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13 Dec 2019

The average bond enthalpy for a C=C double bond is 614 kJ/mol and that of a C?C single bond is 348 kJ/mol. Estimate the energy needed to break only the ? bond of the double bond of 2-butene.

Express your answer numerically in joules per molecule.

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Related questions


The strength of common bonds in living organisms range from 300 to500 kJ/mol. for example single carbon-carbon bonds in organicmolecules have energies of about 348 kJ/mol. (That is the energyrequired to break a single carbon-carbon bond is 348kJ/mol).Calculate the minimum wavelength of light needed to break the C-Cbond, Could UV lamps be used to break the C-C bond?

Explanations, equations, and steps are appreciated! Thank you!

Use the table to answer questions about bond energies.

Bond Bond Energy (KJ/mol)
C—C 347
C=C 611
C-H 414
C-O 360
C=O 736
O-O 142
O=O 498
H-O 464


(i) Calculate the bond energy for breaking all the bonds in a moleof methane, CH4
Express your answer numerically in kilojoules per mole.

Change in Heat Ch4 ?=KJ/mol

(ii) Calculate the bond energy for breaking all the bonds in a moleof O2 molecules?
Express your answer numerically in kilojoules per mole.

Change in Heat O2 ? =KJ/mol

(iii) Calculate the bond energy for forming all the bonds in a moleof water molecules, H2O
Express your answer numerically in kilojoules per mole.

Change in Heat H2O =? KJ/mol

(iv) Calculate the bond energy for forming all the bonds in a moleof carbon dioxide, .

Express your answer numerically in kilojoules per mole.

Change in Heat CO2 =? KJ/mol

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