\(3 \mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{O}_{3}(\mathrm{g}) \) 
For the above reaction at 298 K, \(K_c\) is found to be \(3.0 \times 10^{-59} \). If the concentration of \(O_2\) at equilibrium is 0.040 M, then the concentration of \(O_3 \) in M is: 
1. \(1.2 \times 10^{21} \)
2. \(4.38 \times 10^{-32} \)
3. \(1.9 \times 10^{-63} \)
4. \(2.4 \times 10^{31} \)

Consider the following reaction taking place in 1L capacity container at 300 K.
\(A +B \rightleftharpoons C+D \)
If one mole each of A and B are present initially and at equilibrium 0.7 mol of C is formed, then the equilibrium constant \((K_c) \) for the reaction is

Equilibrium constants K₁ and K₂ for the following equilibria

$\begin{array}{l}\mathrm{NO}\left(\mathrm{g}\right)+\frac{1}{2}{\mathrm{O}}_2\stackrel{{\mathrm{K}}_1}{⟶}{\mathrm{NO}}_2\left(\mathrm{g}\right)\text{ and }\\ 2{\mathrm{NO}}_2\left(\mathrm{g}\right)\stackrel{{\mathrm{K}}_2}{\rightleftharpoons }2\mathrm{NO}\left(\mathrm{g}\right)+{\mathrm{O}}_2\left(\mathrm{g}\right)\end{array}$

are related as:

1. ${\mathrm{K}}_2=\frac{1}{{\mathrm{K}}_1}$

2. ${\mathrm{K}}_2=\frac{{\mathrm{K}}_1}{2}$

3. ${\mathrm{K}}_2=\frac{1}{{\mathrm{K}}_1^2}$

4. ${\mathrm{K}}_2={\mathrm{K}}_1^2$

The following equilibria are given:

The equilibrium constant of the reaction
\(2NH_{3} \ + \ \frac{5}{2}O_{2} \ \rightleftharpoons \ 2NO \ + \ 3H_{2}O\) in terms of K₁, K₂ and K₃ is:

1. K₁.K₂.K₃
2. \(\mathrm{\frac{K_{1}K_{2}}{K_{3}}}\)
3. \(\mathrm{\frac{K_{1}K_{3}^{2}}{K_{3}}}\)
4. \(\mathrm{\frac{K_{2}K_{3}^{3}}{K_{1}}}\)