For the reaction $SO_{2(g)} + NO_{2(g)} \rightleftharpoons SO_{3(g)} + NO_{(g)}$,the equilibrium constant $K_c$ is $16$. If $1 \ mol$ of each gas is taken in a $1 \ dm^3$ vessel,the equilibrium concentration of $NO$ will be ....

For the reaction,$NO_2 + CO \rightleftharpoons NO + CO_2$,one mole of $NO_2$ and $2$ moles of $CO$ were kept in a vessel. Calculate the equilibrium constant $K_p$,if at equilibrium $25 \%$ of the initial amount of $CO$ is consumed.

$A$ solid $XY$ kept in an evacuated sealed container undergoes decomposition to form a mixture of gases $X$ and $Y$ at temperature $T$. The equilibrium pressure is $10 \, bar$ in the vessel. $K_p$ for this reaction is

For the following reactions,equilibrium constants are given:
$S_{(s)} + O_{2(g)} \rightleftharpoons SO_{2(g)}; K_1 = 10^{52}$
$2S_{(s)} + 3O_{2(g)} \rightleftharpoons 2SO_{3(g)}; K_2 = 10^{129}$
The equilibrium constant for the reaction $2SO_{2(g)} + O_{2(g)} \rightleftharpoons 2SO_{3(g)}$ is:

$A$ plot of $\ln \ K$ against $\frac{1}{T}$ (abscissa) is expected to be a straight line with an intercept on the ordinate axis equal to:

For the reaction $3A + B \rightleftharpoons 2C + D$,if the equilibrium concentrations of $A, B,$ and $C$ are $0.03 \ M, 0.01 \ M,$ and $0.008 \ M$ respectively,what is the initial concentration of $A$ (in $M$)?