using the appropriate bond energies, calculate the heat of reaction δh for the following reaction: 2 h - cl…

using the appropriate bond energies, calculate the heat of reaction δh for the following reaction: 2 h - cl + br - br → 2 h - br + cl - cl you can find a table of bond energies by using the data button on the aleks toolbar. round your answer to the nearest kj/mol. note: for clarity, all lone pairs have been omitted from the molecular structures.

using the appropriate bond energies, calculate the heat of reaction δh for the following reaction: 2 h - cl + br - br → 2 h - br + cl - cl you can find a table of bond energies by using the data button on the aleks toolbar. round your answer to the nearest kj/mol. note: for clarity, all lone pairs have been omitted from the molecular structures.

Answer

Explanation:

Step1: Identify bond - breaking and forming

The bonds broken are 2 H - Cl and 1 Br - Br. The bonds formed are 2 H - Br and 1 Cl - Cl.

Step2: Look up bond energies

Let (E_{H - Cl}) be the bond energy of H - Cl, (E_{Br - Br}) be the bond energy of Br - Br, (E_{H - Br}) be the bond energy of H - Br, and (E_{Cl - Cl}) be the bond energy of Cl - Cl. Assume (E_{H - Cl}=431\ kJ/mol), (E_{Br - Br}=193\ kJ/mol), (E_{H - Br}=366\ kJ/mol), (E_{Cl - Cl}=243\ kJ/mol) (values from standard bond - energy tables).

Step3: Calculate energy for bond - breaking

The energy required for bond - breaking ((E_{break})) is (2\times E_{H - Cl}+E_{Br - Br}=2\times431 + 193=862+193 = 1055\ kJ/mol).

Step4: Calculate energy for bond - forming

The energy released during bond - forming ((E_{form})) is (2\times E_{H - Br}+E_{Cl - Cl}=2\times366+243 = 732 + 243=975\ kJ/mol).

Step5: Calculate (\Delta H)

(\Delta H=E_{break}-E_{form}=1055 - 975=80\ kJ/mol).

Answer:

80 kJ/mol