The reaction `AB_(2)`(g) `harr` A(g)+ 2B(g) is studied in a "10" -litre flask. Initially there is "0.40" mole of `AB_(2)` .After the introduction of the catalyst, at `27^(@)C` ,equilibrium is reached, the pressure of the mixture is 1.2 atm.The degree of dissociation is

A homogeneous ideal gaseous reaction AB_(2(g)) ƒhArr A_((g)) + 2B_((g)) is carried out in a 25 litre flask at 27^@ C. The initial amount of AB_2 was 1 mole and the equilibrium pressure was 1.9 atm. The value of K_P is x xx 10^(-2) . The value of x is______.(Integer answer)

For the reaction , N_2O_4(g)hArr2NO_2(g) the degree of dissociation at equilibrium is 0.4 at a pressure of 1 atm. The value of K_p is

For the reaction, N_(2)O_(4)(g)hArr 2NO_(2)(g) the degree of dissociation at equilibrium is 0.14 at a pressure of 1 atm. The value of K_(p) is

In the reaction AB(g) hArr A(g) + B(g) at 30^(@)C, k_(p) for the dissociation equilibrium is 2.56xx10^(-2) atm . If the total pressure at equilibrium is 1 atm, then the percentage dissociation of AB is

For reaction 2NO(g)hArr N_(2)(g)+O_(2)(g) degree of dissociation of N_(2) and O_(2) is x. Initially 1 mole of NO is taken then number of moles of O_(2) at equilibrium is