In any chemical reaction,equilibrium is supposed to be established when

The equilibrium constant of the reaction $H_{2(g)} + I_{2(g)} \rightleftharpoons 2HI_{(g)}$ is $64$. If the volume of the container is reduced to one-fourth of its original volume,the value of the equilibrium constant will be

Assertion : The equilibrium constant is fixed and a characteristic for any given chemical reaction at a specified temperature.
Reason : The composition of the final equilibrium mixture at a particular temperature depends upon the starting amount of reactants.

In which of the following cases does the reaction proceed towards completion?

Given the reactions at $500 \ K$:
$(i) \ H_{2(g)} + 1/2 O_{2(g)} \rightleftharpoons H_2O_{(g)}$,$K_c = 2.4 \times 10^{47}$
$(ii) \ H_2O_{(g)} \rightleftharpoons H_{2(g)} + 1/2 O_{2(g)}$,$K_c = 4.1 \times 10^{-48}$
What does the magnitude of $K_c$ indicate about the formation of the product in reaction $(i)$?

In which of the following reactions,the concentration of product is higher than the concentration of reactant at equilibrium? $(K = \text{equilibrium constant})$