For the reaction,$PCl_{3(g)} + Cl_{2(g)} \rightleftharpoons PCl_{5(g)}$,the value of $K_c$ at $250 \ ^oC$ is $26$. The value of $K_p$ at this temperature will be:

For the reaction $PCl_{3(g)} + Cl_{2(g)} \rightleftharpoons PCl_{5(g)}$ at $250 \ ^oC$,the value of $K_c$ is $26$. The value of $K_p$ at the same temperature is .........

For $NH_4HS_{(s)} \rightleftharpoons NH_{3_{(g)}} + H_2S_{(g)}$; the observed pressure for the reaction mixture at equilibrium is $1.12 \ atm$ at $106 \ ^oC$. The value of $K_p$ for the reaction is: (in $atm^2$)

$2 SO_{2(g)} + O_{2(g)} \rightleftharpoons 2 SO_{3(g)}$
In an equilibrium mixture,the partial pressures are
$P_{SO_{3}} = 43 \ kPa$,$P_{O_{2}} = 530 \ Pa = 0.53 \ kPa$,and
$P_{SO_{2}} = 45 \ kPa$. The equilibrium constant $K_{p} = ...... \times 10^{-2} \ kPa^{-1}$. (Nearest integer)

For a reaction $aA_{(g)} \rightleftharpoons bB_{(g)}$ at equilibrium,the heat of reaction at constant volume is $1500 \text{ cal}$ more than that at constant pressure. If the temperature is $27^\circ\text{C}$,then:

For the equilibrium $N_2O_{4(g)} \rightleftharpoons 2NO_{2(g)}$,$K_p$ is equal to $K_c$ when $T = ....... \ K$.