`AB_(2)` dissociates as
`AB_(2)(g) hArr AB(g)+B(g)`. If the initial pressure is `500` mm of Hg and the total pressure at equilibrium is `700` mm of Hg. Calculate `K_(p)` for the reaction.

A gaseous compound XY_2 dissociates as: XY_2(g) hArr XY(g) + Y(g) If the initial pressure is 500 mm of Hg and the total pressure at equilibrium is 700 mm of Hg, calculate K_p for the reaction.

AB_(2) dissociates as : AB_(2 (g)) hArr AB_((g)) + B_((g)) When the intial pressure of AB_(2) is 500 mm Hg , the total equilibrium pressure is 700 mm Hg . Calculate equilibrium constant for the reaction , assuming that the volume of the system remains unchanged .

XY_(2) dissociates XY_(2)(g) hArr XY(g)+Y(g) . When the initial pressure of XY_(2) is 600 mm Hg, the total equilibrium pressure is 800 mm Hg. Calculate K for the reaction Assuming that the volume of the system remains unchanged.

XY_(2) dissociates XY_(2)(g) hArr XY(g)+Y(g) . When the initial pressure of XY_(2) is 600 mm Hg, the total equilibrium pressure is 800 mm Hg. Calculate K for the reaction Assuming that the volume of the system remains unchanged.

XY_(2) dissociates XY_(2)(g) hArr XY(g)+Y(g) . When the initial pressure of XY_(2) is 600 mm Hg, the total equilibrium pressure is 800 mm Hg. Calculate K for the reaction Assuming that the volume of the system remains unchanged.

XY_2 dissociates as XY_2(g) iff XY(g) + Y(g) . When the initial pressure is 600 mm of Hg, the total pressure at equilibrium developed is 800 mm of Hg. Therefore pressure of Y at equilibrium is