At 3000 K the equilibrium pressures of `CO_(2)` CO and `O_(2)` are `0.6, 0.4` and `0.2` atmospheres respectively. `K_(p)` fot the reaction, `2CO_(2)hArr2CO + O_(2)` is

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

The equilibrium pressure of CO_2 , CO and O_2 for the reaction 2CO_2(g)iff2CO(g)+O_2(g) at 3000K are 0.6, 0.4 and 0.2 atm respectively calculate (i) K_p and (ii) K_c for this reaction at that temperature.

For the reaction C(s)+CO_(2)(g) rarr 2CO(g) an equilibrium mixture has parital pressure, for CO_(2) and CO, of 4.0 and 8.0 atm respectively . K_(p) for the reaction is

When the reaction, 2NO_(2)(g) hArr N_(2)O_(4)(g) reaches equilibrium at 298 K . The partial pressure of NO_(2) and N_(2)O_(4) are 0.2 Kpa and 0.4 Kpa , respectively. What is the equilibrium constant K_(p) of the above reaction at 298 K ?