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At a particular temperature, Kp = 0.26 for the reaction below. N2O4(g) equilibrium reaction arrow 2...

At a particular temperature, Kp = 0.26 for the reaction below. N2O4(g) equilibrium reaction arrow 2 NO2(g) (a) A flask containing only N2O4 at an initial pressure of 4.9 atm is allowed to reach equilibrium. Calculate the equilibrium partial pressures of the gases. b) he volume of the container in part (a) is decreased to one-half the original volume. Calculate the new equilibrium partial pressures.

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Answer #1

a)

N2O4 (g) <----------------> 2 NO2 (g)

4.9 atm                                  0

4.9 - x                                    2x

Kp = (2x)^2 / (4.9 - x)

0.26 = 4x^2 / 4.9 - x

x = 0.533

equilibrium partial pressures :

PNO2 = 2x = 1.07 atm

PN2O4 = 4.9 - x = 4.37 atm

b)

new equilibrium pressures

PNO2 = 2.14 atm

PN2O4 = 8.73 atm

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