Practice Standard Gibbs Free Energy Change (δg°) (4.4.4) - Chapter 4: Energetics/Thermochemistry

Practice: Standard Gibbs Free Energy Change (ΔG°)

Lesson 4.4.4Energetics/Thermochemistry

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6 sample questions

Question 1.
What is the formula for calculating standard Gibbs free energy change?
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Remember to sum the free energies of products and reactants.
Question 2.
If ΔG < 0, what can we say about the spontaneity of the reaction?
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Think about what a negative Gibbs free energy means.
3Question 3.
What does a negative ΔG value mean for a reaction?
- The reaction is spontaneous.
- The reaction is at equilibrium.
- The reaction is non-spontaneous.
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Think about what 'spontaneous' means in this context.
4Question 4.
True or False: ΔG = 0 indicates that the reaction is non-spontaneous.
- True
- False
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Consider the definition of equilibrium.
Question 5.
Consider the following reaction at standard condition: N₂(g) + 3H₂(g) → 2NH₃(g). If ΔG_f°(NH₃) = -33.0 kJ/mol, ΔG_f°(N₂) = 0 kJ/mol, and ΔG_f°(H₂) = 0 kJ/mol, what is ΔG° for the reaction?
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Apply the Gibbs energy formula and carefully multiply the coefficients.
Question 6.
Calculate the equilibrium temperature (T_eq) for the reaction where ΔH = 40 kJ/mol and ΔS = 0.1 kJ/K. What does your answer mean?
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Ensure ΔH and ΔS are in consistent units!

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