In which of the following equilibria,the value of $K_p$ is less than $K_c$?

For the following reaction in gaseous phase $CO_{(g)} + \frac{1}{2} O_{2(g)} \to CO_{2(g)}$,$K_p/K_c$ is

For the decomposition of the compound,represented as $NH_2COONH_{4(s)} \rightleftharpoons 2NH_{3(g)} + CO_{2(g)}$,the $K_p = 2.9 \times 10^{-5} \ atm^3$. If the reaction is started with $1 \ mol$ of the compound,the total pressure at equilibrium would be............ $\times 10^{-2} \ atm$.

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 formation of ammonia gas from its constituent elements,the $K_{P} / K_{C}$ is

In which one of the following gaseous equilibria is $K_p$ less than $K_c$?