Asked by Anonymous
Using the bond entalpies ∆H:
C---C: 348kJ C=C: 612 kJ C—C (triple bond) : 960 kJ C---H: 412 kJ H---H: 436 kJ
Calculate the calculate the value of ∆H of reaction for
H2C=CH2(g) + H2(g) → CH3—CH3(g)
C---C: 348kJ C=C: 612 kJ C—C (triple bond) : 960 kJ C---H: 412 kJ H---H: 436 kJ
Calculate the calculate the value of ∆H of reaction for
H2C=CH2(g) + H2(g) → CH3—CH3(g)
Answers
Answered by
DrBob222
Delta H reaction = (sum bond energy reactants)-(sum bond energy products)
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