In a reversible reaction at equilibrium between two reactants,if the concentration of the reactants is doubled,the equilibrium constant ..........

In the chemical equilibrium of a reversible reaction,which of the following does not cause any change?

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 a reversible chemical reaction at equilibrium, if the concentration of any one of the reactants is doubled, then the equilibrium constant will

If the concentration of reactants is increased by $x$ times,the equilibrium constant $K$ will become ................

Explain liquid-vapour equilibrium.