Skip to main content
Back

Enzyme Activation Energy quiz #1

Control buttons has been changed to "navigation" mode.
1/10
  • What is activation energy (EA) in a chemical reaction, and how does it relate to the transition state?
    Activation energy (EA) is the minimum amount of energy required to initiate a chemical reaction. It is defined as the energy difference between the reactants and the transition state, which is a temporary state of maximum energy during the reaction.
  • How do enzymes affect the activation energy of a chemical reaction, and what is the result of this effect?
    Enzymes lower the activation energy of a chemical reaction by reducing the energy required to reach the transition state. This allows reactions to proceed much faster than they would without enzymes.
  • In an exergonic reaction, how do the energy levels of reactants, products, and the transition state compare?
    In an exergonic reaction, the reactants have higher energy than the products, and the transition state has the highest energy, representing a peak between the reactants and products.
  • Why does a higher activation energy result in a slower reaction rate?
    A higher activation energy means that fewer reactant molecules have enough energy to reach the transition state, resulting in a slower reaction rate.
  • What is activation energy (EA) in a chemical reaction, and how is it represented on a reaction energy diagram?
    Activation energy (EA) is the minimum amount of energy required to start a chemical reaction, represented as the energy difference between the reactants and the transition state at the peak of the energy diagram.
  • How do enzymes affect the activation energy of a chemical reaction?
    Enzymes lower the activation energy required for a reaction, making it easier for reactants to reach the transition state and thus speeding up the reaction.
  • In an exergonic reaction, how do the energy levels of reactants, products, and the transition state compare?
    In an exergonic reaction, the reactants have higher energy than the products, and the transition state has the highest energy, forming a peak between them.
  • Why does a higher activation energy result in a slower reaction rate?
    A higher activation energy means fewer reactant molecules have enough energy to reach the transition state, so the reaction proceeds more slowly.
  • What is the transition state in a chemical reaction?
    The transition state is a temporary state of maximum energy during a reaction, located at the peak of the energy curve.
  • How does the presence of an enzyme change the reaction energy diagram for a chemical reaction?
    With an enzyme, the peak representing the transition state is lower, indicating a reduced activation energy and a faster reaction rate.