If the equilibrium constant for the reaction ${N_2}_{(g)} + {O_2}_{(g)} \rightleftharpoons 2NO_{(g)}$ is $K$,then what is the equilibrium constant for the reaction $\frac{1}{2}{N_2}_{(g)} + \frac{1}{2}{O_2}_{(g)} \rightleftharpoons NO_{(g)}$?

The least stable oxide of nitrogen is:

For a chemical reaction $A \rightleftharpoons B, K_1 = 2.0$ and $B \rightleftharpoons C, K_2 = 0.01$. The equilibrium constant for the reaction $2C \rightleftharpoons 2A$ is $:-$

The compounds $A$ and $B$ are mixed in equimolar proportion to form the products,$A + B \rightleftharpoons C + D$. At equilibrium,one-third of $A$ and $B$ are consumed. The equilibrium constant for the reaction is:

The decomposition of $N_2O_4$ to $NO_2$ is carried out at $280 \ K$ in chloroform. When equilibrium has been established,$0.2 \ mol$ of $N_2O_4$ and $2 \times 10^{-3} \ mol$ of $NO_2$ are present in $2 \ L$ solution. The equilibrium constant for the reaction $N_2O_4 \rightleftharpoons 2NO_2$ is:

At $780 \ K$ and $10 \ atm$ pressure,the equilibrium constant for the reaction $2 \ A_{(g)} \rightleftharpoons B_{(g)} + C_{(g)}$ is $3.52$. At the same temperature and $7.04 \ atm$ pressure,the equilibrium constant for the same reaction is: