What is the relationship between temperature and rate constant?

The rate constant increases with an increase in temperature, as described by the Arrhenius equation.

The relationship between temperature and the rate constant is a fundamental concept in chemical kinetics. This relationship is quantitatively described by the Arrhenius equation, which states that the rate constant (k) of a reaction increases exponentially with an increase in temperature (T).

The Arrhenius equation is k = Ae^(-Ea/RT), where A is the pre-exponential factor (also known as the frequency factor), Ea is the activation energy, R is the gas constant, and T is the absolute temperature. The equation shows that the rate constant is directly proportional to the temperature. This means that as the temperature increases, the rate constant also increases, leading to a faster reaction rate.

The reason for this relationship lies in the nature of chemical reactions. For a reaction to occur, the reactant molecules must collide with sufficient energy to overcome the activation energy barrier. As the temperature increases, the kinetic energy of the molecules also increases. This means that a greater proportion of molecules have the necessary energy to overcome the activation energy barrier, leading to an increase in the rate of reaction.

Furthermore, the exponential term in the Arrhenius equation, e^(-Ea/RT), indicates that even a small increase in temperature can lead to a significant increase in the rate constant. This is because the rate constant is exponentially dependent on the inverse of the temperature.

To understand how molecular collisions affect reaction rates, you may refer to Basics of Collision Theory.

For more detailed information on what activation energy means in this context and its implications for chemical reactions, see Activation Energy: An Introduction.

Explore the Arrhenius Equation further to see a comprehensive breakdown of its components and their significance in predicting reaction rates.

In summary, the relationship between temperature and the rate constant is a key aspect of chemical kinetics. The Arrhenius equation provides a mathematical description of this relationship, showing that the rate constant increases exponentially with an increase in temperature. This is due to the increased kinetic energy of the molecules at higher temperatures, which allows a greater proportion of them to overcome the activation energy barrier and react.