Under which of the following conditions of temperature and pressure will molecular hydrogen $(H_2)$ dissociate into atomic hydrogen $(H)$?

Which of the following changes will not alter the equilibrium concentration of ammonia in the reaction: $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)} \quad \Delta H = -x \text{ kJ}$?

In a vessel containing $SO_3$,$SO_2$,and $O_2$ at equilibrium,some helium gas is introduced so that the total pressure increases while temperature and volume remain constant. According to Le Chatelier's principle,the dissociation of $SO_3$:

Under which conditions of temperature and pressure is the dissociation of molecular hydrogen into atomic hydrogen favored?

The equilibrium $2SO_{2(g)} + O_{2(g)} \rightleftharpoons 2SO_{3(g)}$ shifts forward,if

Which of the following reactions will be affected by increasing the pressure? Also,mention whether the change will cause the reaction to proceed in the forward or backward direction.
$(i)$ $COCl_{2(g)} \longleftrightarrow CO_{(g)} + Cl_{2(g)}$
$(ii)$ $CH_{4(g)} + 2S_{2(g)} \longleftrightarrow CS_{2(g)} + 2H_2S_{(g)}$
$(iii)$ $CO_{2(g)} + C_{(s)} \longleftrightarrow 2CO_{(g)}$
$(iv)$ $2H_{2(g)} + CO_{(g)} \longleftrightarrow CH_3OH_{(g)}$
$(v)$ $CaCO_{3(s)} \longleftrightarrow CaO_{(s)} + CO_{2(g)}$
$(vi)$ $4NH_{3(g)} + 5O_{2(g)} \longleftrightarrow 4NO_{(g)} + 6H_2O_{(g)}$