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:

Kp=productsreactants

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)
View Complete Written Solution
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.

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the ICE Chart concept. You can view video lessons to learn ICE Chart. Or if you need more ICE Chart practice, you can also practice ICE Chart practice problems.