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Ch.19 - Chemical Thermodynamics
All textbooksBrown 14th EditionCh.19 - Chemical ThermodynamicsProblem 60
Chapter 19, Problem 60

Using data from Appendix C, calculate the change in Gibbs free energy for each of the following reactions. In each case, indicate whether the reaction is spontaneous at 298 K under standard conditions.
(a) 2 Ag(s) + Cl2(g) → 2 AgCl(s)
(b) P4O10(s) + 16 H2(g) → 4 PH3(g) + 10 H2O(g)
(c) CH4(g) + 4 F2(g) → CF4(g) + 4 HF(g)
(d) 2 H2O2(l) → 2 H2O(l) + O2(g)

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1
Identify the standard Gibbs free energy of formation (ΔG_f°) for each reactant and product in the given reactions from Appendix C.
For each reaction, use the formula ΔG°_reaction = Σ(ΔG_f° products) - Σ(ΔG_f° reactants) to calculate the change in Gibbs free energy.
For reaction (a), calculate ΔG° using the ΔG_f° values for AgCl(s), Ag(s), and Cl2(g).
For reaction (b), calculate ΔG° using the ΔG_f° values for PH3(g), H2O(g), P4O10(s), and H2(g).
Determine the spontaneity of each reaction at 298 K by checking if ΔG° is negative (spontaneous) or positive (non-spontaneous).

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Related Practice
Open Question
Using data in Appendix C, calculate ΔH°, ΔS°, and ΔG° at 298 K for each of the following reactions. (a) H₂(g) + F₂(g) → 2 HF(g) (b) C(s, graphite) + 2 Cl₂(g) → CCl₄(g) (c) 2 PCl₃(g) + O₂(g) → 2 POCl₃(g) (d) 2 CH₃OH(g) + H₂(g) → C₂H₆(g) + 2 H₂O(g)
Textbook Question

Use data in Appendix C to calculate ΔH°, ΔS°, and ΔG° at 25 °C for each of the following reactions.

a. 4 Cr(s) + 3 O2(g) → 2 Cr2O3(s)

b. BaCO3(s) → BaO(s) + CO2(g)

c. 2 P(s) + 10 HF(g) → 2 PF5(g) + 5 H2(g)

d. K(s) + O2(g) → KO2(s)

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Textbook Question

Using data from Appendix C, calculate ΔG° for the following reactions. Indicate whether each reaction is spontaneous at 298 K under standard conditions.

(a) 2 SO2(g) + O2(g) → 2 SO3(g)

(b) NO2(g) + N2O(g) → 3 NO(g)

(c) 6 Cl2(g) + 2 Fe2O3(s) → 4 FeCl3(s) + 3 O2(g)

(d) SO2(g) + 2 H2(g) → S(s) + 2 H2O(g)

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Open Question
Without using thermochemical data, predict whether ΔG° for the reaction involving octane (1C8H182) is more negative or less negative than ΔH°.
Textbook Question

Sulfur dioxide reacts with strontium oxide as follows: SO2(g) + SrO(g) → SrSO3(s) (a) Without using thermochemical data, predict whether ΔG° for this reaction is more negative or less negative than ΔH°.

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Textbook Question

Classify each of the following reactions as one of the four possible types summarized in Table 19.3: (i) spontanous at all temperatures; (ii) not spontaneous at any temperature; (iii) spontaneous at low T but not spontaneous at high T; (iv) spontaneous at high T but not spontaneous at low T.

(a) N2(g) + 3 F2(g) → 2 NF3(g) ΔH° = -249 kJ; ΔS° = -278 J/K

(b) N2(g) + 3 Cl2(g) → 2 NCl3(g) ΔH° = 460 kJ; ΔS° = -275 J/K