Acetylene Welding Torch
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Acetylene gas (C2H2) burns with oxygen in an oxyacetylene torch to produce carbon dioxide, water vapor, and th?
Acetylene gas (C2H2) burns with oxygen in an oxyacetylene torch to produce carbon dioxide, water vapor, and the great heat needed for welding metals. The heat of combustion of acetylene is -1259 kJ/mol. Estimate the bond energy of the carbon-carbon triple bond in acetylene. You might need to know some of the following:
C=O 799 kJ/mol
C-H 414 kJ/mol
O-H 464 kJ/mol
C-C 347 kJ/mol
C=C 611 kJ/mol
O=O 498 kJ/mol
The combustion reaction of one mole of acetylene is given by:
C₂H₂ + (5/2) O₂ → H₂O + 2 CO₂ , ∆H = -1259 kJ/mol
To get an integer values for stochiometric coefficients (and number of bonds) consider the combustion of 2 moles of acetylene:
2 C₂H₂ + 5 O₂ → 2 H₂O + 4 CO₂ , ∆H = -2518 kJ/mol
The bond energy D is defined as the enthalpy change when the bond is cleaved. When you estimate the enthalpy change due to reaction from the bond energies, you need to sum up the bond energies of reactants (bonds are cleaved), and subtract the bond energies of the products (bonds are formed).
The bonds involved in this reaction are
C₂H₂ (H-C≡C-H) contains two H-C bonds and one C≡C bond
O₂ (O=O) contains one O=O
H₂O (H-O-H) contains two O-H bonds
CO₂ (O=C=O) contains two C=O bonds.
Hence,
∆H = 2∙( 2∙D(C-H) + D(C≡C)) + 5∙D(O=O)) - 2∙2∙D(O-H) - 4∙2∙D(C=O)
<=>
∆H = 4∙D(C-H) + 2∙D(C≡C) + 5∙D(O=O) - 4∙D(O-H) - 8∙D(C=O)
So the bond energy of the triple bond is
D(C≡C) = (1/2)∙( ∆H - 4∙D(C-H) - 5∙D(O=O) + 4∙D(O-H) + 8∙D(C=O))
= (1/2)∙(-2518kJ/mol - 4∙414kJ/mol - 5∙498kJ/mol + 4∙464kJ/mol + 8∙799kJ/mol)
= 792 kJ/mol
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