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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.
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.