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

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

For the chemical reaction $3X_{(g)} + Y_{(g)} \to X_3Y_{(g)}$,the amount of $X_3Y$ at equilibrium is affected by

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 gaseous reaction $A(g) + B(g) \rightleftharpoons 2C(g) + D(g) + Q$ is most favoured at

In what manner will an increase of pressure affect the following equilibrium equation?
$C_{(s)} + H_2O_{(g)} \rightleftharpoons CO_{(g)} + H_{2(g)}$