Calculate the equilibrium constant `K_(p)` and `K_(c )` for the reaction: `CO(g)+1//2O_(2)(g) hArr CO_(2)(g)`. Given that the partial pressure at equilibrium in a vessel at `3000 K` are `p_(CO)=0.4 atm, p_(CO_(2))=0.2 atm`

Calculate the equilibrium constant K_(p) and K_(c ) for the reaction: CO(g)+1//2O_(2)(g) hArr CO_(2)(g) . Given that the partial pressure at equilibrium in a vessel at 3000 K are p_(CO)=0.4 atm, p_(CO_(2))=0.6 atm pO2=0.2 atm

Calculate the equilibrium constants K_(p) and K_(c) for the reaction , CO (g) + 1//2 O_(2) (g) hArr CO_(2) Given that the partial pressures at equilibrium in a vessel at 3000 K are p_(co) = 0.4" atm ". p_(co_(2)) = 0.6 " atm "and p_(o_(2))= 0.2" atm"

K_(p)//K_(c) for the reaction CO(g)+1/2 O_(2)(g) hArr CO_(2)(g) is

K_(p)//K_(c) for the reaction CO(g)+1/2 O_(2)(g) hArr CO_(2)(g) is

K_(p)//K_(c) for the reaction CO(g)+1/2 O_(2)(g) hArr CO_(2)(g) is

K_p/K_c for the reaction: CO(g)+1/2O_2(g) hArr CO_2(g) is :

For the reaction CO(g)+(1)/(2) O_(2)(g) hArr CO_(2)(g),K_(p)//K_(c) is

For the reaction CO(g)+(1)/(2) O_(2)(g) hArr CO_(2)(g),K_(p)//K_(c) is