Open Question
What is the difference between an exothermic reaction and an exergonic reaction?
7. Energy, Rate and Equilibrium
Gibbs Free Energy (Simplified)
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Join thousands of students who trust us to help them ace their exams!Watch the first videoMultiple Choice
What are the signs of ∆H, ∆S and ∆G for the spontaneous conversion of a solid into gas?
A
–∆H; –∆S; +∆G
B
–∆H; +∆S; +∆G
C
–∆H; +∆S; –∆G
D
+∆H; +∆S; –∆G
E
+∆H; +∆S; +∆G
Verified step by step guidance1
Identify the process: The image shows a solid converting into a gas, which is sublimation.
Consider the enthalpy change (∆H): Sublimation requires energy to overcome intermolecular forces, so ∆H is positive.
Consider the entropy change (∆S): The disorder increases as a solid becomes a gas, so ∆S is positive.
Consider the Gibbs free energy change (∆G): For a process to be spontaneous, ∆G must be negative.
Use the Gibbs free energy equation: ∆G = ∆H - T∆S. For a spontaneous process, ∆G < 0, which can occur if the increase in entropy (T∆S) outweighs the positive ∆H.
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