Molecular Collisions

What is collision theory?

• Molecules must collide in the correct orientation with enough energy to bond.

• Molecules need enough energy to collide and react.

• Atoms constantly collide and react.

• The minimum energy needed for atoms to react

Which PE Diagram represents an endothermic reaction?

• A

• B

Tags

NGSS.HS-PS1-4

NGSS.HS-PS3-4

Which PE Diagram represents an exothermic reaction?

• A

• B

Tags

NGSS.HS-PS1-4

Increasing the temperature of your solution will.......

• Not affect the rate of reaction.

• Speed up the rate of reaction

• Slow down the rate of reaction

Tags

NGSS.HS-PS1-5

More collisions correspond to a: 

• Faster reaction rate  
• Slower reaction rate
• Constant reaction rate 
• None of the above

Tags

NGSS.HS-PS1-5

Increase in temperature of the reactants can do one of the following

• Slow collision frequency
• Allow less effective collision between the particles
• Cause particles to lose speed
• Increase collision between the particles thus increasing the reaction rate

Tags

NGSS.HS-PS1-5

B represents

• energy absorbed
• energy released
• activation energy

Tags

NGSS.HS-PS1-4

Products will form faster if____________

• the particle size of the reactants are larger.
• temperature is decreased.
• concentration of the reactants are increased.
• the reaction is not stirred.

Tags

NGSS.HS-PS1-5

How does increasing concentration increase the reaction rate?

• There are more particles in a given space meaning more collisions therefore more successful collsions

• It increases the kinetic energy of the particles resulting in more successful collisions

• It reduces the activation energy of the reaction

• It provides an alternative route for the chemical reaction to occur

Tags

NGSS.HS-PS1-5

Which of the following lowers the activation energy of a reaction?

• reactants

• products

• catalysts

• inhibitors