The equilibrium constant for a reaction $A + B \rightleftharpoons C + D$ is $1 \times 10^{-3}$ at $298 \ K$ and is $2$ at $273 \ K$. The chemical reaction resulting in the formation of $C$ and $D$ is

On addition of an inert gas at constant volume to the reaction $N_2 + 3H_2 \rightleftharpoons 2NH_3$ at equilibrium,

Which of the following will favour the reverse reaction in a chemical equilibrium?

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:

The increase of pressure on the ice $\rightleftharpoons$ water system at constant temperature will lead to:

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