question: an equilibrium mixture contains N2O4 (P=0.27 atm) and NO2 (P=1.2 atm) at 350K. the volume is doubled at constant temperature. calculate the equilibrium pressure of both at new equilibrium. what i know: when you double volume, pressure is halved and le chatliers principle says the equation will shift to the side with more moles of gas: N2O4 <--> 2NO2 which in this case will shift to the right. and i also know you cannot simply just half the pressures of each. how do i start the rest of this problem? is it an ICE problem? any help to get started would be appreciated. thanks.