calculate the heat of reaction δh for the following reaction: 2 hcl(g) + f₂(g)→2 hf(g) + cl₂(g) you can find…

Explanation:

Step1: Identify bonds broken

For $2HCl$, 2 $H - Cl$ bonds are broken; for $F_2$, 1 $F - F$ bond is broken.

Step2: Identify bonds formed

For $2HF$, 2 $H - F$ bonds are formed; for $Cl_2$, 1 $Cl - Cl$ bond is formed.

Step3: Look - up bond energies

Let $E_{H - Cl}$ be the bond energy of $H - Cl$, $E_{F - F}$ be the bond energy of $F - F$, $E_{H - F}$ be the bond energy of $H - F$, and $E_{Cl - Cl}$ be the bond energy of $Cl - Cl$. Assume $E_{H - Cl}=431\ kJ/mol$, $E_{F - F}=155\ kJ/mol$, $E_{H - F}=567\ kJ/mol$, $E_{Cl - Cl}=243\ kJ/mol$.

Step4: Calculate energy of bonds broken

Energy of bonds broken $E_{broken}=2\times E_{H - Cl}+E_{F - F}=2\times431 + 155=862+155 = 1017\ kJ/mol$.

Step5: Calculate energy of bonds formed

Energy of bonds formed $E_{formed}=2\times E_{H - F}+E_{Cl - Cl}=2\times567+243 = 1134 + 243=1377\ kJ/mol$.

Step6: Calculate $\Delta H$

$\Delta H=E_{broken}-E_{formed}=1017 - 1377=- 360\ kJ/mol$.

Answer:

$-360$