Will mark BRAINLIEST!
2 NO2(g) ⇄ N2O4(g)
If a large quantity of argon is added to the container in which this equilibrium is taking place, in what direction will the equilibrium shift?

NH4OH(aq) ⇄ NH3(g) + H2O(l)
In what direction will the equilibrium shift if ammonia is removed from the container as soon as it is produced?

Explanation:

2 NO2(g) ⇄ N2O4(g)

Adding Argon to this reaction will have NO effect. Catalysts nor inert gases have an affect on equilibrium conditions.

Only changes in concentration, temperature conditions and pressure-volume conditions (unless both sides have equal molar volumes) will affect the equilibria.  

NH4OH(aq) ⇄ NH3(g) + H2O(l)

Removing ammonia from reaction equilibrium causes the reaction to shift right to replace removed ammonia. => Think of the reaction as being on a seesaw => removing ammonia from the product side tilts the seesaw left causing the NH₄OH to decompose and deliver more NH₃ and H₂O to the product side to increase weight on that side and level the seesaw. :-)

chemistry sucks a**

explanation: