lkene a dow12-Yahoo Se). \\?. owu2 . Cengage Mail-stop 2330 x re east.cengagenow
ID: 1035414 • Letter: L
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lkene a dow12-Yahoo Se). ?. owu2 . Cengage Mail-stop 2330 x re east.cengagenow.com/ilm/takeAssignment/takeCovalentActivity.do?locator-assignment-take&takeAssignmentSessionlocator; assignment-take For the reaction below H2C=CH2 + a Determine whether the fom the table below reaction is energetically favorable at room temperature. Assume that &S-O; Calculate the gas phase enthalpy change using bond dissociation enthalpies at 25C Bond Bond Enthalpy Bond Enthalpy kJ (kcamol 439 (105) 422 (101 ) 376 (90) ?_N | 355 (85) -01385 (92) c-o(aldehyde)| 728 (174) ceo (CO2) 1803 (192) C-H (-CH) -ED |NEN 1075 (257) C--H (-CH2t 464 (111) ?C- | 238 (57) 50 (227) 966 (231) o498 (119 (111) c?1 238 (57) C--H (-CH)| 556 (133) - 301 (72) 1391 (93) 318 (76) 727 (174) Si--H Be anaze that the boed enengy for the CH bond varies considerably and may charge during the reaction therefoce, you nall fird veveral entries for C-H bonds in the table lisclude the algebraic siga and specify units, eg 45 lJmol. Calculate to the pearest single energ anit PiesiousExplanation / Answer
dHrxn = sum of B.E( reactants) - sum of B.E(products)
Sum of B.E(reactants) = ( 10*464 ) + (3*727) + (1*376) = 7197 kJ
Sum of B.E(products) = (8*422)+(2*464)+(5*376)+(1*727)= 6911 kJ
dHrxn = 7197 - 6911
dHrxn = 286 kJ
As dHrxn is positive and dS = 0, the reaction is non-spontaneous at room temperature.
Therefore, energetically the reaction is not favourable.
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