$A$ reversible reaction $H_2 + Cl_2 \rightleftharpoons 2HCl$ is carried out in a $1 \ L$ flask. If the same reaction is carried out in a $2 \ L$ flask,the equilibrium constant will be

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:

Predict which of the following reactions will have an appreciable concentration of both reactants and products:
$(a)$ $Cl_{2(g)} \longleftrightarrow 2Cl_{(g)};$ $K_{c}=5 \times 10^{-39}$
$(b)$ $Cl_{2(g)}+2NO_{(g)} \longleftrightarrow 2NOCl_{(g)};$ $K_{c}=3.7 \times 10^{8}$
$(c)$ $Cl_{2(g)}+2NO_{2(g)} \longleftrightarrow 2NO_{2}Cl_{(g)};$ $K_{c}=1.8$

For the reaction $H_{2(g)} + I_{2(g)} \rightleftharpoons 2HI_{(g)}$,the equilibrium constant is $64$. If the volume of the container is reduced to $1/4$ of its original value,the value of the equilibrium constant will be .......

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

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