N2(g) + 3H2(g) =2NH3(g)
Number of moles of reactants > product...
Therfore if pressure is increased.
Equilibrium is disturbed according to LCP....
Equilibrium shift to the right (product)
......
If you want to understant the fundamental concept:
Take for example 2A + 3B = 4C
Reactant: 5 moles (5 volumes)
Product: 4 moles (4 volumes)
When pressure of a gas is increased, volume decreases!
(Vice-versa)
If pressure is increased, volume decreases. Hence number of collisions INCREASES(constrain). Equilibrium shifts in such a direction so as to decrease the number of collision accordinf to LCP...
This happens when number of paeticles decreases as equilibrium shift forward because the forward reaction is accompanied by a decrease in number of particles (5 to 4)
