$2 \ HI_{(g)} \rightleftharpoons H_{2(g)} + I_{2(g)}$
The equilibrium constant of the above reaction is $6.4$ at $300 \ K$. If $0.25 \ mol$ each of $H_{2}$ and $I_{2}$ are added to the system,the equilibrium constant will be

Equilibrium is a steady state,but it is dynamic in nature. What is the meaning of this statement?

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?

$A$ chemical reaction $A \rightleftharpoons B$ is said to be in equilibrium when ........

Pure ammonia is placed in a vessel at a temperature where its dissociation constant $(\alpha)$ is appreciable. At equilibrium,

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