For the reaction ${N_2}_{(g)} + {O_2}_{(g)} \rightleftharpoons 2NO_{(g)}$,the equilibrium constant ${K_C}$ is $4 \times 10^{-4}$ at temperature $T$. Calculate ${K_P}$.

At $413 \ K$ temperature and $100 \ atm$ pressure,$1 \ mol$ $N_2$ and $3 \ mol$ $H_2$ are heated in a closed vessel. At equilibrium,$0.50 \ mol$ $NH_3$ is present. Find $K_p$.

$1 \ mol$ $N_2$ and $3 \ mol$ $H_2$ are heated at $473 \ K$ and $100 \ atm$ pressure. At equilibrium,the number of moles of $NH_3$ is $0.5 \ mol$. Calculate the equilibrium constant $K_p$ of the given reaction: $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$

Calculate the value of the equilibrium constant $(K_p)$ for the reaction of oxygen gas oxidizing ammonia gas to nitric oxide and water vapor. The pressure of each gas at equilibrium is $0.5 \ atm$. (in $atm$)

For the reaction $PCl_5 \, (g) \rightleftharpoons PCl_3 \, (g) + Cl_2 \, (g)$,the two reaction constants $K_p$ and $K_c$ are related to each other by the expression

In a $1 \ L$ closed container,$4 \ moles$ of $PCl_5$ are heated. If $80\%$ of $PCl_5$ remains undissociated at equilibrium,what is the value of the equilibrium constant $(K_c)$?