Question

Why does an increase in temperature favor an increase in the speed of a reaction?

Short answer

An increase in temperature favors an increase in the speed of a reaction because it raises the average kinetic energy of particles. As the temperature increases, particles move faster and collide more energetically, increasing the probability of overcoming the activation energy barrier and successful collisions that form products.

Step-by-step solution

Understand reaction rates

Reaction rates refer to the speed at which a chemical reaction occurs. This is typically measured as the change in the concentration of reactants or products over a specific period. There are several factors that can influence the rate of a reaction, including temperature, concentration, surface area, and the addition of catalysts.

Examine the role of kinetic energy in chemical reactions

In chemical reactions, molecules or atoms collide with one another, forming and breaking bonds to create new products. The kinetic energy of these particles plays a crucial role in determining the likelihood of successful collisions. Greater kinetic energy implies more intense collisions, increasing the chances of bond formation or breakage processes.

Relate temperature to kinetic energy

Temperature is a measure of the average kinetic energy of the particles in a system. When the temperature increases, the average kinetic energy of the particles also increases. This means that the particles are moving faster, and their collisions will be more energetic.

Understand the activation energy

For a reaction to occur, the particles involved need to overcome a specific energy barrier called activation energy (E_a). Activation energy is the minimum energy required for the reactants to form products in a chemical reaction. If the particles have sufficient energy to overcome the activation energy barrier, the reaction can proceed.

Apply the effect of temperature on reaction rate

With an increase in temperature, the kinetic energy of particles increases, and there is a greater probability that more particles have the necessary energy to surpass the activation energy barrier. This results in a higher frequency of successful collisions between reacting particles that form products, ultimately increasing the reaction rate. In conclusion, an increase in temperature favors an increase in the speed of a chemical reaction because it raises the average kinetic energy of particles, making it more likely for them to have sufficient energy to overcome the activation energy barrier and leading to more successful collisions that form products.