Le Chatelier's Principle

Question 1

What is Le Chatelier’s Principle?

Answer 1

If you change the conditions of a reversible reaction at equilibrium, the system will try to counter that change in order to restore the equilibrium.

Question 2

Why is Le Chatelier’s principle useful?

Answer 2

It allows you to predict the affect of any changes made to a system.

Question 3

According to Le Chatelier’s principle, what happens if you decrease the temperature?

Answer 3

The position of equilibrium will shift towards the exothermic direction, to produce more heat (and counteract the decrease in temperature).

Question 4

According to Le Chatelier’s principle, what happens if you increase the temperature?

Answer 4

The position of equilibrium will shift towards the endothermic direction in order to decrease the temperature (and counteract the increase in temperature).

Question 5

According to Le Chatelier’s principle, what happens if you increase the pressure?

Answer 5

The equilibrium will shift to the side with fewer molecules (moles) of gas, to reduce the pressure (and counteract the increase in pressure).

Question 6

According to Le Chatelier’s principle, what happens if you decrease the pressure?

Answer 6

The equilibrium will shift to the side with more molecules (moles) of gas, to increase the pressure (and counteract the decrease in pressure).

Question 7

According to Le Chatelier’s principle, what happens if you increase the concentration of the reactants?

Answer 7

The equilibrium will shift to the right (products side), to reduce the reactant concentrations and restore equilibrium.

Question 8

According to Le Chatelier’s principle, what happens if you decrease the concentration of the reactants?

Answer 8

The equilibrium will shift to the left (reactants side), to increase the reactant concentrations and restore equilibrium.