$K_p$ for the reaction $2SO_3 \rightleftharpoons 2SO_2 + O_2$ at $700 \ K$ is $1.3 \times 10^{-3} \ atm$. The $K_c$ at the same temperature for the reaction $2SO_2 + O_2 \rightleftharpoons 2SO_3$ will be:

$A + B \rightleftharpoons C + D$. If the final equilibrium concentrations of $A$ and $B$ are equal,and the equilibrium concentration of $D$ is twice that of $A$,what is the equilibrium constant $(K_c)$ of the reaction?

One of the reactions that takes place in producing steel from iron ore is the reduction of iron $(II)$ oxide by carbon monoxide to give iron metal and $CO_{2}$.
$FeO(s) + CO(g) \longleftrightarrow Fe(s) + CO_{2}(g);$ $K_{p} = 0.265$ at $1050 \, K$
What are the equilibrium partial pressures of $CO$ and $CO_{2}$ at $1050 \, K$ if the initial partial pressures are: $p_{CO} = 1.4 \, atm$ and $p_{CO_{2}} = 0.80 \, atm$?

The degree of dissociation of $PCl_{5(g)}$ at $16.8 \ bar$ and $127 \ ^oC$ is $0.4$. The value of $K_p$ for the reaction $PCl_{5(g)} \rightleftharpoons PCl_{3(g)} + Cl_{2(g)}$ is

Find the value of $\frac{P}{K_p}$ for the reaction at a certain temperature: $2NOBr_{(g)} \rightleftharpoons 2NO_{(g)} + Br_{2(g)}$,where $P$ is the total pressure of gases at equilibrium and $P_{Br_2} = \frac{P}{9}$.

For the reactions $NO_{(g)} + 1/2 O_{2(g)} \rightleftharpoons NO_{2(g)}$ and $2NO_{2(g)} \rightleftharpoons 2NO_{(g)} + O_{2(g)}$,the equilibrium constants at a given temperature are $K_1$ and $K_2$ respectively. If the value of $K_1$ is $4 \times 10^{-3}$,then the value of $K_2$ will be ....