At 298 K , the value of $K_c$ for the following reaction is $x \mathrm{~mol} \mathrm{~L}^{-1}$.

What is the approximate $K_{\mathrm{P}}$ value for this reaction?

$$ \begin{array}{r} \left(R=0.082 \mathrm{~L} \mathrm{~atm} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}\right) \\ \mathrm{A}_2 \mathrm{O}_4(\mathrm{~g}) \rightleftharpoons 2 \mathrm{AO}_2(\mathrm{~g}) \end{array} $$

At $293 \mathrm{~K}, \Delta_r G^{\circ}$ for the following reaction is $165.469 \mathrm{~kJ} \mathrm{~mol}^{-1}$.

$$ \frac{3}{2} \mathrm{O}_2(\mathrm{~g}) \longrightarrow \mathrm{O}_3(\mathrm{~g}) $$

What is the equilibrium constant for this reaction?

$$ \left(R=83 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}\right) $$

The following equilibrium is established at STP.

$$ B_2(g) \rightleftharpoons 2 B(g) $$

Atoms of $B$ occupy $20 \%$ of total volume at STP. The total pressure of the system is 1 bar. What is its $K_p$ ? $($ STP volume $=22.7 \mathrm{~L})$

At $300 \mathrm{~K}, K_C$ for the reaction. $$ A_2 B_2(g) \rightleftharpoons A_2(g)+B_2(g) $$ is $100 \mathrm{~mol} \mathrm{~L}^{-1}$, What is its $K_p$ (in atm ) at the same temperature ? $\left(R=0.082 \mathrm{~L} \mathrm{~atm} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}\right)$