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nevsk [136]
3 years ago
15

Estimate ΔH for the reaction: C2H6(g) + Cl2(g)--> C2H5Cl(g) + HCl(g) given the following average bond energies (in kJ/mol): C

-C, 348 C-H, 414 CI-CI, 242 C-CI, 327 H-CI, 431 68 kJ/mol 344 kJ/mol +276 kJ/mol -102 kJ/mo 113 kJ/mol
Chemistry
1 answer:
Leno4ka [110]3 years ago
5 0

Explanation:

The reaction equation will be as follows.

    C_{2}H_{6}(g) + Cl_{2}(g) \rightarrow C_{2}H_{5}Cl(g) + HCl(g)

Using bond energies, expression for calculating the value of \Delta H is as follows.

    \Delta H = \sum B.E_{reactants} - \sum B.E_{products}

On reactant side, from C_{2}H_{6} number of bonds are as follows.

C-C bonds = 1

C-H bonds = 6

From Cl_{2}; Cl-Cl bonds = 1

On product side, from C_{2}H_{5}Cl number of bonds are as follows.

C-C bonds = 1

C-H bonds = 5

C-Cl bonds = 1

From HCl; H-Cl bonds = 1

Hence, using the bond energies we will calculate the enthalpy of reaction as follows.

  \Delta H = \sum B.E_{reactants} - \sum B.E_{products}

  =[(1 \times 348 kJ/mol) + (6 \times 414 kJ/mol) + (1 \times 242 kJ/mol)] - [(1 \times 348 kJ/mol) + (5 \times 414 kJ/mol) + (1 \times 327 kJ/mol) + (1 \times 431 kJ/mol)]            = -102 kJ/mol

Thus, we can conclude that change in enthalpy for the given reaction is -102 kJ/mol.

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