Gibbs Free Energy
Chemistry ⇒ Thermochemistry and Energetics
Gibbs Free Energy starts at 12 and continues till grade 12.
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See sample questions for grade 12
A reaction has ΔG° = -25 kJ/mol at 298 K. Is the equilibrium constant K greater than, less than, or equal to 1?
A reaction has ΔH = 0 and ΔS < 0. What can you say about the spontaneity of the reaction?
A reaction mixture has Q > K. What is the sign of ΔG?
Describe how Gibbs free energy is related to maximum non-expansion work.
A reaction has ΔG° = -25 kJ/mol at 298 K. Is the equilibrium constant K greater than, less than, or equal to 1?
A reaction has ΔH = 0 and ΔS < 0. What can you say about the spontaneity of the reaction?
A reaction has ΔH = -40 kJ/mol and ΔS = -100 J/(mol·K). At what temperature does the reaction become non-spontaneous?
A reaction mixture has Q > K. What is the sign of ΔG?
At equilibrium, the value of ΔG is: (1) Positive (2) Negative (3) Zero (4) Cannot be determined
Which of the following best describes a process with ΔG > 0? (1) Spontaneous (2) Non-spontaneous (3) At equilibrium (4) Exothermic
Which of the following conditions always results in a spontaneous reaction? (1) ΔH < 0, ΔS > 0 (2) ΔH > 0, ΔS < 0 (3) ΔH < 0, ΔS < 0 (4) ΔH > 0, ΔS > 0
Which of the following is a correct statement? (1) ΔG is always negative for spontaneous reactions. (2) ΔG is always positive for spontaneous reactions. (3) ΔG is zero for spontaneous reactions. (4) ΔG is unrelated to spontaneity.
Fill in the blank: For a reaction at constant temperature and pressure, the change in Gibbs free energy is equal to the maximum _______ work.
Fill in the blank: For a reaction to be spontaneous at all temperatures, ΔH must be _______ and ΔS must be _______.
Fill in the blank: The relationship between ΔG and ΔG° is ΔG = ΔG° + _______
Fill in the blank: The standard Gibbs free energy change is denoted as _______.
True or False: A reaction with ΔG = 0 is at equilibrium.
True or False: Gibbs free energy is only defined for open systems.
True or False: If ΔG is zero, the system is at equilibrium and no net change occurs.
True or False: The sign of ΔG determines whether a reaction is exothermic or endothermic.
