All Flashcards
What are the steps to construct a reaction energy profile?
- 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).
What are the differences between 'intermediates' and 'transition states'?
Intermediates: Relatively stable, exist for a short time, appear between elementary steps. | Transition States: Unstable, exist momentarily, represent the highest energy point.
Differentiate between an 'exothermic' and 'endothermic' reaction in terms of energy change.
Exothermic: Releases heat, ΔE < 0, products have lower energy than reactants. | Endothermic: Absorbs heat, ΔE > 0, products have higher energy than reactants.
What is the effect of a higher activation energy (Ea) on the reaction rate?
A higher activation energy results in a slower reaction rate because more energy is required for the reaction to occur.
What is the effect of adding a catalyst to a reaction?
A catalyst increases the rate of reaction by lowering the activation energy.