If the equilibrium constant of a reaction is $K_c = 1.6 \times 10^{12}$,then at equilibrium,the system will contain:

If some $He$ gas is added to the equilibrium $PCl_{5(g)} \rightleftharpoons PCl_{3(g)} + Cl_{2(g)}$ at constant pressure and temperature,the equilibrium constant of the reaction will....

$A$ 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?

For the reaction $2HI_{(g)} \rightleftharpoons H_{2(g)} + I_{2(g)}$,the equilibrium constant $K$ at room temperature is $2.85$,and at $698 \ K$ it is $1.4 \times 10^{-2}$. This indicates that:

For a reaction $H_2 + I_2 \rightleftharpoons 2HI$ at $721 \ K$,the value of equilibrium constant is $50$. If $0.5 \ mol$ each of $H_2$ and $I_2$ is added to the system,the value of equilibrium constant will be

In a chemical reaction,equilibrium is established when: