Using the bond energies provided below, calculate δh° for the reaction ch4 (g) + 4cl2 (g) → ccl4 (g) + 4hcl (g) bond energies: c-h = 413 kj/mol, cl-cl = 243 kj/mol, c-cl = 339 kj/mol, h-cl = 427 kj/mol

a. 1422 kj

b. 110 kj

c. 440 kj

d. - 440 kj

e. - 110 kj

option d = - 440 kj

Explanation:

chemical equation:

CH4 + 4Cl2 → CCl4 + 4HCl

Given dа ta:

Bond broken energies:

C-H = 413 Kj/mol

Cl-Cl = 243 Kj/mol

Bond formation energies:

C-Cl = 339 Kj/mol

H-Cl = 427 Kj/mol

Formula:

δh° = ∑n (bonds broken) - ∑m (bonds formation)

Solution:

Total bonds broken energy:

C-H = 413 Kj/mol 4*413 Kj/mol = 1652 Kj/mol

Cl-Cl = 243 Kj/mol 4*243 Kj/mol = 272Kj/mol

total = 2624 Kj/mol

Total bond formation energy:

C-Cl = 339 Kj/mol 4*339 Kj/mol = 1356 Kj/mol

H-Cl = 427 Kj/mol 4*427 Kj/mol = 1708 Kj/mol

total = 3064 Kj/mol

Now we will put the values in formula to calculate the δh° for reaction.

δh° = ∑n (bonds broken) - ∑m (bonds formation)

δh° = (2624) - (3064)

δh° = - 440 kj