# Problem: What are the equilibrium partial pressures of PCl3 , Cl2, and PCl5, respectively?For the exothermic reaction PCl3(g)+Cl2(g) →  PCl5(g) Kp = 0.100 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.

###### FREE Expert Solution

We are being asked to calculate the equilibrium partial pressures for the given reaction:

PCl3(g)+Cl2(g) →  PCl5(g) Kp = 0.100

When dealing with equilibrium and Kp:

Kp → equilibrium units in terms of pressure
Kp is an equilibrium expression:

$\overline{){{\mathbf{K}}}_{{\mathbf{p}}}{\mathbf{=}}\frac{\mathbf{products}}{\mathbf{reactants}}}$

only gaseous species are included in the equilibrium expression
▪ the coefficient of each compound in the reaction equation will be the exponent of the pressures in the equilibrium expression

Given:

99% (18 ratings) ###### Problem Details

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

For the exothermic reaction PCl3(g)+Cl2(g) →  PCl5(g) Kp = 0.100 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.