Understanding Chemical Reactions: Collision Theory and Catalysts

The video tutorial explains how collision theory and activation energy are crucial for chemical reactions. It discusses how increasing concentration, pressure, surface area, and temperature can enhance reaction rates. The role of catalysts, including enzymes, in speeding up reactions by lowering activation energy is also covered, with examples like iron in ammonia production and catalase in decomposing hydrogen peroxide.

What is the effect of increasing the concentration of reactants in a solution?

• It decreases the rate of reaction.

• It increases the rate of reaction.

• It has no effect on the rate of reaction.

• It changes the color of the solution.

How does increasing the surface area of solid reactants affect the reaction rate?

• It increases the reaction rate.

• It decreases the reaction rate.

• It changes the state of the reactants.

• It has no effect on the reaction rate.

What happens to the kinetic energy of reactants when the temperature is increased?

• It becomes zero.

• It increases.

• It remains the same.

• It decreases.

What is the primary function of a catalyst in a chemical reaction?

• To change the color of the reactants.

• To lower the activation energy.

• To increase the temperature of the reaction.

• To increase the pressure of the reaction.

Which of the following is an example of a biological catalyst?

• Iron

• Copper

• Enzyme

• Zinc