Use the results of Example 29-12 to determine the rate of desorption of CO from palladium at 300

step 1 So just to start off with some contextual learning, we've got the definition of entropy here. So

Use the results of Example 29-12 to determine the rate of...

Key Concepts

Activation Energy

Activation energy is the energy barrier that must be overcome for a reaction, such as desorption, to occur. A higher activation energy usually results in a slower desorption rate at a given temperature, while an increase in temperature can lead to a significant increase in the rate by providing the necessary energy to overcome this barrier.

Temperature Dependence of Reaction Rates

The rate of desorption is highly sensitive to temperature changes. As temperature increases, a larger fraction of molecules possess sufficient energy to overcome the activation barrier, thus increasing the rate constant exponentially as described by the Arrhenius equation. This concept is critical when comparing reaction rates at different temperatures, such as 300 K versus 500 K.

Desorption Kinetics

Desorption kinetics describes the process and rate at which molecules leave a surface, which is often characterized by a rate constant that depends on the order of the reaction. In many cases, the desorption process is assumed to follow first-order kinetics, where the desorption rate is directly proportional to the number of adsorbed molecules present on the surface.

Arrhenius Equation

The Arrhenius equation provides a fundamental relationship that quantifies the temperature dependence of reaction rates, including desorption. It expresses the rate constant as k = A exp(-E?/RT), where A is the pre-exponential factor, E? is the activation energy required for desorption, R is the universal gas constant, and T is the absolute temperature.

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