For a gasous reaction, `2A+B hArr 2C`, the partial pressures of A,B and C at equilibrium are 0.3 atm, 0.4 atm and 0.6 atm respectively. The value of `K_P` for the reaction would be :

For a reaction 2A+B hArr C+D , the partial pressures of A, B , C and D at equilibrium are 0.5, 0.8, 0.7 and 1.2 atmospheres respectively. The value of K_(p) for this reaction is

For the reaction A_(2)(g) + 2B_(2)hArr2C_(2)(g) the partial pressure of A_(2) and B_(2) at equilibrium are 0.80 atm and 0.40 atm respectively. The pressure of the system is 2.80 atm. The equilibrium constant K_(p) will be

For the reaction A_(2)(g) + 2B_(2)hArr2C_(2)(g) the partial pressure of A_(2) and B_(2) at equilibrium are 0.80 atm and 0.40 atm respectively.The pressure of the system is 2.80 atm. The equilibrium constant K_(p) will be

For the reaction C(s) + CO_(2) (g) hArr 2CO(g). the partial pressures of CO_(2) and CO are 2.0 and 4.0 atm respectively at equilibrium. What is the value of K_(p) for this reaction?

For a gaseous equilibrium, A +2B hArr C + 3D the partial pressures of A, B, C and D are found to be 0.20, 0.10, 0.30 and 0.50 atm respectively. Predict the value of equilibrium constant.

In the reversible gaseous reaction , A + 2B hArr C+3D The partial pressure of A B C and D are 0.20 , 0.10 , 0.30 ,0.50 atm respectively at equilibrium. The numerical value of K_p is :

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 a C(s) + CO_2(g) hArr 2CO(g) , the partial pressure of CO_2 and CO are 2.0 and 4.0 atm respectively at equilibrium. The K_p for 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 is 2.0 and 4.0 atm, respectively, at equilibrium. The K_(p) of the reaction is