Practice Influence Of Temperature On Spontaneity (4.5.2) - Chapter 4: Energetics/Thermochemistry

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6 sample questions

Question 1.
What does a negative ΔG value indicate about a reaction?
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Think about the meaning of spontaneity in chemical reactions.
Question 2.
What is the formula for Gibbs Free Energy?
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Remember the components contributing to Gibbs Free Energy.
3Question 3.
What is the condition for a reaction to be spontaneous?
- ΔG < 0
- ΔG > 0
- ΔG = 0
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Remember the Gibbs Free Energy criterion.
4Question 4.
True or False: Positive ΔH and negative ΔS can lead to spontaneous reactions at any temperature.
- True
- False
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Think about the relationship between enthalpy and entropy.
Question 5.
A reaction has ΔH = -100 kJ/mol and ΔS = 300 J/(mol·K). At what temperature will this reaction change from spontaneous to non-spontaneous? Calculate T_eq.
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Ensure units for ΔH and ΔS match before dividing.
Question 6.
If a reaction has a positive ΔH and a negative ΔS, assess its spontaneity across a range of temperatures from low to high.
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Think about the implications of the signs of ΔH and ΔS.

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