For the reversible reaction,N2(g)+3H2(g)⇌2NH3(g)+ Heat The equilibrium shifts in forward direction

Any change in the concentration, pressure and temperature of the reaction results in change in the direction of equilibrium. This change in the direction of equilibrium is governed by Le-Chatelier's principle. According to Le-Chatelier's principle, equilibrium shifts in the opposite direction to undo the change.N2(g)+3H2(g)⇌2NH3(g)(a) Increasing the concentration of NH3 (g) On increasing the concentration of NH3(g), the equilibrium shift in the backward direction where concentration of NH3(g)decreases.(b) Decreasing the pressure Equilibrium shifts in the backward direction where number of moles are increasing.(c) Decreasing the concentration of N2(g) and H2(g) Equilibrium shifts in the backward direction, when concentration of N2(g) and H2(g) decreases.(d) Increasing pressure and decreasing temperature On increasing pressure, equilibrium shifts in the forward direction where number of moles decreases, while on decreasing temperature, it will move in forward direction where temperature increases.