Average Bond Energies (kJ/mol) egin{tabular}{|cllllc|} hline ( mathrm{H}-mathrm{H} ) & ( 436 mathrm{~kJ} / mathrm{mol} ) & ( mathrm{C}-mathrm{H} ) & ( 413 mathrm{~kJ} / mathrm{mol} ) & ( mathrm{C}=mathrm{C} ) & ( 614 mathrm{~kJ} / mathrm{mol} ) \ ( mathrm{H}-mathrm{Cl} ) & ( 431 mathrm{~kJ} / mathrm{mol} ) & ( mathrm{C}-mathrm{C} ) & ( 348 mathrm{~kJ} / mathrm{mol} ) & ( mathrm{C}=mathrm{C} ) & ( 839 mathrm{~kJ} / mathrm{mol} ) \ ( mathrm{H}-mathrm{F} ) & ( 567 mathrm{~kJ} / mathrm{mol} ) & ( mathrm{C}-mathrm{N} ) & ( 293 mathrm{~kJ} / mathrm{mol} ) & ( mathrm{C}=mathrm{O} ) & ( 799 mathrm{~kJ} / mathrm{mol} ) \ ( mathrm{N}-mathrm{H} ) & ( 391 mathrm{~kJ} / mathrm{mol} ) & ( mathrm{C}-mathrm{O} ) & ( 358 mathrm{~kJ} / mathrm{mol} ) & ( mathrm{O}=mathrm{O} ) & ( 495 mathrm{~kJ} / mathrm{mol} ) \ ( mathrm{N}-mathrm{O} ) & ( 201 mathrm{~kJ} / mathrm{mol} ) & ( mathrm{C}-mathrm{F} ) & ( 485 mathrm{~kJ} / mathrm{mol} ) & ( mathrm{C}=mathrm{O} ) & ( 1072 mathrm{~kJ} / mathrm{mol} ) \ ( mathrm{O}-mathrm{H} ) & ( 463 mathrm{~kJ} / mathrm{mol} ) & ( mathrm{C}-mathrm{Cl} ) & ( 328 mathrm{~kJ} / mathrm{mol} ) & ( mathrm{C}=mathrm{N} ) & ( 615 mathrm{~kJ} / mathrm{mol} ) \ ( mathrm{O}-mathrm{O} ) & ( 146 mathrm{~kJ} / mathrm{mol} ) & ( mathrm{C}-mathrm{S} ) & ( 259 mathrm{~kJ} / mathrm{mol} ) & ( mathrm{N}=mathrm{N} ) & ( 418 mathrm{~kJ} / mathrm{mol} ) \ ( mathrm{F}-mathrm{F} ) & ( 155 mathrm{~kJ} / mathrm{mol} ) & ( mathrm{Cl}-mathrm{Cl} ) & ( 242 mathrm{~kJ} / mathrm{mol} ) & ( mathrm{N}=mathrm{N} ) & ( 941 mathrm{~kJ} / mathrm{mol} ) \ & & & & ( mathrm{C}=mathrm{N} ) & ( 891 mathrm{~kJ} / mathrm{mol} ) \ hline end{tabular} Estimate the enthalpy change ( left(Delta H_{mathrm{rxn}} ight) ) of the following reactions using the bond energies above. [ underset{egin{array}{l} mathrm{H} \ mathrm{H} \ mathrm{H} end{array}}{stackrel{mathrm{H}}{mathrm{H}}-mathrm{H}}+underset{mathrm{O}=mathrm{O}}{mathrm{O}}=mathrm{O} ightarrow mathrm{O}=mathrm{C}=mathrm{O}+egin{array}{r} mathrm{H}-mathrm{O}-mathrm{H} \ mathrm{H}-mathrm{O}-mathrm{H} end{array} ] ( mathrm{HCN}(g)+2 mathrm{H}_{2}(g) quad->quad mathrm{CH}_{3} mathrm{NH}_{2}(g) )
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The bonds formed are 2 C=O bonds and 4 O-H bonds. Using the bond energies from the table: Energy required to break bonds = (4 * 436 kJ/mol) + (1 * 495 kJ/mol) = 2249 kJ/mol Energy released when bonds are formed = (2 * 799 kJ/mol) + (4 * 463 kJ/mol) = 3198 Show more…
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Common bond energies The table below lists the average bond energies that you would need to determine reaction enthalpies. Bond Bond energy (kJ/mol) Bond Bond energy (kJ/mol) C-C 347 C-H 414 H-H 436 C-O 360 N=N 418 N-H 389 N≡N 946 O-H 464 O=O 498 C=O 799* * Bond energy in CO2. Part B Use bond energies to calculate the enthalpy of combustion of methanol in kJ/mol. Express your answer in kilojoules per mole as an integer. ΔHrxn = kJ/mol
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Average Bond Enthalpy (kJ/mol): 413, 495, 799, 463 Bond: C-H, O=O, C=O, O-H Use the bond enthalpies in the table above to estimate ΔH for the following reaction: H H-C-H + 2 O=O → O=C=O + 2 H-O-H H -377 kJ -808 kJ 2170 kJ -354 kJ -2831 kJ 1244 kJ
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The table below lists the average bond energies that you would need to determine reaction enthalpies. Bond Bond energy (kJ/mol) C−C 347 C−H 414 H−H 436 C−O 360 N=N 418 N−H 389 N≡N 946 O−H 464 O=O 498 C=O 799* * Bond energy in CO2. Use bond energies to calculate the enthalpy of combustion of one mole of methanol in kJ per mole of methanol. Express your answer in kilojoules as an integer. Use bond energies to calculate ΔHrxn for the following reaction: N2(g) + 3H2(g) → 2NH3(g) Express your answer in kilojoules as an integer.
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