According to Le ’s principle, when a system which is in equilibrium is disturbed, it will respond in such a way as to the disturbance. An increase in pressure [de/in]creases the crowding of gaseous molecules. The system will respond by [de/in]creasing their crowding. Crowding is decreased in gases when [fewer/more] molecules are formed. In the Haber Process the [forward/reverse] reaction makes fewer molecules than the [forward/reverse] reaction. In the forward reaction [?] molecules of ammonia are made from every 4 molecules of reactants (1 N2 and 3 H2 molecules). Consequently, an increase in pressure equilibrium for a while by making the [forward/reverse] reaction occur at a higher rate than the [forward/reverse] reaction. This causes [more/less] ammonia to be formed and [more/less] nitrogen and hydrogen. After a while a new dynamic equilibrium is reached. The rates of forward and reverse reactions are again to one another, and the amounts of reactants and products will [change/remain constant]. 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.