Understanding Collision Theory and Activation Energy for Chemical Reactions

The video explains collision theory, which states that particles must collide with sufficient energy for a reaction to occur. This energy is known as activation energy. The rate of reaction depends on the number of collisions with energy exceeding the activation energy. To increase reaction rates, one can increase the number of particles or the energy of the particles, leading to more frequent and energetic collisions.

What is necessary for a chemical reaction to occur according to collision theory?

• Particles must collide with enough energy.

• Particles must be stationary.

• Particles must be in a solid state.

• Particles must be at absolute zero temperature.

What happens when particles collide with energy less than the activation energy?

• A reaction occurs.

• The particles bounce off each other.

• The particles form a new compound.

• The particles explode.

What is the role of activation energy in a chemical reaction?

• It is the energy required to start a reaction.

• It is the energy that stops a reaction.

• It is the energy released during a reaction.

• It is the energy that cools down the reactants.

How can the rate of a chemical reaction be increased?

• By decreasing the number of particles.

• By increasing the energy of the particles.

• By reducing the temperature.

• By keeping the particles stationary.

Which of the following is NOT a way to increase the rate of reaction?

• Increasing the energy of the particles.

• Increasing the number of particles.

• Ensuring collisions have more energy than the activation energy.

• Decreasing the number of collisions.