Shift in the position of equilibrium by a catalyst to favor the forward reaction
Wikipedia says 


  Catalyzed reactions have a lower activation energy (rate-limiting free energy of activation) than the corresponding uncatalyzed reaction, resulting in a higher reaction rate at the same temperature and for the same reactant concentrations.


This means that a catalyst will reduce activation energy as seen here


  


We clearly see that the activation energy of both forward and backward reaction equally. Hence by Arrhenius equation both the rate constants change by same factor thereby there is no change in equilibrium constant.