Calculate the enthalpy change of the reaction,
$\text{H}_2\text{(g)} + \text{Cl}_2\text{(g)} \rightarrow 2\text{HCl(g)}$
if bond energies (kJ mol$^{-1}$):
H–H = 436, Cl–Cl = 242, H–Cl = 431

The equilibrium constant for a reaction is $100$. What will be the value of standard Gibbs energy change at $298$ K ? ($R = 8.314$ J $\text{K}^{-1}\text{mol}^{-1}$)

The bond dissociation enthalpy of $\text{H}_2$, $\text{Cl}_2$ and HCl are $434$, $242$ and $431$ kJ $\text{mol}^{-1}$ respectively. Calculate the enthalpy of formation of HCl.

$200$ mL of ethylene gas and $150$ mL of HCl gas were allowed to react at $1$ bar. Pressure to form gaseous ethyl chloride. What is the work done during the reaction?