For the reaction $N_2 + 3H_2 \rightleftharpoons 2NH_3 + 21.9 \, kcal$,under which conditions is the production of ammonia favored according to Le Chatelier's principle?

Adding an inert gas to the system $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$ at equilibrium at constant volume will lead to:

For the reaction $2SO_2(g) + O_2(g) \rightleftharpoons 2SO_3(g)$,$\Delta H^o = -198 \, kJ$. According to Le Chatelier's principle,the favorable conditions for the forward reaction are:

Describe the effect of:
$(a)$ Addition of $H_2$
$(b)$ Addition of $CH_3OH$
$(c)$ Removal of $CO$
$(d)$ Removal of $CH_3OH$ on the equilibrium of the reaction:
$2H_{2(g)} + CO_{(g)} \longleftrightarrow CH_3OH_{(g)}$

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?

Raising the temperature of an equilibrium system: