Gibbs Free Energy represents the maximum amount of work that can be done by a thermodynamic reaction at constant pressure and temperature.
Concept #1: The signs of Gibbs Free Energy can be used to determine if a reaction is spontaneous or non-spontaneous.
Example #1: Which of the following is an example of a nonspontaneous process?
a) Ice melting at room temperature
b) Sodium metal reacting violently with water
c) Rusting of iron at room temperature
d) A ball rolling downhill
e) Water freezing at room temperature
Example #2: Consider the decomposition of a metal oxide to its elements, where M represents a generic metal.
M3O4 (s) ⇌ 3 M (s) + 2 O2 (g)
i) What is the standard change in Gibbs energy for the reaction, as written, in the forward direction?
ii) What is the equilibrium constant of this reaction, as written, in the forward direction at 298 K?
iii) What is the equilibrium pressure of 02 (g) over M (s) at 298 K?
Example #3: For the reaction:
2 C (graphite) + H2 (g) → C2H2 (g)
ΔG° = + 209.2 kJ at 25°C. If PH2 = 100 atm, and PC2H2 = 0.10 atm, calculate ΔG for reaction.
a) +192.1 kJ
b) +266.3 kJ
c) -16.9 kJ
d) +207.8 kJ
e) +17.3 kJ
Example #4: Sodium carbonate can be made by heating sodium bicarbonate:
2 NaHCO3 (s) → Na2CO3 (s) + CO2 (g) + H2O (g)
Given that ΔH° = 128.9 kJ/mol and ΔG° = 33.1 kJ/mol at 25°C, above what minimum temperature will the reaction become spontaneous under standard-state conditions?
a) 0.4 K
B) 3.9 K
C) 321 K
D) 401 K
E) 525 K
Practice: The signs of ∆H, ∆S, and ∆G at 25oC are shown below for three chemical reactions.
∆H ∆S ∆G
Which reaction would go in the reverse direction at high temperatures?