2.1 Rates of Reactions (Part 2 of 2)

What is collision theory used to explain?

• Molecular shapes

• Chemical bonding

• Atomic structure

• Reaction rates

What is required for a collision to be considered successful according to collision theory?

• Particles must collide with low energy

• Particles must collide in any orientation

• Particles must collide with sufficient energy and in the correct orientation

• Particles must collide with insufficient energy

What does increasing the concentration of reactants do to the rate of reaction?

• Has no effect on the rate of reaction

• Initially increases then decreases the rate of reaction

• Increases the rate of reaction

• Decreases the rate of reaction

How does temperature affect the rate of a chemical reaction?

• Decreases the kinetic energy of particles

• Increases the proportion of particles with lower energies

• Increases the kinetic energy of particles, increasing the rate of reaction

• Has no effect on the kinetic energy of particles

What effect does increasing pressure have on reactions involving gases?

• Only affects the volume, not the rate of reaction

• Has no effect on the rate of reaction

• Increases the rate of reaction

• Decreases the rate of reaction

Why do smaller particles react more rapidly than larger ones?

• They have less mass

• They have a greater surface area exposed for reaction

• They are more dense

• They contain more atoms

What role do catalysts play in chemical reactions?

• They increase the activation energy

• They are consumed in the reaction

• They decrease the activation energy

• They decrease the number of successful collisions

How do enzymes function as biological catalysts?

• By providing an alternate pathway of lower activation energy

• By increasing the temperature

• By reducing the concentration of reactants

• By acting as a competitive inhibitor

Does increasing the rate of reaction increase the amount of product formed?

• Yes, but only in exothermic reactions

• No, it does not affect the amount of product formed

• No, it only affects how quickly the product is formed

• Yes, it increases the amount of product