At $T(\mathrm{~K}), K_c$ value of $A \mathrm{O}_2(g)+B \mathrm{O}_2(g) \rightleftharpoons A \mathrm{O}_3(g)+B O(g)$ is 16 . In a closed 1 L flask, one mole each of $A O_2, B O_2 A \mathrm{O}_3$ and $B \mathrm{O}$ are taken and heated to $T(\mathrm{~K})$. Identify the correct statements about this equilibrium.

I. Total number of moles at equilibrium is 4 .

II. At equilibrium, the ratio of moles of $A \mathrm{O}_2$ and $A \mathrm{O}_3$ is $1: 4$.

III. Total number of moles of $A \mathrm{O}_2$ and $B \mathrm{O}_2$ at equilibrium is 0.8 .

Consider the following equilibrium reaction in gaseous state at $T(\mathrm{~K})$.

$$ A+2 B \rightleftharpoons 2 C+D $$

The initial concentration of $B$ is 1.5 times that of $A$. At equilibrium, the concentrations of $A$ and $B$ are equal. The equilibrium constant for the reaction is

For the following given equilibrium reaction $\frac{K_c}{K_p}$ is equal to 1076 at $T(\mathrm{~K})$. What is the value of $T$ (in K )?

$$ \begin{aligned} & \left(R=0.082 \mathrm{~L}-\mathrm{atm} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\right) \\ & \mathrm{N}_2(\mathrm{~g})+3 \mathrm{H}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NH}_3(\mathrm{~g}) \end{aligned} $$

At $T(\mathrm{~K})$, consider the following gaseous reaction, which is in equilibrium.

$$ \mathrm{N}_2 \mathrm{O}_5 \rightleftharpoons 2 \mathrm{NO}_2+\frac{1}{2} \mathrm{O}_2 $$

What is the fraction of $\mathrm{N}_2 \mathrm{O}_5$ decomposed at constant volume and temperature, if the initial pressure is 300 mm Hg and pressure at equilibrium is 480 mm Hg ? (Assume all gases as ideal)