In the reaction `C(s)+CO_(2)(g) hArr 2CO(g)`, the equilibrium pressure is `12` atm. If `50%` of `CO_(2)` reacts, calculate `K_(p)`.

In the reaction C(s) + CO_2(g) hArr 2CO(g) the equilibrium pressure is 12 atm. If 50% OF CO_2 reacts. Calculate the K_P for the change:

In the reaction C_((s)) + CO_(2(g)) hArr CO_(2(g)) , the equilibrium pressure is 6.75 atm. If 50% of CO_(2) reacts then the find value of K_(p) .

In the reaction C_((s))+CO_(2(g))hArr2CO_((g)) , the equilibrium pressure is 6.75 atm . If 50% of CO_(2) reacts, then find the value of K_(p) .

In the reaction : C(s)+CO2(g)⇌2CO(g) , the equilibrium pressure is 6 atm. If 50% of CO2 reacts, then Kp of the reaction is

For the reaction, 0.5 C(s)+0.5CO_(2)(g) hArr CO(g) the equilibrium pressure is 12 atm. If CO_(2) conversion is 50%, the value of K_(p) , in atom is

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