Practice Hl: Spontaneity Of Reactions (4.5) - Chapter 4: Energetics/Thermochemistry

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6 sample questions

Question 1.
What does it mean if ΔG is less than 0?
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Think about reactions that occur naturally.
Question 2.
What is the relationship between ΔG and equilibrium?
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Consider when reactants and products are stable.
3Question 3.
What is the significance of a negative ΔG?
- The reaction is non-spontaneous
- The reaction is spontaneous
- The reaction is at equilibrium
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Look at definitions of spontaneity.
4Question 4.
True or False: All spontaneous reactions have a negative ΔH.
- True
- False
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Consider both endothermic and exothermic reactions.
Question 5.
A chemical reaction has ΔH = -120 kJ and ΔS = 0.4 kJ/K. Calculate the temperature at which this reaction becomes non-spontaneous.
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Use the equilibrium temperature formula.
Question 6.
Discuss how an increase in temperature might affect a system where ΔH is +30 kJ and ΔS is +0.1 kJ/K. Will it eventually become spontaneous?
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Refer to the influence of temperature on ΔG.

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