Le Chatelier’s Principle Flashcards

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State Le Chatelier's Principle in simple words.

If a system is at equilibrium and you change the conditions, the equilibrium moves to oppose the change and a new equilibrium is set up.

At equilibrium, what happens if you add more reactant, according to Le Chatelier's Principle?

The position of equilibrium moves to the right, towards the products, to use up some of the extra reactant.

At equilibrium, what happens if you remove some product, according to Le Chatelier's Principle?

The position of equilibrium moves to the right, making more product to replace what was removed.

For a reaction that is exothermic in the forward direction, what happens if you increase the temperature?

The equilibrium moves to the left, towards the endothermic direction, so less product is formed.

For a reaction that is exothermic in the forward direction, what happens if you decrease the temperature?

The equilibrium moves to the right, towards the exothermic direction, so more product is formed.

In a gaseous equilibrium, what does Le Chatelier's Principle predict if you increase the pressure?

The equilibrium moves to the side with fewer gas molecules, to reduce the pressure.

In a gaseous equilibrium, what does Le Chatelier's Principle predict if you decrease the pressure?

The equilibrium moves to the side with more gas molecules, to increase the pressure again.

Does adding a catalyst change the position of equilibrium, according to Le Chatelier's Principle?

No. A catalyst speeds up both the forward and backward reactions equally, so the position of equilibrium does not change.

What is meant by 'equilibrium shifts to the right' when using Le Chatelier's Principle?

The forward reaction is favoured, so more products are formed and fewer reactants remain.

How does Le Chatelier's Principle help choose conditions for an industrial reaction?

It helps predict how changes in temperature, pressure and concentration will affect the yield, so conditions can be chosen to make more product.

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