Cards (72)

    • The Gibbs Free Energy is calculated using the formula: ΔG = ΔH - TΔS
    • Match the variable with its symbol and units:
      Enthalpy ↔️ H, kJ mol⁻¹
      Temperature ↔️ T, K
      Entropy ↔️ S, J mol⁻¹ K⁻¹
      Gibbs Free Energy ↔️ G, kJ mol⁻¹
    • In the ΔG formula, ΔH represents the enthalpy change
    • Match the variable with its symbol and effect on spontaneity:
      Enthalpy Change (ΔH) ↔️ Negative favors, positive disfavors
      Temperature (T) ↔️ Affects the TΔS term
      Entropy Change (ΔS) ↔️ Positive favors, negative disfavors
      Gibbs Free Energy Change (ΔG) ↔️ Negative indicates spontaneity
    • Negative values of ΔH favor spontaneity in a reaction.

      True
    • What is entropy (ΔS) a measure of?
      Disorder or randomness
    • A positive ΔS indicates an increase in disorder, which generally favors spontaneity.

      True
    • A negative ΔS indicates a decrease in disorder
    • The Gibbs Free Energy formula is G = H - TS.

      True
    • Match the ΔG value with its corresponding spontaneity:
      ΔG < 0 ↔️ Spontaneous
      ΔG = 0 ↔️ Equilibrium
      ΔG > 0 ↔️ Non-spontaneous
    • A positive ΔS always leads to a spontaneous reaction.
      False
    • What is enthalpy (ΔH) measured in?
      kJ/mol
    • A positive ΔS means the system's disorder increases, favoring spontaneity.

      True
    • Higher temperatures can favor reactions with positive ΔS, while lower temperatures favor reactions with negative ΔH.
    • Match the ΔG scenario with its example:
      ΔG < 0 ↔️ Combustion of methane
      ΔG = 0 ↔️ Phase transition at melting point
      ΔG > 0 ↔️ Photosynthesis without light
    • A negative ΔG indicates a spontaneous reaction.

      True
    • What does a ΔG of zero indicate about a reaction?
      Reaction is at equilibrium
    • Gibbs Free Energy predicts spontaneity at constant temperature and pressure.

      True
    • A negative ΔG indicates a spontaneous reaction.
    • What does the ΔH term in the Gibbs Free Energy formula represent?
      Enthalpy change
    • Positive ΔS values favor spontaneity.

      True
    • If ΔH = -50 kJ/mol and ΔS = 0.1 kJ/(mol·K) at T = 300 K, then ΔG = -80 kJ/mol
    • What does a negative ΔG indicate about a reaction?
      The reaction is spontaneous
    • What is the effect of a negative ΔH on the spontaneity of a reaction?
      It favors spontaneity
    • What is entropy (ΔS) a measure of?
      Disorder or randomness
    • A positive ΔS generally favors spontaneity.

      True
    • At higher temperatures, the term `-TΔS` becomes more significant, especially if ΔS is positive
    • A reaction with ΔG < 0 is spontaneous.

      True
    • The Gibbs Free Energy (ΔG) and the equilibrium constant (K) are related by the formula: ΔG = -RTlnK
    • What is the value of the ideal gas constant (R) in the Gibbs Free Energy equation?
      8.314 J/(mol·K)
    • The ideal gas constant (R) has a value of 8.314
    • What is the unit of the equilibrium constant (K)?
      Unitless
    • What is the formula for Gibbs Free Energy involving enthalpy (ΔH) and entropy (ΔS)?
      ΔG = ΔH - TΔS
    • If ΔG is equal to zero, the reaction is at equilibrium
    • What is the ΔG for a reaction with ΔH = -50 kJ/mol, ΔS = 0.1 kJ/(mol·K), and T = 300 K?
      -80 kJ/mol
    • What does a higher temperature do to the effect of entropy change (ΔS) on spontaneity?
      Amplifies it
    • A negative ΔG indicates a spontaneous process.
      True
    • Arrange the conditions that favor a spontaneous reaction according to ΔG:
      1️⃣ Exothermic reactions (negative ΔH)
      2️⃣ Reactions with a positive ΔS
      3️⃣ Lower temperatures favoring negative ΔH
    • Exothermic reactions with a negative ΔH are more likely to be spontaneous.

      True
    • A negative ΔH indicates that the reaction is exothermic