For the gaseous reaction,equilibrium constant is given:
$XeF_6 + H_2O \rightleftharpoons XeOF_4 + 2HF, K_1$
$XeO_4 + XeF_6 \rightleftharpoons XeOF_4 + XeO_3F_2, K_2$
The equilibrium constant for the reaction:
$XeO_4 + 2HF \rightleftharpoons XeO_3F_2 + H_2O$ will be

The equilibrium constants for some reactions are given below:
$(1)$ $x \rightleftharpoons y ; K = 10^{-1}$
$(2)$ $y \rightleftharpoons z ; K = 2 \times 10^{-2}$
$(3)$ $p \rightleftharpoons Q ; K = 3 \times 10^{-4}$
$(4)$ $R \rightleftharpoons S ; K = 2 \times 10^{-3}$
The initial concentrations of reactants are taken to be the same for each reaction. Which of the above reactions indicate that the reaction mixture contains high concentrations of reactants and products respectively?

For the reaction $A + 2B \rightleftharpoons C$,the expression for equilibrium constant is

$3 O_{2(g)} \rightleftharpoons 2 O_{3(g)}$
For the above reaction at $298 \ K$,$K_c$ is found to be $3.0 \times 10^{-59}$. If the concentration of $O_2$ at equilibrium is $0.040 \ M$,then the concentration of $O_3$ in $M$ is ...... .

The value of $K_{c}$ for the reaction $2 A \rightleftharpoons B + C$ is $2 \times 10^{-3}$. At a given time,the composition of the reaction mixture is $[ A ] = [ B ] = [ C ] = 3 \times 10^{-4} \ M$. In which direction will the reaction proceed?

The following equilibria are given:
$N_2 + 3H_2 \rightleftharpoons 2NH_3 ; K_1$
$N_2 + O_2 \rightleftharpoons 2NO ; K_2$
$H_2 + \frac{1}{2}O_2 \rightleftharpoons H_2O ; K_3$
The equilibrium constant of the reaction $2NH_3 + \frac{5}{2}O_2 \rightleftharpoons 2NO + 3H_2O$ in terms of $K_1, K_2$ and $K_3$ is: