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19. Chemical Thermodynamics

Gibbs Free Energy And Equilibrium

19. Chemical Thermodynamics

Gibbs Free Energy And Equilibrium

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∆G° and K Example

∆G° and K Example

∆G, ∆G° and Q

∆G, ∆G°, and Q Example

∆G, ∆G°, and Q 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/mol*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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Open Question
NaHCO₃ ⇌ NaOH(s) + CO₂(g) Calculate the value of the equilibrium constant.
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Open Question
Calculate the equilibrium constant at 25°C for a reaction for which ∆G° = -4.22 kcal/mol.
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Open Question
What is δg° for the following reaction at 25 °C? COBr₂(g) ⇌ CO(g) + Br₂(g) K_p = 4.11 × 10⁴
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Open Question
When two reactions are coupled in a cell, what determines if they will both proceed spontaneously?
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Multiple Choice
A redox reaction has an equilibrium constant of K = 1.2 x 10^3. Which statement is true regarding ΔG°_rxn and E°_cell for this reaction?
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Multiple Choice
At 1120 K, ΔG° = 78.9 kJ/mol for the reaction 3 A (g) + B (g) → 2 C (g). If the partial pressures of A, B, and C are 11.5 atm, 8.60 atm, and 0.510 atm respectively, what is the Gibbs free energy change (ΔG) for this reaction under these conditions?
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