Decreasing pressure [de/in]creases the crowding of gaseous molecules. The system will respond by [de/in]creasing their crowding. Crowding can be increased by forming [fewer/more] molecules. In the Haber Process, that means that for a while the [forward/reverse] reaction will occur at a higher rate than the [forward/reverse] reaction. The reverse reaction changes every 2 molecules of ammonia into [?] molecules (1 nitrogen and 3 hydrogen molecules). This causes the amount of ammonia present to [de/in]crease and the amount of nitrogen and hydrogen to [de/in]crease. While this is happening the system [is/is not] in equilibrium. After a while a new dynamic equilibrium will be reached, in which the rates of both forward and reverse reactions will one another, and the amounts of reactants and products will remain . However, compared to before the pressure was applied, there will now be [more/less] ammonia present at equilibrium. The equilibrium constant value, Kc, however, will be [higher than/lower than/the same as] it was in the original equilibrium.