Practice Criteria For Spontaneity (4.5.1) - Chapter 4: Energetics/Thermochemistry

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6 sample questions

Question 1.
What does ΔG < 0 signify in a reaction?
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Recall the definition of spontaneity.
Question 2.
What happens at equilibrium concerning ΔG?
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Think about the balance of reactants and products.
3Question 3.
What does a negative Gibbs free energy change indicate?
- The reaction is spontaneous
- The reaction is non-spontaneous
- The system is at equilibrium
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Remember the basic criterion of spontaneity.
4Question 4.
True or False: A reaction is non-spontaneous when ΔG is greater than zero.
- True
- False
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Think about the meaning of spontaneity in chemical reactions.
Question 5.
Given a reaction with ΔH = -200 kJ/mol and ΔS = 300 J/K·mol, calculate ΔG at 298 K and determine spontaneity.
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Remember to align units.
Question 6.
Explain situations where increasing temperature switches a reaction from non-spontaneous to spontaneous, giving examples.
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Use the melting of ice as a practical example.

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