How to apply Le Chatelier's principle? The following reaction is at equilibrium $$\ce{4HCl(aq) + O2(g) &lt;=&gt;2H2O(l) + 2Cl2(g)}\quad \Delta H&gt;0$$Which one of the following changes will result in an increase in the concentration of $\ce{Cl2(g)}$
  
  
  adding some $\ce{H2O}$
  decreasing the temperature
  adding a catalyst
  decreasing the pressure
  removing some $\ce{HCl}$ 
  


Decreasing the pressure (4) is the answer but I don't understand why. I though decreasing pressure shifts the equilibrium to the side with the larger number of moles which is the left?
Remember that $\ce{HCl}$ (aq) and $\ce{H2O}$(l) are liquids while the oxygen and chlorine are gases . As the number of moles of gases on the left  hand side (one mole of oxygen) is smaller than that of the right hand side (two moles of chlorine), decreasing the pressure makes the equilibrium position move to the right hand side, therefore the concentration of chlorine increases.