Chemical Reaction Rates

How many ways are there to SPEED up a chemical reaction?

• 5

• 2

• 4

• 1

• 3

What are the two conditions needed for chemical reactions to occur

• correct pressure and temperature

• correct temperature and speed

• correct orientation and enough energy

How does decreasing the volume of a container help reactions to occur? 

• it will cause faster speed 

• it will cause more collisions to occur

What is the same as increasing the number of students at the school for a chemical reaction? 

(Hint: High concentration means particles are closer together).

• increasing concentration

• decreasing temperature

• increasing temperature

• decreasing the concentration 

How can we increase the speed of the molecules for chemical reactions? 

(Hint: More heat energy means particles are moving FASTER).

• decrease the energy

• increase the volume

• increase the number of molecules

• increase the temperature

If the temperature is higher - what happens?

• Particles are slower (more kinetic energy), causing more collisions, causing the reaction rate to go down.

• Particles are slower (less kinetic energy), causing fewer collisions, causing the reaction rate to go up.

• Particles are faster (more kinetic energy), causing fewer collisions, causing the reaction rate to go down.

• Particles are faster (more kinetic energy), causing more collisions, causing the reaction rate to go up.
   

What happens when larger clumps of reactants are broken down into smaller clumps?

• Available surface area increases causing reaction rate to decrease.

• Available surface area increases causing reaction rate to increase.

• Available surface area decreases causing reaction rate to increase.

• Available surface area decreases causing reaction rate to decrease.

What does a catalyst do to help the reaction to occur? 

• lowers the activation energy needed to start the reaction.

• increases the temperature needed to start the reaction.

• lowers the pressure needed to start the reaction.

Reaction rate measures the speed at which reactants ______ and products ______.

• disappear; appear

• appear; disappear

In order for a collision to be considered effective, the reactant particles must have the correct orientation and the proper amount of...

• surface area.

• space.

• concentration.

• energy.