The rate constant for a reaction can be increased by ______ the stability of the reactant or by ______ the stability of the transition state.

Verified step by step guidance

1. Identify the relationship between the rate constant and the activation energy using the Arrhenius equation: k = Ae^{-Ea/RT}, where k is the rate constant, A is the pre-exponential factor, Ea is the activation energy, R is the gas constant, and T is the temperature.
2. Understand that the activation energy (Ea) is the energy barrier that must be overcome for a reaction to proceed. Lowering the activation energy increases the rate constant.
3. Recognize that increasing the stability of the reactant typically increases the activation energy, as the reactant is at a lower energy state, making it harder to reach the transition state.
4. Realize that increasing the stability of the transition state lowers the activation energy, as the energy difference between the reactant and the transition state is reduced.
5. Conclude that the rate constant for a reaction can be increased by decreasing the stability of the reactant or by increasing the stability of the transition state.

Key Concepts

Rate Constant

The rate constant (k) is a proportionality factor in the rate equation of a chemical reaction, indicating how quickly a reaction proceeds. It is influenced by factors such as temperature, concentration, and the nature of the reactants. A higher rate constant signifies a faster reaction, while a lower rate constant indicates a slower reaction.

Stability of Reactants

The stability of reactants refers to their energy state and tendency to undergo a reaction. More stable reactants have lower energy and are less likely to react, while less stable reactants are more reactive. Enhancing the stability of reactants can lead to a decrease in the rate of reaction, as they are less inclined to transition into products.

Transition State

The transition state is a high-energy, unstable arrangement of atoms that occurs during the transformation from reactants to products. It represents the peak of the energy barrier that must be overcome for a reaction to proceed. Increasing the stability of the transition state lowers the activation energy, thereby increasing the rate constant and accelerating the reaction.