C2H2(g) + 2 H2(g)--> C2H6(g)

Bond Bond Energy (kJ/mol)
C-C 347
C=C 611
C-H 414
H-H 436
Calculate the value of the C C (triple bond) energy in C2H2 in kJ/mole.

It appears to me that one needs the delta H for the reaction. Perhaps another tutor will see it differently.

- 311.4 kJ = [(2) (436) + E* + (2) (414)] - [(347) + (6) (414)]

E* = 820 kJ

To calculate the value of the C-C (triple bond) energy in C2H2, we need to consider the overall reaction:

C2H2(g) + 2 H2(g) --> C2H6(g)

Given that the C-H bond energy is 414 kJ/mol and the H-H bond energy is 436 kJ/mol, we can subtract the bond energies of the products from the reactants to find the overall change in energy.

For the reactants:
C2H2(g) has 1 C-C triple bond and 2 C-H bonds, so the energy required to break these bonds is:
(1 x C-C bond energy) + (2 x C-H bond energy) = (1 x 347 kJ/mol) + (2 x 414 kJ/mol) = 1175 kJ/mol.

For the products:
C2H6(g) has 3 C-C single bonds and 6 C-H bonds, so the energy released when these bonds are formed is:
(3 x C-C bond energy) + (6 x C-H bond energy) = (3 x 347 kJ/mol) + (6 x 414 kJ/mol) = 3648 kJ/mol.

Now, we can calculate the energy change (ΔH) for the overall reaction:
ΔH = (energy of products) - (energy of reactants) = 3648 kJ/mol - 1175 kJ/mol = 2473 kJ/mol.

Since the reaction is exothermic, the energy value we just calculated represents the energy released when the reaction occurs.

Therefore, the value of the C-C (triple bond) energy in C2H2 is 2473 kJ/mol.

To calculate the value of the C-C (triple bond) energy in C2H2, we need to recognize that a triple bond consists of one sigma bond and two pi bonds.

The first step is to understand that the overall reaction equation involves the breaking of one C-C triple bond in C2H2 and the formation of two C-C single bonds in C2H6.

The energy change for this reaction can be calculated using the bond energy values provided.

Given:
C-C (single bond) energy = 347 kJ/mol
C=C (double bond) energy = 611 kJ/mol
C-H (bond) energy = 414 kJ/mol

We need to determine the energy change for breaking two C-C single bonds (2 x C-C) and forming one C=C double bond in C2H2, and forming two C-C single bonds in C2H6.

Breaking two C-C single bonds (2 x C-C):
Energy change = 2 x C-C energy = 2 x 347 kJ/mol = 694 kJ/mol

Forming one C=C double bond in C2H2:
Energy change = -1 x C=C energy = -1 x 611 kJ/mol = -611 kJ/mol

Forming two C-C single bonds in C2H6:
Energy change = 2 x C-C energy = 2 x 347 kJ/mol = 694 kJ/mol

Now, let's sum up the energy changes:
Energy change = (694 kJ/mol) + (-611 kJ/mol) + (694 kJ/mol) = 777 kJ/mol

Therefore, the value of the C-C (triple bond) energy in C2H2 is 777 kJ/mol.