O 11/7/2016 11:00 PM A 00 11/5/2016 09:59 PM Gradebook Print Calculator Periodic

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O 11/7/2016 11:00 PM A 00 11/5/2016 09:59 PM Gradebook Print Calculator Periodic Table Question 2 of 35 Sapling Learning macmillan learning Bromination of isobutane is a two-step reaction, as shown below. Using the table of bond dissociation energies below, calculate the enthalpy of each step and the enthalpy of the overall reaction Number CH3 CH3 H-Ein Ana- kJ mol H3C-C-H Step 1 Br CH3 CH3 Number CH3 CH3 Step 2 H3C-C. kJ mol H3C-C-Br AH Br Br-Br CH3 CH3 Number CH3 CH3 Overall Hac-C-H Br Br H3C- Br H-Br reaction kJ mol AH CH3 CH3 Bond broken ANH, kJ/mol H-H 436 Bond dissociation energies for Br-Br 194 A- B A+ B 366 H-Br are shown here (CH3) 3C-H 400 (CH3)3C- Br 292 Previous X Give Up & View Solution Check Answer Next Exit Hint

Explanation / Answer

step 1:
delta H = E (bond broken) - E (bond formed)
= 400 - 366
= 34 KJ/mol

step 2:
delta H = E (bond broken) - E (bond formed)
= 194 - 292
= -98 KJ/mol

overall:
delta H = delta H1 + delta H2
= 34 -98
= -64 KJ/mol

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