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
Using the table of bond energies below, the delta H for the reaction is? H2C =...
Using the table of average bond enthalpies, what is the ∆H for the following gas phase reaction (in kJ/mol)? Bond Ave. Bond Enthalpy (kJ/mol) C – C 348 C = C 614 C ≡ C 839 C – H 413 C – Br 276 H – Br 366 H – H 436 a - 304 b + 304 c - 2134 d - 57 e + 3292
6 2 attempts left Check my work 6.66 points Enter your answer in the provided box. Sports trainers treat sprains and soreness with ethyl bromide. It is manufactured by reacting ethylene with hydrogen bromide: 11 + H- Print H References Use bond energies to find the enthalpy change for this reaction. kJ Average Bond Energies Bond Bond Enthalpy (kJ/mol) 432 C-c 347 614 cuc 839 CH 413 C-Br 276 Br-Br 193 H-Br 363
Using the bond energies from the table below estimate ∆H for the following reaction C2H2(g) + H2(g) → C2H4(g) C-H (413), H-H (436), C-C (348), C=C (614), C≡C (839) A) +165 kJ/mol B) -390. kJ/mol C) +390. kJ/mol D) –124 kJ/mol E) –165 kJ/mol
Using the table of average bond energies below, the AH for the reaction is k], C=0(g) + 2H2(g) → H3C-0-Hg) Bond: C-0 C=0 C=0 D(kJ/mol): 358 799 1072 C-H 413 H-H 436 O-H 463 -116 -276 +116 +276
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:
Use the bond enthalpy data given to estimate the enthalpy of reaction for the addition of HBr to acetylene gas, C2H2 to form C2H4Br2 (with the condensed structural formula Br-CH2-CH2-Br ) at 25°C. BE(C-C) = 348 kJ/mol; BE(CC triple bond) = 839 kJ/mol; BE(C-H) = 413 kJ/mol; BE(H-Br) = 366 kJ/mol; BE(C-Br) = 276 kJ/mol -581 kJ/mol -4949 kJ/mol +155 kJ/mol -887 kJ/mol +887 kJ/mol
Please show work! I've tried this problem a few times, but seem to be going wrong somewhere. The answer should be 366 kJ/mol, but I do not understand how to arrive at that solution. Thank you! a.) AHxn for the reaction below was determined using bond dissociation energies (BDEs) to be -57 kJ Using the table of BDE below, find the bond energy for H-Br c-C НН НН H-C-C-Br НН + H-Br Bond C-C с-с C-H C-Br H-Br Bond Enthalpy...
Use bond enthalpies (in kJ/mol): C-C 348 C=C 614 C≡C 839 H-H 436 C-H 413 O-H 463 C-O 358 C=O 799 to estimate ΔH for the reaction H2C=CH–CH2–OH (g) = > HC≡C–CH=O(g) + 2 H2(g)
Using the table of average bond energies below, the AH for the reaction is kJ. нн H-CEC-H(g) 2HI (g) I-CC-I(g) нн Bond: CECC-C H-1 C-IC-H D (kJ/mol): 839 348 299 240 413 -63 -160 +160 +63 -217 B. Are the following statements true or false? Consider the hypothetical molecule B A Drag the appropriate statements to their respective bins. Help Reset If resonance was important, the molecule would have identical A bond lengths. This molecule cannot exist true false
Using the table of bond energies below, calculate the following enthalpy values associated with this reaction: Co2 (g)2 H20 (g) CH4 (g)+2 02 (8) Bond type Bond Energy (kJ/mol) C-C 347 C=C 614 C-H 413 O-O 204 498 O=O 358 C-O C=O 799 H-O 467 Enter your answers to zero decimal places. Ignore significant figure rules. Include negative signs if necessary. What is the sum of the reactant bond enthalpies? kJ What is the sum of the product bond enthalpies?...