At a certain temperature , `K_(p)` for dissociation of solid `CaCO_(3)` is `4xx10^(-2)` atm and for the reaction, `C(s)+CO_(2) hArr 2CO` is `2.0` atm, respectively. Calculate the pressure of CO at this temperature when solid `C, CaO, CaCO_(3)` are mixed and allowed to attain equilibrium.

For the reaction : CaCO_(3) (s) hArr CaO (s) + CO_(2) (g)

At 100 k , the pressure of CO_2 in equilibrium with CaCO_3 and CaO is equal to 3.9 xx 10^(-2) atm. The equilibrium constant for the reaction C(s) +CO_2 hArr 2CO(g) , is 1.9 at the same temperature when pressure are in atmospheres, solid carbon CaO and CaCO_3 are instead allowed to come to equilibrium at 100 K in closed vessel . what is the pressure of CO at equilibrium ?

Consider the heterogeneous equilibrium CaCO_3(s) hArr CaO(s) +CO_2(g) k_p=4 xx 10^(-2) atm ……….(i) C(s) +CO_2(g) hArr 2CO(g) K_p=2.0 atm ………(ii) Calculate the partial pressure of CO(g) when CaCO_3 and C are mixed and allowed to attain equilibrium at the temperature for which the above two equilibria have been studied.

Consider the heterogeneous equilibrium CaCO_3(s) hArr CaO(s) +CO_2(g) k_p=4 xx 10^(-2) atm ……….(i) C(s) +CO_2(g) hArr 2CO(g) K_p=2.0 atm ………(ii) Calculate the partial pressure of CO(g) when CaCO_3 and C are mixed and allowed to attain equilibrium at the temperature for which the above two equilibria have been studied.

For the reaction CaCO_(3(s)) hArr CaO_((s))+CO_(2(g))k_p is equal to

For the reaction CaCO_(3(s)) hArr CaO_((s))+CO_(2(g))k_p is equal to

For the reaction C(s)+CO_(2)(g) hArr 2CO(g) , the partial pressure of CO_(2) and CO is 4.0atm amd 8.0 atm, respectively, at equilibrium. The K_(p) of the reaction is

For the reaction C(s)+CO_(2)(g) hArr 2CO(g) , the partial pressure of CO_(2) and CO is 5.0atm amd 10 atm, respectively, at equilibrium. The K_(p) of the reaction is

For the reaction C(s)+CO_(2)(g) hArr 2CO(g) , the partial pressure of CO_(2) and CO both is 4.0 atm, respectively, at equilibrium. The K_(p) of the reaction is