What would happen to a reversible reaction at equilibrium when an inert gas is added while the pressure remains unchanged?

On the basis of the $Le \ Chatelier$ principle,explain how temperature and pressure can be adjusted to increase the yield of ammonia in the following reaction: $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$; $\Delta H = -92.38 \ kJ \ mol^{-1}$. What will be the effect of the addition of argon to the above reaction mixture at constant volume?

Write the effect of concentration change on equilibrium and explain it with a suitable example.

In a reversible reaction,a catalyst:

For a given equilibrium reaction,addition of inert argon gas at constant volume can shift the equilibrium in $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$

The equilibrium of the reaction $2A_{(s)} + 3B_{(g)} \rightleftharpoons 3C_{(g)} + D_{(g)} + Q$ is represented as shown. If the pressure on the system is reduced to half of its original value,then: