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\begin{equation*}  4HCl +O_2 \rightleftharpoons 2Cl_2 + 2H_2O  \end{equation*}  As it is an exothermic reaction, perfect conditions would be high pressure, low temperature, and excess $O_2$. However, a compromise is used.  \subsection{Le Chatelier's Principle (LCP)}  If a system is at equilibrium, the position of the equilibrium will move to oppose any change imposed on the system.  \begin{itemize}  \item Increasing concentration of reactants will cause the position to move towards the product side  \item Increasing concentration of products will cause the position to move towards the reactants side  \item A higher temperature will favour an endothermic reaction; the position will move in the direction of the endothermic reaction  \item A lower temperature will favour an exothermic reaction; the position will move in the direction of the exothermic reaction  \item An increase in pressure will move the equilibrium towards the side with fewer moles  \item A decrease in pressure will favour the side with more moles  \end{itemize}