH – Br 68 (CH3)3C – Br 65 These data show that the carbon–bromine bond is weakest when bromine is bound to a ____. a) methyl carbon b) primary carbon c) secondary carbon d) tertiary carbon e) quaternary carbon 1b. Predict the product for the halogenation reaction given below when methyl cyclohexane is subjected to free radical bromination Br2...
7. Calculate the AHRxn for the following transformation. A table of bond dissociation energies is provided below. All work must be shown for partial credit. (8 pts.) hv Br + Br-Br + HBr: Table of Selected Homolytic Bond Dissociation Energies. Bond Broken (CH3)3C-H (CH3)2CH-H Br-Br H-Br CH3CH2-H (CH3)3C-Br (CH3)2CH-Br CH3CH2-Br kJ/mol 400 413 193 366 421 292 298 295
Use deltaH and S to calculate DeltaG rxn...
Use Delta H degree_f and S degree to calculate Delta G degree rxn (Delta G degree sys) at 25 C for the reaction below: 4 KClO3 (s) rightarrow 3 KClO4 (s) + KCl (s) Delta H degree_f KClO3 = -397.7 kJ/mol; KClO4 = -432.8 kJ/mol; KCl = -436.7 kJ/mol S degree KClO3 = 143.1 kJ/mol; KClO4 = 151.0 kJ/mol; KCl = 82.6 kJ/mol
Using the table of bond energies below, the delta H for the reaction is? H2C = CH2 + H-Br -> H3C - CH2Br This is ethylene plus hydrogen going to ethyl bromide. Bond C-C C = C C - H H - Br C - Br D (kj/mol) 348 614 413 366 276 SHOW WORK