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, N_(2)(g)+3H_(2)(g) hArr 2NH_(3)(g) the partial pressure of N_(2) and H_(2) are 0.80 and 0.40 atmosphere, respectively, at equilibrium. The total pressure of the system is 2.80 atm. What is K_(p) for the above reaction?

For the reaction, N_(2)(g)+3H_(2)(g) hArr 2NH_(3)(g) the partial pressure of N_(2) and H_(2) are 0.80 and 0.40 atmosphere, respectively, at equilibrium. The total pressure of the system is 2.80 atm. What is K_(p) for the above reaction?

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 the reaction at 127^@ C N_2(g) + 3H_2(g) hArr 2NH_3(g) the partial pressures of N_2 and H_2 are 0.80 and 0.40 atm respectively at equilibrium. The total pressure of the system is 2.80 atm. Calculate K_p and K_c for the reaction.

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 2.0 and 4.0 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 2.0 and 4.0 atm, respectively, at equilibrium. The K_(p) of the reaction is