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Gibbs Free Energy quiz

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Terms in this set (8)

  • How does the change in free energy differ between exergonic and endergonic reactions?
    In exergonic reactions, the change in free energy (ΔG) is negative, indicating spontaneity, while in endergonic reactions, ΔG is positive, indicating non-spontaneity.
  • How does the amount of free energy input differ between exergonic and endergonic reactions?
    Exergonic reactions release free energy, requiring no input, while endergonic reactions require an input of free energy to proceed.
  • What is the significance of a negative ΔG in a chemical reaction?
    A negative ΔG indicates that the reaction is spontaneous and will proceed without external energy input.
  • What does a positive ΔG signify about a reaction's spontaneity?
    A positive ΔG signifies that the reaction is non-spontaneous and requires energy input to proceed.
  • Under what conditions is a reaction with both positive ΔH and ΔS spontaneous?
    A reaction with both positive ΔH and ΔS is spontaneous at high temperatures.
  • What does ΔG equal at equilibrium?
    At equilibrium, ΔG equals zero, indicating no net change in the system.
  • How does the reaction quotient (Q) relate to Gibbs free energy under non-standard conditions?
    Under non-standard conditions, ΔG is calculated using the reaction quotient (Q) in the equation ΔG = ΔG° + RTlnQ.
  • What is the role of the gas constant (R) in the Gibbs free energy equation under non-standard conditions?
    The gas constant (R) is used in the equation ΔG = ΔG° + RTlnQ to relate temperature and reaction quotient to Gibbs free energy.