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Hydrogenation reactions are used to add hydrogen across double bonds in hydrocarbons and other organic compounds. use average bond energies to calculate δhrxn for the hydrogenation reaction.

Respuesta :

H2(g) +C2H4(g)→C2H6(g)
H-H +H2C =CH2→H3C-Ch3
2C -H bonds and one C-C bond are formed while enthalpy change (dH) of the reaction,
H-H: 432kJ/mol
C=C: 614kJ/mol
C-C: 413 kJ/mol
C-C: 347 kJ/mol
dH is equal to sum of the energies released during the formation of new bonds or negative sign, and sum of energies required to break old bonds or positive sign.
The bond which breaks energy is positive.
432+614 =1046kJ/mol
Formation of bond energy is negative
2(413) + 347 = 1173 kJ/mol
dH reaction is -1173 + 1046 =-127kJ/mol 
adefioyelaoye

The average bond energies to calculate δhrxn for the hydrogenation

reaction is -127kJ/mol.

What is Hydrogenation?

This is the reaction which involves the addition of Hydrogen to other

elements or compounds.

H₂(g) +C₂H₄(g)→ C₂H₆(g)

H-H +H₂C =CH₂→ H₃C-CH₃

2C-H bonds and 1 C-C bond are formed in the process.

Parameters for Enthalpy change (dH)

H-H: 432kJ/mol

C=C: 614kJ/mol

C-C: 413 kJ/mol

C-C: 347 kJ/mol

dH = sum of the energies released during the formation of new bonds(-) + sum of energies required to break old bonds(+).

Sum of energies required to break old bonds(+).

432+614 =1046 kJ/mol.

Sum of the energies released during the formation of new bonds(-)

2(413) + 347 = 1173 kJ/mol.

dH reaction = -1173 + 1046 = -127kJ/mol

Read more about Hydrogenation here https://brainly.com/question/1381520

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