For the reaction $CO_{(g)} + \frac{1}{2} O_{2(g)} \rightleftharpoons CO_{2(g)}$,the ratio $\frac{K_p}{K_c}$ is equivalent to:

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 equilibrium $SO_2Cl_{2(g)} \rightleftharpoons SO_{2(g)} + Cl_{2(g)}$,what is the temperature at which $\frac{K_p}{K_c} = \frac{1}{3}$? (Given $R = 0.0821 \ L \ atm \ K^{-1} \ mol^{-1}$)

For the reaction $2NO_{2(g)} \rightleftharpoons 2NO_{(g)} + O_{2(g)}$,the equilibrium constant $K_c = 1.8 \times 10^{-6}$ at $184 \, ^\circ C$. Comparing $K_p$ and $K_c$ at $184 \, ^\circ C$,we find that:

For the reactions $N_{2(g)} + O_{2(g)} \rightleftharpoons 2NO_{(g)}$ and $NO_{(g)} \rightleftharpoons 1/2N_{2(g)} + 1/2O_{2(g)}$,the equilibrium constants are $K_1$ and $K_2$ respectively. What is the relationship between $K_1$ and $K_2$?

$1 \ mol$ $N_2$ 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: $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$