The reaction you've provided is the synthesis of ammonia (NH3) from nitrogen (N2) and hydrogen (H2):
2NH3 ⇌ N2 + 3H2
When you increase the pressure of a system at equilibrium, the system will try to counteract the change by shifting the equilibrium in a direction that reduces the change in pressure. In this case, the reaction involves different numbers of moles on each side, with two moles of ammonia (NH3) on the left and four moles of gases (N2 + 3H2) on the right.
Increasing the pressure will favor the side with fewer moles of gas to reduce the pressure. In other words, it will favor the side with fewer molecules colliding with the container walls. In this reaction, the right side (N2 + 3H2) has more moles of gas, so increasing the pressure will drive the equilibrium to the left, favoring the formation of ammonia (NH3).
Therefore, by increasing the pressure from 5 atm to 8 atm, the equilibrium position of the reaction will shift towards the reactants (NH3), resulting in more ammonia being formed in an attempt to counteract the increase in pressure.