In which of the following equilibrium reactions does the equilibrium shift to the right when the total pressure is decreased?

$KMnO_4$ can be prepared from $K_2MnO_4$ as per the reaction:
$3MnO_4^{2-} + 2H_2O \rightleftharpoons 2MnO_4^- + MnO_2 + 4OH^-$
The reaction can go to completion by removing $OH^-$ ions by adding:

$H_2O_{(s)} \rightleftharpoons H_2O_{(\ell)}$
Which of the following statements are correct for the above reaction?
$(A)$ At $273 \ K$ and $1 \ atm$, $\Delta G = 0$ and $\Delta S > 0$.
$(B)$ On increasing pressure, more ice will melt.
$(C)$ On increasing pressure, the melting point of ice will decrease.
$(D)$ The melting point of ice increases on increasing pressure.

The exothermic formation of $ClF_3$ is represented by the equation
$Cl_{2(g)} + 3F_{2(g)} \rightleftharpoons 2ClF_{3(g)}$; $\Delta H_r = -329 \ kJ$
Which of the following will increase the quantity of $ClF_3$ in an equilibrium mixture of $Cl_2, F_2$ and $ClF_3$?

The oxidation of $SO_2$ to $SO_3$ by $O_2$ is an exothermic reaction: $2SO_2(g) + O_2(g) \rightleftharpoons 2SO_3(g) + \text{Heat}$. The yield of $SO_3$ will increase if:

Which one of the following conditions will favour maximum formation of the product in the reaction
$A_{2(g)} + B_{2(g)} \rightleftharpoons X_{2(g)}; \Delta_{r} H = -X \ kJ$