If the concentration of reactants is increased by $x$,then the equilibrium constant $K$ becomes:

In which of the following cases does the reaction proceed towards completion?

For the reaction $N_2 + 3H_2 \rightleftharpoons 2NH_3$,the value of $K_c$ does not depend on: $(a)$ Initial concentration of reactants $(b)$ Pressure $(c)$ Temperature $(d)$ Catalyst

$2 \ HI_{(g)} \rightleftharpoons H_{2(g)} + I_{2(g)}$
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

In the chemical reaction $A \rightleftharpoons B$,the system will be known to be in equilibrium when:

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 .......