Inert Gas and Le Chatliers
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Re: Inert Gas and Le Chatliers
An inert gas doesn't react with the reactants so it does not change the concentration or the reaction in any way since it also does not change the volume.
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Re: Inert Gas and Le Chatliers
Although adding an inert gas will increase the pressure of a system, the partial pressures of the reactive gases are not changing because the volume has stayed the same. Therefore, K stays the same and there is no shift in the system.
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Re: Inert Gas and Le Chatliers
Michael Nguyen 1E wrote:Although adding an inert gas will increase the pressure of a system, the partial pressures of the reactive gases are not changing because the volume has stayed the same. Therefore, K stays the same and there is no shift in the system.
so do we not have to be concerned about the change in pressure either? will adding an inert gas break equilibrium?
Re: Inert Gas and Le Chatliers
Adding an inert gas to a system in equilibrium at constant volume doesn't effect the equilibrium. However, when adding an inert gas to a system in equilibrium at constant pressure the the total volume will increase.
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Re: Inert Gas and Le Chatliers
If you had Cl- as an inert gas it would be Cl- on the reactant side and Cl- on the product side. If you add this into the chemical equilibrium constant equation, the concentration of Cl- will be on the top and bottom of the division sign, so they will simply cancel each other out.
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Re: Inert Gas and Le Chatliers
805307623 wrote:Adding an inert gas to a system in equilibrium at constant volume doesn't effect the equilibrium. However, when adding an inert gas to a system in equilibrium at constant pressure the the total volume will increase.
I'm kinda confused here; won't the rate of the reaction change if there is an inert gas because the reactants now have to undergo collisions with the inert gas as well? Does that not affect the equilibrium?
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Re: Inert Gas and Le Chatliers
inert gases don't react with the reactants so they ultimately don't consume the partial pressure or the concentration of the reactants. The fact that partial pressure of the reactants (which directly impacts the K constant) is not effected, the K constant is therefore not effected.
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