$1 \ mole$ of $HI$ is heated in a closed container of capacity $2 \ L$. At equilibrium,half a mole of $HI$ is dissociated. The equilibrium constant of the reaction is

For the reactions:
$2NO + O_2 \rightleftharpoons 2NO_2$; $K_1$
$4NO + 2Cl_2 \rightleftharpoons 4NOCl$; $K_2$
$NO_2 + \frac{1}{2}Cl_2 \rightleftharpoons NOCl + \frac{1}{2}O_2$; $K_3$
Where $K_1, K_2, K_3$ are equilibrium constants,then $K_3^2$ is equal to:

For the reaction $C_{(s)} + CO_{2(g)} \rightleftharpoons 2CO_{(g)}$,at equilibrium,$P_{CO_2} = 2$ and $P_{CO} = 4$. The value of $K_p$ is:

The partial pressures of $CH_3OH$,$CO$ and $H_2$ in the equilibrium mixture for the reaction $CO(g) + 2H_2(g) \rightleftharpoons CH_3OH(g)$ at $427 \ ^oC$ are $2.0 \ atm$,$1.0 \ atm$ and $0.1 \ atm$ respectively. The value of $K_P$ for the decomposition of $CH_3OH$ to $CO$ and $H_2$ is:

For the given equilibrium reaction $H_{2(g)} + I_{2(g)} \rightleftharpoons 2 HI_{(g)}$,choose the correct equation to calculate $K_p$.

For which of the following equilibria are $K_P$ and $K_C$ different?