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# Dynamic equilibrium and le chatelier's principle? watch

1. I'm confused with way the equilibrium moves and why, with changes in
Concentration
Temperature
Pressure.

Please clarify this for me, my textbook appears to contradict itself ( or perhaps it's me..I don't know)
2. (Original post by Questioness)
I'm confused with way the equilibrium moves and why, with changes in
Concentration
Temperature
Pressure.

Please clarify this for me, my textbook appears to contradict itself ( or perhaps it's me..I don't know)
Le chatelielier principle states that if a system is at equilibrium and a change is made in any of the conditions then the system will respond to minimize the change.

Therefore if the forward reaction is exothermic and you increase temperature the the reverse reaction wll be favored to "use up the extra heat" (temperature increase favors the endothermic reaction.)

Increasing the pressure will favor the side with fewer gas molecules.
Decreasing the pressure will favor the side of the reaction with More gas molecules.

Increasing the contraction of reactants with cause the equilibrium position to move in the direction of the products. (To decrease the the amount of reactant minimizing the change)

The opposing arguments are also true.
3. (Original post by Questioness)
I'm confused with way the equilibrium moves and why, with changes in
Concentration
Temperature
Pressure.

Please clarify this for me, my textbook appears to contradict itself ( or perhaps it's me..I don't know)
Well firstly, understanding what La Chatelieurs principle means will help. The principle is if a system in equilibirium is exposed to change the equilibrium will act to oppose that change.

So for temperature if the right side is endothermic, that means the left side will be endothermic. Therefore when we increase the temperature La Chatelieurs principle tells us that equilibirum moves to oppose the change therefore, yield on the left increases since its endothermic. Just think how to oppose change.
4. (Original post by Questioness)
I'm confused with way the equilibrium moves and why, with changes in
Concentration
Temperature
Pressure.

Please clarify this for me, my textbook appears to contradict itself ( or perhaps it's me..I don't know)
Le Chatelier's principle states that; "When the position of equilibrium is subjected to a change, the position of equilibrium will shift to minimise the change''.

Dynamic equilibrium is when the forward reaction is equal to the reverse reaction, and the concentrations of products and reactants do not change.

When you are asked questions relating to temperature, you will be given an enthaply value. If the value is negative, the reaction is exothermic, meaning that the molecules will shift to minimise the change by absorbing energy(endothermic reaction).

Concentration and pressure contains the same answer. You will have to look at the side that contains the most number of moles for the pressure and most number of reactants in the concentration. Basically, the side with the greatest mole/concentration will shift to the side with fewer molecules.

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Updated: April 27, 2016
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