Question

A 20 litre box contains o3 and o2 at equilibrium at 202k. Kp=2×10^14 for 2o3-->3o2. Assume that po2>>po3 and total pressure is 8 atm the partial pressure of o3 is

Answer 1

We have been given 20 liter box that contains ozone, O3 and oxygen, O2 and they are at equilibrium at 202K. kp is given as 2 x 10^14.

Assumption is that pO2 >> pO3 and the total pressure being 8 atm.

Getting the number of moles of each case;

Equation 2O2 ------------->3O2

 Mole ratio of O3 = 2/5

mole ratio of O2 = 3/5

At equilibrium the number of O3 moles of is 2/5 / 20 = 0.02 moles of O3

moles of O2 at equilibrium is            3/5 /20 = 0.03 moles  

partial pressure of O3 = 0.02/0.05 x 8 = 3.2 atm.