Question

The average C - H bond energy in CH4 is 415 kJ / mol. Use the following data to calculate the average C - H bond energy in ethane ( C2H6;C - C bond ) , in ethane ( C2H4;C C bond ) , and in ethyne ( C2H2;C C bond ) .

C2H6 ( g ) + H2 ( g ) rightarrow 2CH4 ( g ) delta H*rxn = - 65.07 kj / mol
C2H4 ( g ) + H2 ( g ) rightarrow 2CH4 ( g ) delta H* = - 202.21kJ / mol
C2H2 ( g ) + 3H2 ( g ) rightarrow 2 CH4 ( g ) delta H* = - 376.74kj / mol

Average C - H bond Average C - H bond energy in ethane = kJ / mol energy in ethane = kj / mol Average C - H bond energy in ethyne = kJ / mol

Answer 1

Answer and Explanation:

ΔH = (Bond energies of the products) - (Bond Energies of the reactants)

a) C2H6 + H2 ----> 2CH4 ΔH = -65.07 KJ/mol

Bond energy of product = 2×Bond energy of CH4 =2 × (4 (C-H)) =2 × 4 × 415 = 3320 KJ/mol

Bond energy of reactants = Bond energy of C2H6 + Bond energy of H2

Bond energy of C2H6 = (C-C) + 6(C-H) = 347 + 6(C-H)

Bond energy of H2 = (H-H) = 432 KJ/mol

-65.07 = 3320 - (Bond energy of C2H6 + 432)

Bond energy of C2H6 = 3320-432+65.07 = 2953.07 KJ/mol

Bond energy of C2H6 = (C-C) + 6(C-H) = 347 + 6(C-H) = 2953.07

(C-H) = (2953.07 -347)/6 = 434.345 KJ/mol

b) C2H4 + 2H2 ------> CH4 ΔH = -202.21 KJ/mol

Bond energy of product = 2×Bond energy of CH4 =2 × (4 (C-H)) =2 × 4 × 415 = 3320 KJ/mol

Bond energy of reactants = Bond energy of C2H4 + (2 × Bond energy of H2)

Bond energy of C2H4 = (C=C) + 4(C-H) = 614 + 4(C-H)

(2 × Bond energy of H2) = 2 × 432 = 864 KJ/mol

-202.21 = 3320 - (Bond energy of C2H4 + 864)

Bond energy of C2H4 = 3320+202.21-864 = 2658.1 KJ/mol

Bond energy of C2H4 = (C=C) + 4(C-H) = 614 + 4(C-H) = 2658.1

(C-H) = (2658.1 - 614)/4 = 511.05 KJ/mol

c) C2H2 + 3H2 ------> 2CH4 ΔH = -376.74 KJ/mol

Bond energy of product = 2×Bond energy of CH4 =2 × (4 (C-H)) =2 × 4 × 415 = 3320 KJ/mol

Bond energy of reactants = Bond energy of C2H2 + (3 × Bond energy of H2)

Bond energy of C2H = (triple bond Carbon to Carbon) + 2(C-H) = 839 + 2(C-H)

(3 × Bond energy of H2) = 3 × 432 = 1296 KJ/mol

-376.74 = 3320 - (Bond energy of C2H2 + 1296)

Bond energy of C2H2 = 3320+376.74-1296 = 2400.74 KJ/mol

Bond energy of C2H2 = (triple bond Carbon to Carbon) + 2(C-H) = 839 + 2(C-H) = 2400.74

(C-H) = (2400.74 - 839)/2 = 780.87 KJ/mol

QED!!!

Answer 2

The bond energy of C-H bond in ethane is 434.345 kJ/mol, ethene is 511.05 kJ/mol, and ethyne is 780.87 kJ/mol.

The bond energy can be given by:

• C-H bond energy in Ethane:

$\Delta$H = energy of reactant - the energy of the product

$\Delta$H = {(C-C) + 6 (C-H)} - {2(4 (C-H))}

65.07 = {347 + 6(C-H)} - 3320

Bond energy of $\rm C_2H_6$ = (C-C) + 6(C-H)

2953.07 = 347 + 6(C-H)

C-H bond in ethane = 434.345 kJ/mol.

• C-H bond energy in Ethene:

$\Delta$H = Bond energy of $\rm C_2H_4$ + (2 $\times$ Bond energy of $\rm H_2$) - 2 $\times$ Bond energy of $\rm CH_4$

$\Delta$H = C=C + 4(C-H) + 2(432) - 2 (4(C-H))

-202.21 kJ/mol = 614 + 4(C-H) + 864 - 3320 kJ/mol

C-H bond = 511.05 kJ/mol

• C-H bond energy in Ethyne:

$\Delta$H = 2 (4(C-H)) - Bond energy of $\rm C_2H_2$ + (3 $\times$ Bond energy of $\rm H_2$)

$\Delta$H = 2 (4(415)) - C=C + 2(C-H) + 3(432) kJ/mol

-376.74 = 3320 - 839 + 2(C-H) + 1296 kJ/mol

C-H bond = 780.87 kJ/mol.

For more information about bond energy, refer to the link:

https://brainly.com/question/24805752