For the reaction $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$,in which direction will the equilibrium shift if an inert gas is added at constant pressure?

Consider the following reaction where the enthalpy change is positive: $2A_{(g)} \rightleftharpoons C_{(g)} + D_{(g)}$. Which of the following will not affect the equilibrium?

For the reaction $CO_{(g)} + H_2O_{(g)} \rightleftharpoons CO_{2(g)} + H_{2(g)}$,the equilibrium amount of $CO_{2(g)}$ increases by:

For the reaction $PCl_{5(g)} \rightleftharpoons PCl_{3(g)} + Cl_{2(g)}$,the forward reaction is favored at constant temperature by: $(1)$ Adding an inert gas at constant volume $(2)$ Adding $Cl_{2(g)}$ at constant volume $(3)$ Adding an inert gas at constant pressure $(4)$ Increasing the volume of the container $(5)$ Adding $PCl_{5(g)}$ at constant volume

In the manufacture of $NH_3$ in Haber's continuous flow process involving the reaction $N_{2(g)} + 3H_{2(g)} \longleftrightarrow 2NH_{3(g)}$,$\Delta H = -22.08 \ kcal$. The favourable conditions are:

For the balanced reaction $2SO_2(g) + O_2(g) \rightleftharpoons 2SO_3(g) + \text{Heat}$,which of the following conditions will favor the forward reaction?