A mixture containing $2$ moles of $N_2$ and $3$ moles of $H_2$ gas is brought to equilibrium in a $3L$ vessel. If the molar concentration of $N{H}_3$ at equilibrium is $1/3mol/L$, calculate the $K_c$ for the formation of $N{H}_3$.
$N_2\left(g\right)+3H_2\left(g\right)\rightleftharpoons 2N{H}_3\left(g\right)$.

Q. An equilibrium mixture of $N_2$, $H_2$, and $N{H}_3$ at $700K$contains $0.036M{N}_2$ and $0.15M$ $H_2$. At this temperature, $K_c$ for the reaction $N_2\left(g\right)+3H_2\left(g\right)\rightleftharpoons 2N{H}_3\left(g\right)$ is $0.29$. What is the concentration of $N{H}_3$?

Q. At a certain temperature (T), the equilibrium constant $\left(K_c\right)$ is 1 for the reaction $N_2\left(g\right)+3H_2\left(g\right)\rightleftharpoons 2N{H}_3\left(g\right)$
If 2 moles of $N_2,$ 4 moles of $H_2,$ 6 moles of $N{H}_3$ and 3 moles of inert gas are introduced into a two litre rigid vessel at constant temperature T. It has been found that equilibrium concentration of $H_2$ and $N{H}_3$ are equal then what is the equilibrium concentration of $N_2$ (in M)?

Q. $1$ mole of $N_2$ and $3$ moles of $H_2$ are placed in $1L$ vessel. Find the concentration of $N{H}_3$ at equilibrium, if the equilibrium constant $\left(K_C\right)$ at $400K$ is $\frac{4}{27}$
$N_2\left(g\right)+3H_2\left(g\right)\rightleftharpoons 2N{H}_3\left(g\right)$.

Q. Calculate the equilibrium constant $\left(Kc\right)$ for the formation of $N{H}_3$ in the following reaction:
$N_2\left(g\right)+3H_2\left(g\right)\rightleftharpoons 2N{H}_3\left(g\right)$
At equilibrium, the concentration of $N{H}_3,H_2$ and $N_2$ are $1.2\times {10}^{-2},3.0\times {10}^{-2}$ and $1.5\times {10}^{-2}M$ respectively.

Q. An equilibrium mixture of $N_2,H_2$ and $N{H}_3$ at $700$K contains $0.036$M $N_2$ and $0.15$M $H_2$. At this temperature, $K_c$ for the reaction $N_2\left(g\right)+3H_2\left(g\right)\rightleftharpoons 2N{H}_3\left(g\right)$ is $0.29$. What is the concentration of $N{H}_3$?