For a reversible reaction involving two reactants,if the concentration of the reactants is doubled,the equilibrium constant will:

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

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

One mole of $A_{(g)}$ is heated to $200^{\circ} C$ in a one litre closed flask,until the following equilibrium is reached:
$A_{(g)} \rightleftharpoons B_{(g)}$
The rate of forward reaction at equilibrium is $0.02 \ mol \ L^{-1} \ min^{-1}$. What is the rate (in $mol \ L^{-1} \ min^{-1}$) of the backward reaction at equilibrium?

For the equilibrium, $H_{2}O_{(l)} \rightleftharpoons H_{2}O_{(g)},$ which of the following is correct?

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