Use the given bond energy values to estimate ΔH for the following gas-phase reaction (see image attached) D-values in kJ/molDH-H = 432 DH-Br = 363 DH-C = 413DH-N = 391 DH-O = 467 DC-C = 347DC=C = 614 DC≡C = 839 DC-N = 305DC=N = 615 DC≡N = 891 DC-O = 358DC=O = 745 DC=O (CO2) = 799 DC≡O=1072DC-Br = 276 DN-N = 160. DN=N = 418DN≡N = 941 DO-O = 146 DO=O = 495DN-O = 201 DN=O = 607 DBr-Br = 193DC-Cl = 339 DH-Cl = 427 DCl-Cl = 239 (Simple energy units required for the answer.) H.H.Br -BrH -BrH.Н—С— нH-Br

Answer: Chemical reaction is a process in which breakage of old bonds and formation of new bonds…

Answered: H. H. Br -Br Н— Br H. H. H- -C H- H Br

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...

See similar textbooks

Similar questions

Use bond enthalpies in Table 5.4 to estimate ΔH for each ofthe following reactions:
Calculate the heat of the following reaction from the given bond energies. Give the answer to 3 significant figures. 2CH3CH3+7O2⟶4CO2+6H2O2CH3CH3+7O2⟶4CO2+6H2O Bond Energies C-H: 349 C-C: 270 O=O: 592 C=O: 695 O-H: 313
19 Hydrogenation of double and triple bonds is an important industrial process. Calculate (in kJ) the standard enthalpy change ΔH° for the hydrogenation of ethyne (acetylene) to ethane using average bond enthalpies (use exam data sheet values). H–C≡C–H(g) + 2H2(g) → H3C–CH3(g)
Using the following bond energies estimate the heat of combustion for one mole of acetylene (H-C≡C-H): C2H2(g) + 5/2O2(g) → 2CO2(g) + H2O(g) Bond Bond Energy (kJ/mol) C≡C 839 C-H 413 O=O 495 C=O 799 O-H 467 Group of answer choices 1228 kJ -1228 kJ -447 kJ +447 kJ +365 kJ
You are given the following average bond energies:H-H 436 kJ/molH-X 431 kJ/molH-C 414 kJ/molC-X 339 kJ/molX-X 243 kJ/molBalance the following chemical reaction and compute the estimated heat of reaction using the values above.CH4(g) + X2(g) → CH1X3(g) + HX (g)
The table below contains some mean bond energy data: Bond H—H C-C N≡N Mean bond energy /kJ mol–1 436 348 944 (i) Balance the equation below for the formation of one mole of ammonia, NH3, from its elements. N2 + H2 → NH3 DH = -38 kJmol-1 (ii) Use the data in the table above to calculate the bond energy of N – H bond in NH3 in the reaction given in (i) above. Comment on why the value obtained is referred to as ‘mean bond enthalpy’
Using bond dissociation energies predict the energy given off in the following reaction: C2H4 + O2 → CO2 + H2O a 444 kJ b 634 kJ c 246 kJ d 906 kJ
The bond dissociation energy to break 7 C-H bond(s) in 1 mole of propane (CH;CH;CH3) molecules is c N O Single H Bond H 432 411 346 N 386 305 167 459 358 201 142 C=C 602 C=O 799 C=C 835 C=O 1072 Multiple Bonds C=N 615 O=0 494 C=N 887 N=N 942 **All values in kJ/mol** kJ 1 2 3 4 5 C 7 8 9 +/- x 100 Tap here or pull up for additional resources LO
Calculate delta H for the reaction : Ch4+ 3Cl2= CHCl3+ 3HCl given: CH4 =-74.85(kJ/mol) HCl= -92.30(kJ/mol) CHCl3=-134.3 (kJ/mol) CHCl3=-103.2 (kJ/mol)

Recommended textbooks for you

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Organic Chemistry

Chemistry

ISBN:

9780078021558

Author:

Janice Gorzynski Smith Dr.

Publisher:

McGraw-Hill Education

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Elementary Principles of Chemical Processes, Bind…

Chemistry

ISBN:

9781118431221

Author:

Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard

Publisher:

WILEY

SEE MORE TEXTBOOKS

D_H-H = 432	D_H-Br = 363	D_H-C = 413
D_H-N = 391	D_H-O = 467	D_C-C = 347
D_C=C = 614	D_C≡C = 839	D_C-N = 305
D_C=N = 615	D_C≡N = 891	D_C-O = 358
D_C=O = 745	D_{C=O (CO2)} = 799	D_C≡O=1072
D_C-Br = 276	D_N-N = 160.	D_N=N = 418
D_N≡N = 941	D_O-O = 146	D_O=O = 495
D_N-O = 201	D_N=O = 607	D_Br-Br = 193
D_C-Cl = 339	D_H-Cl = 427	D_Cl-Cl = 239