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

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

How many types of equilibrium are there based on the proportion of reactant and product?

$A$ 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

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?

Which of the following is not a characteristic property of chemical equilibrium?