A higher activation energy results in a slower reaction rate because more energy is required for the reaction to occur.

A catalyst increases the rate of reaction by lowering the activation energy.

1. Plot reactants and products with their potential energies. 2. Add transition state(s) at the highest energy point(s). 3. Connect reactants to transition state(s) and transition state(s) to products with curves. 4. Label activation energy (Ea) and overall energy change (ΔE).

A single step in a reaction mechanism that represents the change of reactants to products.

The balanced chemical equation representing the entire reaction process, combining all elementary steps.

A graph showing the potential energy of reactants and products during a reaction, illustrating activation energy and overall energy change.

The highest energy point on a reaction energy profile, representing the unstable intermediate complex during a reaction.

The minimum energy required for a reaction to occur, represented by the energy difference between reactants and the transition state.

The difference in potential energy between the reactants and products, determining if a reaction is exothermic (ΔE < 0) or endothermic (ΔE > 0).

A species formed during a reaction mechanism that is consumed in a subsequent step and does not appear in the overall balanced equation.