According to le chatelier's principle, increasing the pressure of the system shown below will shift equilibrium to the left (towards reactants).n2 (
g. + 3h2 (
g. 2nh3 (
g.

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)

I’m not sure what your trying to say here.. can you clarify again?