PN2O4 = 0.30 atm

PNO2 = 1.1 atm

Equilibrium constant at 350 K:

Kp = [NO2]^2/[N2O4] = (1.1 atm)^2/0.30 atm = 4.07 atm

At equilibrium, let the partial pressures of N2O4 and NO2 be x atm and y atm, respectively.

Kp = [NO2]^2/[N2O4] = y^2/x = 4.07 atm

Since the volume of the container is doubled, the partial pressures of N2O4 and NO2 will each be halved:

x = PN2O4 = 0.30 atm / 2 = 0.15 atm

y = PNO2 = 1.1 atm / 2 = 0.55 atm

Therefore, the equilibrium pressures are:

PN2O4 = 0.15 atm

PNO2 = 0.55 atm