$2NOBr(g) \rightleftharpoons 2NO(g) + Br_2(g)$. If nitrosyl bromide $(NOBr)$ is $40\%$ dissociated at a certain temperature and a total pressure of $0.3 \ atm$,what is the $K_P$ for the reaction $2NO(g) + Br_2(g) \rightleftharpoons 2NOBr(g)$?

For the reaction $H_{2(g)} + I_{2(g)} \rightleftharpoons 2HI_{(g)}$,the value of $K_c$ at $440 \ ^oC$ is $50$. If the reaction is initiated in a $1 \ L$ flask with $1 \ mol$ of $H_2$,$2 \ mol$ of $I_2$,and $3 \ mol$ of $HI$,then the equilibrium concentration of $HI$ will be .......... $M$.

At $T(K)$,the $K_c$ value of the reaction $AO_{2(g)} + BO_{2(g)} \rightleftharpoons AO_{3(g)} + BO_{(g)}$ is $16$. In a closed $1 \ L$ flask,one mole each of $AO_2, BO_2, AO_3$ and $BO$ are taken and heated to $T(K)$. Identify the correct statements about this equilibrium.
$I)$ Total number of moles at equilibrium is $4$
$II)$ At equilibrium,the ratio of moles of $AO_2$ and $AO_3$ is $1:4$
$III)$ Total number of moles of $AO_2$ and $BO_2$ at equilibrium is $0.8$

For the reaction $A_{(g)} + 2B_{(g)} \rightleftharpoons 2C_{(g)}$,if the reaction is carried out in a constant volume vessel starting with equal amounts of $A$ and $B$,which of the following will be true at equilibrium?

At $500 \ K$,for a reversible reaction $A_{2(g)} + B_{2(g)} \rightleftharpoons 2 AB_{(g)}$ in a closed container,$K_C = 2 \times 10^{-5}$. In the presence of a catalyst,the equilibrium is attained $10$ times faster. The equilibrium constant $K_C$ in the presence of a catalyst at the same temperature is:

Reaction between $N_{2}$ and $O_{2}$ takes place as follows:
$2 N_{2(g)} + O_{2(g)} \longleftrightarrow 2 N_{2}O_{(g)}$
If a mixture of $0.482 \ mol$ of $N_{2}$ and $0.933 \ mol$ of $O_{2}$ is placed in a $10 \ L$ reaction vessel and allowed to form $N_{2}O$ at a temperature for which $K_{c} = 2.0 \times 10^{-37}$,determine the composition of the equilibrium mixture.