Partial Pressure

[Luc Zelissen 1K]

A sample of ozone,O3, amounting to 0.10 mol, is placed in a sealed container of volume 1.0 L and the reaction is allowed to reach equilibrium.Then 0.50 mol O3 is placed in a second container of volume 1.0 L at the same temperature and allowed to reach equilibrium.

Question: Will the partial pressures be different even if the initial amounts of reactants are different?

[Ryan Chang 1C]

The partial pressures will be different. In this case, the partial pressure in the second container will be higher. Keeping in mind that K = products/reactants, since K must remain a constant, the partial pressure of the product O2 must be higher to match the higher partial pressure of the reactant O3.

[Vincent Leong 2B]

Remember that the only thing that remains constant is the equilibrium constant value. As long as you put the reaction under the same testing conditions (which should be constant temp) the equilibrium constant will remain the same. Do the ICE table to reason how initial amounts eventually affect the concentrations/partial pressures of all reactants and products at equilibrium

[Matthew Tsai 2H]

Yes, in this case the partial pressures would be different because the moles of gas are different but the volume of the containers that they are in is the same.