In which of the following reactions at equilibria, the position of the equilibrium shifts towards the products, if the total pressure is increased?

(i) $X_2(g)+3 Y_2(g) \rightleftharpoons 2 X_3(g)$

(ii) $X_2(g)+Y_2(g) \rightleftharpoons 2 X Y(g)$

(iii) $X_2(g)+Z_2(g) \rightleftharpoons 2 X Z(g)$

(iv) $X_2(g)+Y_4(g) \rightleftharpoons 2 X Y_2(g)$

For the formation of ammonia gas from its constituent elements, the $K_p / K_C$ is

For a reaction, $A(s) \rightleftharpoons B(s)+C(g)$ the set of all correct statements are (A) $K$ is independent of $[A]$. (B) $K$ is dependent on partial pressure of $C$ at a given temperature. (C) $\Delta H$ will be independent of temperature. (D) $\Delta H$ is independent of the catalyst addition.

For a given reaction, $2 A \rightleftharpoons B+C$, the equilibrium constant is $2 \times 10^{-3}$. If at any given time the composition of the reaction mixture is $[A]=[B]=[C]=6 \times 10^{-5} \mathrm{M}$; predict in which direction the reaction will proceed and the correct value for reaction quotient.