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 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?
Calculate the temperature at which a reaction with ΔH = 50 kJ/mol and ΔS = 100 J/(mol·K) becomes spontaneous.
Calculate ΔG for a reaction at 400 K if ΔH = 20 kJ/mol and ΔS = 50 J/(mol·K).
Describe how Gibbs free energy is related to maximum non-expansion work.
Describe the effect of pressure on Gibbs free energy for gases.
Describe the physical meaning of Gibbs free energy.
Explain the significance of standard Gibbs free energy change (ΔG°) in chemical reactions.
Explain why a reaction with a positive ΔH and a positive ΔS can be spontaneous at high temperatures.
Explain why a reaction with ΔG < 0 may not occur rapidly.
Explain why ΔG is temperature dependent.
If ΔG for a reaction is negative, what does this indicate about the spontaneity of the reaction?
If ΔG° = 0 for a reaction at 298 K, what is the value of the equilibrium constant K?
If ΔG° = 10 kJ/mol at 298 K, calculate the equilibrium constant K. (R = 8.314 J/(mol·K))
If ΔH = -100 kJ/mol and ΔS = -200 J/(mol·K), calculate ΔG at 298 K.
State the effect of increasing temperature on the spontaneity of a reaction with positive ΔH and positive ΔS.
State the relationship between Gibbs free energy and the equilibrium constant (K) at temperature T.
What is the formula for Gibbs free energy change (ΔG) at constant temperature and pressure?
