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)

At 298 K , the value of $K_p$ for $\mathrm{N}_2 \mathrm{O}_4(g) \rightleftharpoons 2 \mathrm{NO}_2(g)$ is 0.113 atm . The partial pressure of $\mathrm{N}_2 \mathrm{O}_4$ at equilibrium is 0.2 atm . What is the partial pressure (in atm) of $\mathrm{NO}_2$ equilibrium?

Consider the following gaseous equilibrium reactions (I), (II) and (III) with equilibrium constants $K_1, K_2$ and $K_3$ respectively

(I) $\frac{1}{2} \mathrm{~N}_2+\frac{3}{2} \mathrm{H}_2 \rightleftharpoons \mathrm{NH}_3$

(II) $2 \mathrm{NO} \rightleftharpoons \mathrm{N}_2+\mathrm{O}_2$

(III) $\mathrm{H}_2+\frac{1}{2} \mathrm{O}_2 \rightleftharpoons \mathrm{H}_2 \mathrm{O}$

The correct expression for the equilibrium constant for the gaseous equilibrium reaction

$$ 2 \mathrm{NH}_3+\frac{5}{2} \mathrm{O}_2 \rightleftharpoons 2 \mathrm{NO}+3 \mathrm{H}_2 \mathrm{O} \text { is } $$