The endothermic reaction $(M + N \rightleftharpoons P)$ is allowed to attain an equilibrium at $25^o C$. Formation of $P$ can be increased by

Match List-$I$ (Equilibrium) with List-$II$ (Conditions for the process) and select the correct answer from the options given below.

List-$I$ (Equilibrium)	List-$II$ (Conditions for the process)
$P. A_{2(g)} + B_{2(g)} \rightleftharpoons 2AB_{(g)}$ (Endothermic)	$1. \text{High temperature}$
$Q. 2AB_{2(g)} + B_{2(g)} \rightleftharpoons 2AB_{3(g)}$ (Exothermic)	$2. \text{Low temperature}$
$R. 2AB_{3(g)} \rightleftharpoons A_{2(g)} + 3B_{2(g)}$ (Endothermic)	$3. \text{High temperature}$
	$4. \text{Low temperature}$
	$5. \text{Independent of pressure}$

The equilibrium constant for a reaction,$A + B \rightleftharpoons C + D$ is $1 \times 10^{-2}$ at $298 \ K$ and is $2$ at $273 \ K$. The chemical process resulting in the formation of $C$ and $D$ is

In a reversible reaction,a catalyst...

In which reaction will an increase in the volume of the container favour the formation of products?

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: