Question

In: Chemistry

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

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 , 0.500 atm 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 three digits after the decimal point, separated by commas.

Solutions

Expert Solution

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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