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

In the given reaction $N_2 + O_2 \rightleftharpoons 2NO$,equilibrium means that

For the equilibrium system $H_2 + I_2 \rightleftharpoons 2HI$,if the concentration of the reactants is increased at $25\,^oC$,what happens to the value of $K_c$?

For the reaction $H_{2(g)} + I_{2(g)} \rightleftharpoons 2HI_{(g)}$,the equilibrium constant changes with:

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:

$A$ liquid is in equilibrium with its vapour in a sealed container at a fixed temperature. The volume of the container is suddenly increased.
$(a)$ What is the initial effect of the change on vapour pressure?
$(b)$ How do rates of evaporation and condensation change initially?
$(c)$ What happens when equilibrium is restored finally and what will be the final vapour pressure?