Partial Pressure

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Luc Zelissen 1K
Posts: 57
Joined: Mon Jun 17, 2019 7:23 am

Partial Pressure

Postby Luc Zelissen 1K » Wed Jan 08, 2020 4:10 pm

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
Posts: 105
Joined: Sat Aug 24, 2019 12:17 am

Re: Partial Pressure

Postby Ryan Chang 1C » Wed Jan 08, 2020 5:24 pm

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
Posts: 207
Joined: Fri Aug 09, 2019 12:15 am

Re: Partial Pressure

Postby Vincent Leong 2B » Wed Jan 08, 2020 6:42 pm

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
Posts: 101
Joined: Wed Sep 18, 2019 12:20 am

Re: Partial Pressure

Postby Matthew Tsai 2H » Wed Jan 08, 2020 7:04 pm

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.


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