using the appropriate bond energies, calculate the heat of reaction $delta h$ for the following reaction: 2…

using the appropriate bond energies, calculate the heat of reaction $delta h$ for the following reaction: 2 h - br $\rightarrow$ h - h + br - br. 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 $delta h$ for the following reaction: 2 h - br $\rightarrow$ h - h + br - br. 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 and formed

In the reaction $2H - Br\rightarrow H - H+Br - Br$, 2 moles of $H - Br$ bonds are broken, 1 mole of $H - H$ bond is formed and 1 mole of $Br - Br$ bond is formed.

Step2: Look up bond - energies

Let the bond - energy of $H - Br$ be $E_{H - Br}$, $H - H$ be $E_{H - H}$ and $Br - Br$ be $E_{Br - Br}$. Assume $E_{H - Br}=366\ kJ/mol$, $E_{H - H}=436\ kJ/mol$ and $E_{Br - Br}=193\ kJ/mol$.

Step3: Calculate energy for bonds broken

The energy required to break 2 moles of $H - Br$ bonds is $2\times E_{H - Br}=2\times366\ kJ/mol = 732\ kJ/mol$.

Step4: Calculate energy for bonds formed

The energy released when 1 mole of $H - H$ and 1 mole of $Br - Br$ bonds are formed is $E_{H - H}+E_{Br - Br}=436\ kJ/mol + 193\ kJ/mol=629\ kJ/mol$.

Step5: Calculate $\Delta H$

$\Delta H$ (heat of reaction) is given by the energy of bonds broken minus the energy of bonds formed. So, $\Delta H=732\ kJ/mol-629\ kJ/mol = 103\ kJ/mol$.

Answer:

$103\ kJ/mol$