College Chemistry : Le Chatelier's Principle
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Example Questions
Example Question #1 : Equilibrium
Consider the following equation at equilibrium:
What would happen if more 
There is not enough information to determine the effects of adding more 
The reaction would shift towards the products.
The reaction would shift towards the reactants.
There would be no change in the system.
The reaction would shift towards the reactants.
Recall Le Chatelier's principle: A chemical system at equilibrium will shift in the direction that minimizes the disturbance to the system.
Before the addition of 
However, after the addition of 
In order to maintain equilibrium, the reaction will then shift left to favor the reactants in this chemical system.
Example Question #1 : Le Chatelier's Principle
Consider the following equation at equilibrium:
What would happen if more 
More 
There would be no change.
More 
Less 
More
Recall Le Chatelier's principle: A chemical system at equilibrium will shift in the direction that minimizes the disturbance to the system.
Before the addition of 
However, after the addition of 
In order to maintain equilibrium, the reaction will then shift right of favor the formation of more products.
Example Question #1 : Le Chatelier's Principle
Consider the following exothermic equation:
Which of the following actions will cause the products to be favored?
Increase the temperature at which the reaction is conducted.
Decrease the amount of 
Decrease the temperature at which the reaction is conducted.
Increase the amount of 
Decrease the temperature at which the reaction is conducted.
Since the equation is exothermic, you can think of heat as another product of the reaction:
Apply LeChatelier's principle to this equation.
If the temperature at which the reaction is decreased, that is akin to decreasing the amount of product made, thus causing the reaction to shift towards the products.
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