Collision Theory

The video explains how chemical reactions occur through particle collisions, emphasizing the need for sufficient energy, known as activation energy, for successful reactions. It discusses four factors affecting reaction rates: temperature, pressure, concentration, and catalysts. Higher temperatures increase particle energy, leading to more successful collisions. Increased pressure and concentration raise collision frequency. Catalysts provide alternative reaction pathways with lower activation energy, speeding up reactions. Understanding these factors allows control over reaction rates, crucial for chemical manufacturing.

What is the minimum energy required for a reaction to occur called?

• Minimum energy

• Collision energy

• Activation energy

• Reaction energy

How does increasing the temperature affect the rate of a chemical reaction?

• It increases the number of successful collisions

• It decreases the number of collisions

• It decreases the energy of particles

• It has no effect on the reaction rate

What happens to reactant particles when the pressure is increased in a gaseous reaction?

• They move slower

• They become more crowded

• They lose energy

• They stop colliding

What is the effect of increasing the concentration of a solution on the reaction rate?

• It has no effect on the reaction rate

• It increases the number of collisions

• It decreases the number of collisions

• It decreases the energy of particles

How do catalysts speed up chemical reactions?

• By decreasing the pressure

• By providing an alternative pathway with lower activation energy

• By increasing the concentration of reactants

• By increasing the temperature