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Today i will help you to solve this kind of question ” what are the equilibrium partial pressures of pcl3 , cl2, and pcl5, respectively?”. Let’s follow each step carefully to know how to do and understand the way to solve this work in the most through way.

## Question

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.*

An Equilibrium Study: Phosphorus Trichloride/Phosphorus Pentachloride Equilibrium

For the exothermic reaction

PCl3(g)+Cl2(g)→PCl5(g)

*K*p = 0.180 at a certain temperature.

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

## Answer

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## Relevant knowledge

The equilibrium constant, in terms of partial pressure, is the ratio of equilibrium partial pressure of products to equilibrium partial pressure reactants. Each term of the partialpressure must be raised to the power of stoichiometric coeffient of balanced chemical reaction. The equilibrium constant does not include both liquid and solid species.

## Conclusion

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