For the reaction $AB_{(g)} \rightleftharpoons A_{(g)} + B_{(g)}$,$AB$ is $33.3\%$ dissociated at a total equilibrium pressure of $P$. Therefore,$P$ is correctly related to $K_p$ by which of the following options?

For the reaction $SnO_{2(s)} + 2H_{2(g)} \rightleftharpoons 2H_2O_{(g)} + Sn_{(l)}$,at equilibrium,the mixture of steam and hydrogen contains $40\%$ $H_2$ by volume. Find $K_p$ for the reaction.

$3.00 \, mol$ of $PCl_5$ kept in $1 \, L$ closed vessel was allowed to attain equilibrium at $380 \, K$. If $K_C = 1.80$,calculate the equilibrium concentrations of $PCl_3$ and $Cl_2$ respectively.

Given $K_p$ for the reaction $\frac{1}{2} C_{(g)} \rightleftharpoons \frac{1}{2} A_{(g)} + \frac{1}{2} B_{(g)}$ at a fixed temperature is $0.25 \ atm$. Find the $K_p$ for the reaction $A_{(g)} + B_{(g)} \rightleftharpoons C_{(g)}$ at the same temperature.

The ratio $\frac{K_p}{K_C}$ for the reaction: $CO_{(g)} + \frac{1}{2} O_{2(g)} \rightleftharpoons CO_{2(g)}$ is:

Consider the following equilibrium,$CO_{(g)} + 2H_{2(g)} \rightleftharpoons CH_3OH_{(g)}$. $0.1 \ mol$ of $CO$ along with a catalyst is present in a $2 \ dm^3$ flask maintained at $500 \ K$. Hydrogen is introduced into the flask until the pressure is $5 \ bar$ and $0.04 \ mol$ of $CH_3OH$ is formed. The $K_{p}^0$ is $......... \times 10^{-3}$ (nearest integer). Given: $R = 0.08 \ dm^3 \ bar \ K^{-1} \ mol^{-1}$. Assume only methanol is formed as the product and the system follows ideal gas behaviour.