Rates of Reactions

An increase in temperature increases the rate of reaction. Why? How many of these are correct explanations. - The particles move faster because they have more energy. - Particles collides more often. - There are more particles per unit volume, resulting in more collisions. - More of the collisions between particles are successful because they have more energy (have the activation energy). - Rate of reaction increases because there is an increase in the frequency of collisions. /

Increasing the concentration of the reactant increases the rate of the reaction. Why? How many of these are correct explanations. - Rate of reaction increases because the particles move faster and collide more. - Rate of reaction increases because there are more particles per unit volume. - Rate of reaction increases because there is an increase in the frequency of collisions. - Rate of reaction increases because the particles have more energy.

What is the effect of increasing the pressure on the rate of reaction?

Increasing the surface area of a solid reactant causes an increased rate of reaction. Why?

What do catalysts do?

Why do catalysts not need replacing too often?

Which two statements best explain how catalysts speed up reactions? A) Catalysts do not get used up during the reaction. B) Catalysts make reactions exothermic. C) Catalysts lower the activation energy of the reaction. D) Catalysts provide a different route for a chemical reaction to occur. E) Catalysts raise the temperature of the reaction.