Partial pressures of $A$,$B$,$C$,and $D$ for the gaseous system $A + 2B \rightleftharpoons C + 3D$ are $A = 0.20 \ atm$,$B = 0.10 \ atm$,$C = 0.30 \ atm$,and $D = 0.50 \ atm$. The numerical value of the equilibrium constant $(K_p)$ is:

For the chemical equilibrium,$CaCO_{3_{(s)}} \rightleftharpoons CaO_{(s)} + CO_{2_{(g)}}$,$\Delta H_{r}^{\circ}$ can be determined from which one of the following plots?

For the reaction $PCl_{5(g)} \rightleftharpoons PCl_{3(g)} + Cl_{2(g)}$,what is the relationship between $K_p$ and $K_c$?

$CoO_{2(g)} + H_{2(g)} \rightleftharpoons CoO_{(s)} + H_2O_{(g)} \,;\, K_1 = 67$
$CoO_{2(g)} + CO_{(g)} \rightleftharpoons CoO_{(s)} + CO_{2(g)} \,;\, K_2 = 490$
Then the equilibrium constant for the following reaction is ....
$CO_{2(g)} + H_{2(g)} \rightleftharpoons CO_{(g)} + H_2O_{(g)}$

If equilibrium constants of the reaction,$N_2 + O_2 \rightleftharpoons 2NO$ is $K_1$ and $\frac{1}{2}N_2 + \frac{1}{2}O_2 \rightleftharpoons NO$ is $K_2$,then:

The equilibrium constant at $850 \ K$ for the reaction $N_{2(g)} + O_{2(g)} \rightleftharpoons 2 NO_{(g)}$ is $0.5625$. The equilibrium concentration of $NO_{(g)}$ is $3.0 \times 10^{-3} \ M$. If the equilibrium concentrations of $N_{2(g)}$ and $O_{2(g)}$ are equal,the concentration of $N_{2(g)}$ in $M$ is