AP Chem

At a particular temperature, Kp = 0.25 for the following reaction.
N2O4(g) 2 NO2(g)

(a) A flask containing only N2O4 at an initial pressure of 5.3 atm is allowed to reach equilibrium. Calculate the equilibrium partial pressures of the gases.

(b) A flask containing only NO2 at an initial pressure of 7.0 atm is allowed to reach equilibrium. Calculate the equilibrium partial pressures of the gases.

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  1. You should get into the habit of using an arrow; otherwise we must guess which are products and which are reactants.
    ..........N2O4 ==> 2NO2
    initial....5.3atm....0
    change.....-p.....2p
    equil..... 5.3-p....2p

    Kp = 0.25 = (NO2O^2/(N2O4)
    Substitute from the ICE chart into Kp expression and solve for p.
    Then 2p = PNO2 and 5.3-p = PN2O4.

    For #2,
    ...........N2O4 ==> 2NO2
    initial......0........7
    change......+p........-p
    equil........p.......7-p
    Substitute into Ka and solve for p.

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