A sample of N2O4(g) is placed in an empty cylinder at 25oC. After equilibrium is reached, the total pressure is 1.5 atm and 16% (by moles) of the original N2O4 (g) has dissociated to NO2(g). N2O4 (g)2NO2(g) a) Calculate the value of Kp for this dissociation reaction at 25 oC. b)If the volume of the cylinder is increased until the total pressure is 1.0 atm andthe temperature of the system remains constant, calculate the equilibrium pressure of N2O4(g) and NO2(g).