At a certain temperature,the equilibrium constant $(K_C)$ is $16$ for the reaction:
$SO_2(g) + NO_2(g) \rightleftharpoons SO_3(g) + NO(g)$
If we take one mole of each of the four gases in a $1 \ L$ container,what would be the equilibrium concentration of $NO$ and $NO_2$ respectively?

For the reaction $2NO_{2(g)} \rightleftharpoons N_2O_{4(g)}$ at $300 \ K$,the value of $K_p$ is $2 \ atm^{-1}$. The total pressure at equilibrium is $10 \ atm$. If the volume of the container becomes two times its original volume,what will be its equilibrium pressure at $300 \ K$ (in $atm$)?

Air containing $79\%$ of nitrogen and $21\%$ of oxygen by volume is heated at $2200 \ K$ and $1 \ atm$ until equilibrium is established according to the reaction $N_{2(g)} + O_{2(g)} \rightleftharpoons 2NO_{(g)}$. If the $K_p$ of the reaction is $1.1 \times 10^{-3}$,calculate the amount of nitric oxide produced in terms of volume percent.

Identify the incorrect statement.

For the equilibrium reaction $A + B \rightleftharpoons C + D$,if we start with equal concentrations of $A$ and $B$,at equilibrium,the concentration of $C$ is $2$ times that of $A$. Find the value of $K_c$.

Consider a reversible reaction $2A + B \rightleftharpoons 2C$ having equilibrium constant $K_c = 25$. If a reaction vessel contains $2 \ mol$ of $A$,$0.25 \ mol$ of $B$,and $0.5 \ mol$ of $C$ in a $100 \ L$ vessel,what will be the direction of the reaction?