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

using the appropriate bond energies, calculate the heat of reaction δh for the following reaction: 2h - cl + f - f → 2h - f + 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: 2h - cl + f - f → 2h - f + 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 bonds broken

2 moles of H - Cl bonds and 1 mole of F - F bonds are broken. Let $E_{H - Cl}$ be the bond - energy of H - Cl bond, $E_{F - F}$ be the bond - energy of F - F bond. Energy absorbed for bond - breaking, $E_{absorbed}=2E_{H - Cl}+E_{F - F}$.

Step2: Identify bonds formed

2 moles of H - F bonds and 1 mole of Cl - Cl bonds are formed. Let $E_{H - F}$ be the bond - energy of H - F bond, $E_{Cl - Cl}$ be the bond - energy of Cl - Cl bond. Energy released for bond - formation, $E_{released}=2E_{H - F}+E_{Cl - Cl}$.

Step3: Calculate $\Delta H$

The heat of reaction $\Delta H=E_{absorbed}-E_{released}=(2E_{H - Cl}+E_{F - F})-(2E_{H - F}+E_{Cl - Cl})$. Assume $E_{H - Cl}=431\ kJ/mol$, $E_{F - F}=155\ kJ/mol$, $E_{H - F}=567\ kJ/mol$, $E_{Cl - Cl}=243\ kJ/mol$. $\Delta H=(2\times431 + 155)-(2\times567+243)$ $=(862 + 155)-(1134 + 243)$ $=1017-1377$ $=- 360\ kJ/mol$

Answer:

$-360$