In which of the following reactions will the amount of products not increase upon increasing the pressure?

Consider the equilibrium $CO_{(g)} + 3H_{2(g)} \rightleftharpoons CH_{4(g)} + H_2O_{(g)}$. If the pressure applied over the system increases by two-fold at constant temperature,then which of the following statements are correct?
$(A)$ Concentration of reactants and products increases.
$(B)$ Equilibrium will shift in the forward direction.
$(C)$ Equilibrium constant increases since the concentration of products increases.
$(D)$ Equilibrium constant remains unchanged as the concentration of reactants and products remain the same.
Choose the correct answer from the options given below:

For the following gaseous reversible reaction: $3A_{(g)} + B_{(g)} \rightleftharpoons A_3B_{(g)}$ $(\Delta H = -q \text{ kJ})$. The amount of product $A_3B_{(g)}$ is affected by . . . . . .

For the reaction at equilibrium
$N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$
On addition of an inert gas at constant pressure and constant temperature,which of the following changes is $NOT$ observed?

In the melting of ice,which one of the conditions will be more favourable?

What happens when pressure is increased on the equilibrium system $Ice \rightleftharpoons Water$?