Sergey Bylikin, Gary Horner and, Brian Murphy Solutions for Chapter: Energetics and Thermochemistry, Exercise 5: Quick questions

In the chlor-alkali industry chlorine gas is combined with hydrogen gas to produce hydrogen chloride as ${\mathrm{Cl}}_2\left(\mathrm{g}\right)+{\mathrm{H}}_2\left(\mathrm{g}\right)\stackrel{ }{\to }2\mathrm{HCl}\left(\mathrm{g}\right)$. If the enthalpy change for this reaction is $-185 \mathrm{kJ}$, calculate the bond enthalpy for the $\mathrm{H}-\mathrm{Cl}$ bond. Bond enthalpies of $\mathrm{Cl}-\mathrm{Cl}$ and $\mathrm{H}-\mathrm{H}$ are $242 \mathrm{kJ} {\mathrm{mol}}^{-1}$ and $436 \mathrm{kJ} {\mathrm{mol}}^{-1}$ respectively.

Methane and chlorine react to produce chloromethane and hydrogen chloride. Write the balanced chemical equation for this reaction.

Methane and chlorine react to produce chloromethane and hydrogen chloride. Using bond enthalpy values from the below table, determine the enthalpy change for this reaction.

Methane and chlorine react to produce chloromethane and hydrogen chloride. The value of enthalpy change for this reaction is found to be $-107 \mathrm{kJ}$. Deduce whether this reaction is exothermic or endothermic.

Methane and chlorine react to produce chloromethane and hydrogen chloride. The value of enthalpy change for this reaction is found to be $-107 \mathrm{kJ}$. Which are more energetically stable, the reactants or the products?