C8. Flashcards
Rates and Equilibrium.
What is the rate of reaction?
How quickly the reactants turn into the products.
How quickly a reactant is used up =
Quantity of reactant used / time taken.
How quickly a product is produced =
Quantity of product formed / time taken.
What are the conditions of a reaction affected by?
External environment of the reaction.
In a closed system how can you change the conditions?
Changing the concentration, temp and pressure.
What is Le Chatelier’s Principle?
At equilibrium the amount of reactants and products is constant.
At equilibrium, how can you change the amount of reactant and product?
Change the conditions of the reaction.
What does collision theory state?
For a reaction to happen, the reactant particles need to collide. If they don’t have enough energy when this happens they will just bounce apart.
What is the activation energy?
The amount of energy needed in particles when they collide so that they react.
How does increasing temperature affect the rate of reaction.
They move faster leading to more frequent collisions. It gives the particles an increased energy.
How does increasing the concentration affect the rate of reaction?
There are more particles in the reaction mixture so collisions become more often.
How does increasing the pressure affect the rate of reaction?
There is less space between particles which means there are more frequent collisions.
What are catalysts?
Things that get added to reactions to increase the rate.
What do catalysts provide?
They provide a different reaction pathway that has a lower activation energy.
What is a reversible reaction?
When a product produces the original reactant from a reaction.
