The equilibrium constant in a reversible reaction at a given temperature:

The equilibrium constant for the reaction $N_{2(g)} + O_{2(g)} \rightleftharpoons 2NO_{(g)}$ is $4 \times 10^{-4}$ at $2000 \ K$. In the presence of a catalyst,equilibrium is attained ten times faster. Therefore,the equilibrium constant in the presence of the catalyst at $2000 \ K$ is:

For a reversible reaction,if the concentration of reactants is increased,the equilibrium constant of the reaction

For a reversible chemical reaction at equilibrium involving two reactants,if the concentrations of the reactants are doubled,what happens to the equilibrium constant $(K_c)$?

$A$ chemical reaction is at equilibrium when

Explain liquid-vapour equilibrium.