Consider these two gas-phase reactions: a. AA(g) + BB(g) → 2 AB(g) b. AB(g) + CD(g) → AC(g) + BD(g) If the reactions have identical activation barriers and are carried out under the same conditions, which one would you expect to have the faster rate?

Key Concepts

Activation Energy

Activation energy is the minimum energy required for a chemical reaction to occur. It represents the energy barrier that reactants must overcome to form products. In this context, since both reactions have identical activation barriers, the rate of reaction will depend on other factors, such as the concentration of reactants and the reaction mechanism.

Reaction Mechanism

The reaction mechanism describes the step-by-step sequence of elementary reactions that lead to the overall reaction. Different mechanisms can influence the rate of a reaction, even if the activation energy is the same. Understanding the mechanism helps in predicting which reaction may proceed faster based on the number of steps and the nature of intermediates involved.

Rate of Reaction

The rate of reaction refers to the speed at which reactants are converted into products. It is influenced by factors such as concentration, temperature, and the presence of catalysts. In this case, comparing the rates of the two reactions requires considering how the stoichiometry and the number of molecules involved in each reaction affect the overall rate under identical conditions.