Practice Hl: Entropy And Gibbs Free Energy (4.4) - Chapter 4: Energetics/Thermochemistry

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6 sample questions

Question 1.
Define entropy in your own words.
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Think about how the arrangement of particles changes.
Question 2.
What happens to the entropy when a solid melts?
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Remember phase changes.
3Question 3.
What does ΔG < 0 indicate?
- The reaction is not spontaneous
- The reaction is spontaneous
- The system is at equilibrium
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Think about what spontaneity means in thermodynamics.
4Question 4.
True or False: The entropy of a gas is lower than that of a solid.
- True
- False
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Consider the arrangement of particles in different states.
Question 5.
Calculate the change in Gibbs free energy at 298 K for the reaction where ΔH = -150 kJ and ΔS = 0.4 kJ/K. Is this reaction spontaneous?
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Ensure all units are consistent.
Question 6.
Given that the melting point of ice is 0 °C, show the calculation of equilibrium temperature based on the values of ΔH and ΔS for the phase change. Could it be spontaneous below 0 °C?
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Watch out for unit conversions when computing.

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