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

At $380 \ K$,$NH_4HS$ decomposes and the total pressure is $1.12 \ bar$. Find $K_p$ for the reaction: $NH_4HS_{(s)} \rightleftharpoons NH_{3(g)} + H_2S_{(g)}$ (in $bar^2$)

For the equilibrium system $A_{(s)} \rightleftharpoons 2B_{(g)} + 3C_{(g)}$,if the concentration of $C$ is doubled at equilibrium,then the concentration of $B$ at equilibrium will become ...

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

At $1050 \ K$,for the chemical reaction $FeO_{(s)} + CO_{(g)} \rightleftharpoons Fe_{(s)} + CO_{2_{(g)}}$; $K_p = 0.25$. What are the equilibrium partial pressures of $CO_{(g)}$ and $CO_{2_{(g)}}$ at $1050 \ K$,if the initial partial pressures are: $P_{CO_{(g)}} = 1.6 \ atm$ and $P_{CO_{2_{(g)}}} = 0.8 \ atm$?