When $1 \ mol$ of $H_2$ and $1 \ mol$ of $N_2$ are enclosed in a $5 \ L$ vessel and the reaction is allowed to attain equilibrium,it is found that at equilibrium there is $x \ mol$ of $H_2$. The number of moles of $NH_3$ would be

Consider the following reversible first-order reaction of $X$ at an initial concentration $[X]_{0}$. The values of the rate constants are $K_{f} = 2 \ s^{-1}$ and $K_{b} = 1 \ s^{-1}$.
$X \underset{K_{b}}{\stackrel{K_{f}}{\rightleftharpoons}} Y$
Which of the following plots correctly represents the concentration of $X$ and $Y$ as a function of time?

At equilibrium for the reaction $A_{2(g)} + B_{2(g)} \rightleftharpoons 2 AB_{(g)}$,the concentrations of $A_2$,$B_2$,and $AB$ respectively are $1.5 \times 10^{-3} \ M$,$2.1 \times 10^{-3} \ M$,and $1.4 \times 10^{-3} \ M$ in a sealed vessel at $800 \ K$. What will be $K_p$ for the decomposition of $AB$ at the same temperature?

The dissociation of $CO_2$ is represented as $2CO_2(g) \rightleftharpoons 2CO(g) + O_2(g)$. If $2 \ mol$ of $CO_2$ are taken initially and $40\%$ of $CO_2$ dissociates,what will be the total number of moles at equilibrium?

In reaction $A + 2B \rightleftharpoons 2C + D$,the initial concentration of $B$ was $1.5$ times that of $[A]$,but at equilibrium,the concentrations of $A$ and $B$ became equal. The equilibrium constant for the reaction is:

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.