19. Chemical Thermodynamics

Gibbs Free Energy And Equilibrium

19. Chemical Thermodynamics

Gibbs Free Energy And Equilibrium

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Gibbs Free Energy And Equilibrium Example

Gibbs Free Energy And Equilibrium Example

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Multiple Choice

For reaction, Ag₂CO₃ (s) ⇌ Ag₂O (s) + CO₂ (g), the ∆Hº = 79.14 kJ/mol, ∆Sº = 167.2 J/K.

Determine the equilibrium constant at which the temperature is 365.1 K.

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Multiple Choice

Consider a hypothetical reaction at 38 ºC, X₂ (aq) + 2 Y (s) ⇌ 3 Z (aq), with a ∆G of −75.8 kJ.

Concentrations of reactants and products: [X₂] = 1.4 M, [Y] = 0.34 M, [Z] = 2.6 M. Calculate K_eq of this given reaction.

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Textbook Question

Consider the sublimation of iodine at 25.0 °C : I2(s) ¡ I2( g) b. Find ΔG rxn at 25.0 °C under the following nonstandard conditions: i. PI2 = 1.00 mmHg ii. PI2 = 0.100 mmHg

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Textbook Question

Consider the evaporation of methanol at 25.0 °C : CH3OH(l ) ¡ CH3OH( g) b. Find ΔG r at 25.0 °C under the following nonstandard conditions: i. PCH3OH = 150.0 mmHg ii. PCH3OH = 100.0 mmHg iii. PCH3OH = 10.0 mmHg

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Textbook Question

Formation constants for the ammonia and ethylenediamine complexes of nickel(II) indicate that Ni(en)₃²⁺ is much more

stable than Ni(NH₃)₆²⁺:

(1) <REACTION>

(2) <REACTION>

The enthalpy changes for the two reactions, ΔH°₁ and ΔH°₂, should be about the same because both complexes have six Ni﹣N bonds.

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Textbook Question

Spinach contains a lot of iron but is not a good source of dietary iron because nearly all the iron is tied up in the oxalate complex [Fe(C₂O₄)₃]^3-.

(b) Under the acidic conditions in the stomach, the Fe³⁺ concentration should be greater because of the reaction

[Fe(C₂O₄)₃]^3-(aq) + 6 H₃O⁺(aq) ⇌ Fe³⁺(aq) + 3 H₂C₂O₄(aq) + 6 H₂O(l)

Show, however, that this reaction is nonspontaneous under standard-state conditions. (For H₂C₂O₄, K_a1 = 5.9 × 10^-2 and K_a2 = 6.4 × 10^-5.)

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Textbook Question

Nitrogen reacts with fluorine to form nitrogen trifluoride: Calculate ∆G°, and determine whether the equilibrium composition should favor reactions or products at 25 °C (a) ∆G° = -6.7 kJ; the equilibrium composition should favor products. (b) ∆G° = -332 kJ; the equilibrium composition should favor reactants (c) ∆G° = -166 kJ; the equilibrium composition should favor products (d) ∆G° = +82.6 kJ; the equilbirum composiiton should favor reactants.

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Textbook Question

Ammonium hydrogen sulfide, a stink bomb ingredient, decomposes to ammonia and hydrogen sulfide: Calculate the standard free-energy change for the rection at 25 °C if the total pressure resulting from the solid NH4S placed in an evacuated container is 0.658 atm at 25 °C. (a) -43.8 kJ (b) +1.04 kJ (c) -462 kJ (d) +5.51 kJ

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Textbook Question

Consider the reaction: CO2( g) + CCl4( g) ∆ 2 COCl2( g) Calculate ΔG for this reaction at 25 °C under the following conditions: i. PCO2 = 0.112 atm ii. PCCl4 = 0.174 atm iii. PCOCl2 = 0.744 atm

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Textbook Question

Use data from Appendix IIB to calculate the equilibrium constants at 25 °C for each reaction. b. 2 H2S( g) ∆ 2 H2( g) + S2( g)

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Textbook Question

Use data from Appendix IIB to calculate the equilibrium constants at 25 °C for each reaction. a. 2 CO( g) + O2( g) ∆ 2 CO2( g)

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Textbook Question

Consider the reaction: I2( g) + Cl2( g) ∆ 2 ICl( g) K p = 81.9 at 25 °C Calculate ΔG rxn for the reaction at 25 °C under each of the following conditions: a. standard conditions

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Textbook Question

Consider the reaction: I2( g) + Cl2( g) ∆ 2 ICl( g) K p = 81.9 at 25 °C Calculate ΔG rxn for the reaction at 25 °C under each of the following conditions: b. at equilibrium

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Textbook Question

Consider the reaction: I2( g) + Cl2( g) ∆ 2 ICl( g) K p = 81.9 at 25 °C Calculate ΔG rxn for the reaction at 25 °C under each of the following conditions: c. PICl = 2.55 atm; PI2 = 0.325 atm; PCl2 = 0.221 atm

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Textbook Question

Consider the reaction 2 NO21g2¡N2O41g2. (a) Using data from Appendix C, calculate ΔG° at 298 K. (b) Calculate ΔG at 298 K if the partial pressures of NO2 and N2O4 are 0.40 atm and 1.60 atm, respectively.

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Textbook Question

Consider the reaction 3 CH41g2¡C3H81g2 + 2 H21g2. (b) Calculate ΔG at 298 K if the reaction mixture consists of 40.0 atm of CH4, 0.0100 atm of C3H81g2, and 0.0180 atm of H2.

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