Equilibrium Le Chatelier’s Principle. Equilibrium Brown gasColourless gas.

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Equilibrium Le Chatelier’s Principle

Transcript of Equilibrium Le Chatelier’s Principle. Equilibrium Brown gasColourless gas.

Page 1: Equilibrium Le Chatelier’s Principle. Equilibrium Brown gasColourless gas.

Equilibrium

Le Chatelier’s Principle

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Equilibrium

Brown gasColourless gas

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Equilibrium

Imagine we begin with a container that has only N2O4 gas. Some of these molecules will successfully collide and produce NO2.

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Equilibrium

The colour of the gas mixture will get browner as less N2O4 and more NO2 will be present, until equilibrium is achieved.

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Equilibrium

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Equilibrium

At equilibrium there will be NO2 and N2O4 present. The colour of the mixture will be determined by the amount of NO2 present.

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Equilibrium

At equilibrium the macroscopic properties, such as pressure and colour will be constant.

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Equilibrium

At equilibrium the forward and reverse reactions will both be occurring.

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Equilibrium

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Equilibrium expression

An equilibrium expression gives an indication of the relative amounts of products to reactants at equilibrium.

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Equilibrium expression

For this reaction the equilibrium expression is:

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Equilibrium expression

The square bracket represents concentration.

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Equilibrium expressionSolids and liquids do not have a concentration and therefore would not be included in the expression.

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Equilibrium expressionAny co-efficient in the balanced equation appears as an indice in the equilibrium expression.

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Equilibrium expression

The value for this particular reaction, at 100oC is always 0.21.

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Le Chatelier’s PrincipleIf a sy stem at eq u i l ibriu m has a chan g e im posed on i t, then the sy stem wi l l partial ly oppose the chan g e in su ch a way as to re-establ ish the eq u i l ibriu m .

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Le Chatelier’s Principle

If the equilibrium concentrations were

[NO2] = 0.205, [N2O4] = 0.2

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Le Chatelier’s Principle

and we added more N2O4 to bring it’s concentration up to 0.3 mol L-1. The system would adjust to get back to where K = 0.21

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Le Chatelier’s Principle

This would happen by trying to get the [N2O4] partially back to its original value. At the same time the [NO2] would increase.

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Le Chatelier’s Principle

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Le Chatelier’s Principle

The concentrations of each at the new equilibrium are:

[NO2] = 0.245 mol L-1

[N2O4] = 0.28 mol L-1

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Le Chatelier’s Principle

If at these new concentrations the volume of the container was halved:

What would be the new concentrations?

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Le Chatelier’s Principle

If at these new concentrations the volume of the container was halved:

What would happen to the pressure in the container?

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Le Chatelier’s Principle

When pressure increases Le Chatelier’s principle says that the system will try to partially restore the original pressure.

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Le Chatelier’s Principle

This could be achieved by favouring the reaction which produces fewer gas molecules. ie reverse reaction

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Le Chatelier’s Principle

0oCroom temp

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Le Chatelier’s Principle

Lowering the temperature favours the reverse reaction, since the mixture gets lighter in colour.

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Le Chatelier’s PrincipleWhy?

What does Le Chatelier predict will happen when you lower the temperature of a system.

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Le Chatelier’s PrincipleThe principle predicts that the reaction will try and increase the temperature. It can do this by producing heat. ie an exothermic reaction would be favoured.

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Le Chatelier’s PrincipleThe reaction will attempt to re- establish its original equilibrium but will not be able to . The equilibrium constant for a reaction is only constant at one temperature.

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Le Chatelier’s PrincipleAt room temperature

At zero degrees

[N2O4] 0.049 0.098

[NO2] 0.102 0.005

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Le Chatelier’s Principle


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Le Chatelier’s Principle “If a system in equilibrium is subjected to a stress, a change that will offset the stress will occur in the system.”

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