Theory of Reaction Rate

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

The collisions which bring about a chemical reaction are called: 

• Consistent collisions
•  Normal collisions 
• Effective collisions 
• None of the above

Why does a higher temperature increase the rate of a reaction?

• it increases both the frequency and energy of particle collisions
• it only increases the frequency of particle collisions
• it only increases the energy of particle collisions
• it reduces the activation energy of the reaction

What is the concept of successful collision in a chemical reaction?

• Particles colliding and exploding
• Particles colliding but not reacting
• Particles colliding and reacting
• Particles colliding and changing shape

What is activation energy?

• The minimum amount of energy required for a reaction to start
• The energy required for a successful collision
• The energy released during a reaction
• The energy of the reactants and products

How can the chance of a successful collision be increased?

• By decreasing the frequency of collisions
• By decreasing the number of reacting particles
• By decreasing the energy of the particles
• By increasing the frequency of collisions

What can be done to increase the chance of a successful collision?

• Decrease the frequency of collisions
• Decrease the activation energy
• Increase the concentration of reactants
• Increase the size of the products

Collisions may take place between: 

• Atoms
• Ions
• Molecules
• All of the above

What two factors govern whether a collision between reacting particles will be effective?

• orientation and potential energy 
• kinetic energy and temperature 
• kinetic energy and orientation 
• potential energy and kinetic energy 

Which component of collision theory is represented in the image?

• Correct orientation of molecules

• molecules collide with sufficient energy

• Products become reactants

• Molecules form an activated complex