for the reaction N2O4(g) <--> (equilibrium arrows) 2NO2(g), kp = 0.25 at a certa

Question

for the reaction N2O4(g) <--> (equilibrium arrows) 2NO2(g), kp = 0.25 at a certain temperature. Calculate the equilibrium pressures of NO2(g) and N2SO4(g) if the initial pressures of the components when placed in an otherwise empty container are as follows initial PNO2 = 0.0 atm Initial PN2O4= 0.040 atm Equilibrium PNO2 = ? atm Equilibrium PN2O4 = ? atm How do I go about solving this?

Explanation / Answer

kp = 0.25 =>4x^2/(0.04-x) = 0.25 =>4x^2 = 0.25*0.04-0.25x =>4x^2+0.25x-0.01 = 0 =>x = 0.0277124 So Equilibrium PNO2 = 2*x = 0.0554248 atm Equilibrium PN2O4 = 0.0122876 atm

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