Chemical Reaction Rates and Factors

This video by Mr. Millings explains collision theory, which describes how chemical reactions occur and the factors affecting their rates. It covers the necessity of reactant collisions with sufficient energy and correct orientation for reactions to occur. The video discusses methods to increase reaction rates, such as increasing surface area, pressure, temperature, and using catalysts. A simulation demonstrates these concepts, highlighting the importance of activation energy. Catalysts are explained as substances that lower activation energy, speeding up reactions without being consumed.

What is the primary requirement for a chemical reaction to occur according to collision theory?

• Reactant particles must collide with sufficient energy and correct orientation.

• Reactant particles must be in a gaseous state.

• Reactant particles must be at a high temperature.

• Reactant particles must be in a liquid state.

Which of the following is NOT a factor that can increase the rate of a chemical reaction?

• Increasing the concentration of reactants

• Introducing a catalyst

• Decreasing the pressure of the system

• Increasing the surface area of reactants

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

• It decreases the kinetic energy of particles.

• It increases the kinetic energy of particles, leading to more collisions.

• It decreases the number of reactant particles.

• It has no effect on the reaction rate.

In the simulation example, what was necessary for reactant A to successfully react with compound BC?

• A needed to be at a lower temperature.

• A needed to be in a liquid state.

• A needed to collide with BC at a low speed.

• A needed to collide with BC with enough activation energy and correct orientation.

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

• They increase in temperature.

• They form a new compound.

• They bounce off each other without reacting.

• They change state from solid to liquid.

What role does activation energy play in a chemical reaction?

• It determines the color of the reactants.

• It is the minimum energy required for reactants to transform into products.

• It is the energy released during the reaction.

• It is the energy absorbed by the products.

What is an example of activation energy in everyday life?

• Freezing water

• Melting ice

• Boiling water

• Striking a match on a matchbox

How does a catalyst affect a chemical reaction?

• It increases the activation energy required.

• It changes the state of the reactants.

• It decreases the activation energy required, speeding up the reaction.

• It is consumed during the reaction.

Which statement is true about catalysts?

• They are consumed in the reaction.

• They permanently change the reactants.

• They lower the activation energy without being consumed.

• They increase the temperature of the reaction.

What is the effect of introducing an enzyme in a biological reaction?

• It has no effect on the reaction rate.

• It changes the reactants into a different state.

• It decreases the activation energy, speeding up the reaction.

• It increases the activation energy required.