For the exothermic reaction PCl3(g)+Cl2(g)?PCl5(g) Kp = 0.200 at a certain temperature. A flask is charged with 0.500...

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Chemistry

For the exothermic reaction

PCl3(g)+Cl2(g)?PCl5(g)

Kp = 0.200 at a certain temperature.

A flask is charged with 0.500 atm PCl3 , 0.500atm Cl2, and 0.300 atm PCl5 at this temperature.

What are the equilibrium partial pressures of PCl3, Cl2, and PCl5, respectively?

Express your answers numerically in atmospheres with threedigits after the decimal point, separated by commas.

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4.0 Ratings (789 Votes)

For the reaction,

Kp = 0.200

initial,

PCl3 = Cl2 = 0.5 atm

PCl5 = 0.3 atm

ICE chart

            PCl3(g) + Cl2(g) <==> PCl5(g)

I             0.5          0.5                0.3

C           -x            -x                  +x

E          0.5-x      0.5-x             0.3+x

So,

Kp = [PCl5]/[PCl3][Cl2]

0.200 = (0.3+x)/(0.5-x)(0.5-x)

0.05 - 0.2x + 0.2x^2 = 0.3 + x

0.2x^2 - 1.2x - 0.25 = 0

x = -0.2025 atm

at equilibrium,

partial pressure of PCl3 = 0.5 + 0.2025 = 0.702 atm

partial pressure of Cl2 = 0.5 + 0.2025 = 0.702 atm

partial pressure of PCl5 = 0.3 - 0.2025 = 0.097 atm


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