All Flashcards
Differentiate between endothermic and exothermic reactions.
Endothermic: Absorbs energy, products have higher potential energy. Exothermic: Releases energy, products have lower potential energy.
Compare activation energy (Ea) and ΔH.
Ea: Energy to reach the transition state. ΔH: Overall energy change between reactants and products.
What's the difference between a first-order and second-order elementary reaction?
First-order: Rate depends on one reactant. Second-order: Rate depends on two reactants.
What is the effect of increasing temperature on reaction rate?
Generally, an increase in temperature increases the reaction rate.
What is the effect of a catalyst on activation energy?
A catalyst lowers the activation energy.
What is the effect of higher activation energy on reaction rate?
Higher activation energy leads to a slower reaction rate.
Label the axes of a potential energy diagram.
X-axis: Reaction Progress/Coordinate, Y-axis: Potential Energy.
On a potential energy diagram, what does the peak represent?
The peak represents the activated complex or transition state.
On a potential energy diagram, how do you identify ΔH for an exothermic reaction?
ΔH is the negative energy difference between the reactants and products.
On a potential energy diagram, how do you identify ΔH for an endothermic reaction?
ΔH is the positive energy difference between the reactants and products.
On a potential energy diagram, what represents the activation energy?
The energy difference between the reactants and the transition state.