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.
19. Chemical Thermodynamics
Gibbs Free Energy And Equilibrium
Back19. Chemical Thermodynamics
Gibbs Free Energy And Equilibrium
- 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 Keq of this given reaction.
- Open Question
NaHCO3 ⇌ NaOH(s) + CO2(g) Calculate the value of the equilibrium constant.
- Open Question
Calculate the equilibrium constant at 25°C for a reaction for which ∆G° = -4.22 kcal/mol.
- Open Question
What is δg° for the following reaction at 25 °C? COBr2(g) ⇌ CO(g) + Br2(g) Kp = 4.11 × 104
- Open Question
When two reactions are coupled in a cell, what determines if they will both proceed spontaneously?
- Open Question
Br2(g) + Cl2(g) → BrCl(g) ΔG°f for brcl(g) is -1.0 kj/mol
- Multiple ChoiceA 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?
- Multiple ChoiceAt 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?
- Multiple ChoiceCalculate ΔG°rxn at 298 K for the following reaction: I2(g) + Cl2(g) ⇌ 2ICl(g), given that Kp = 81.9. Which of the following is the correct value of ΔG°rxn?
- Multiple ChoiceCalculate the Gibbs free energy change (ΔG_rxn) at 298 K for the reaction N2 (g) + 3 H2 (g) ⇌ 2 NH3 (g) given the standard Gibbs free energy change (ΔG° = -33.3 kJ) and the partial pressures: P(N2) = 1.5 atm, P(H2) = 4.5 atm, P(NH3) = 6.0 atm.
- Multiple ChoiceCalculate the Gibbs free energy change (ΔGᵣₓₙ) at 298 K for the reaction N₂ (g) + 3 H₂ (g) ⇌ 2 NH₃ (g) given the standard Gibbs free energy change (ΔG° = -33.3 kJ) and the partial pressures: P(N₂) = 1.5 atm, P(H₂) = 4.5 atm, P(NH₃) = 1.0 atm.
- Multiple ChoiceGiven the reaction Cl2(g) + 2NO(g) → 2NOCl(g), if the standard Gibbs free energy change (ΔG°) for the reaction is negative, what can be concluded about the reaction at standard conditions?
- Multiple ChoiceDetermine the minimum pressure of N₂ required to keep the reaction N₂(g) + 3 H₂(g) ⇌ 2 NH₃(g) spontaneous at 298 K, given ΔG°rxn = -33.3 kJ/mol, P H₂ = 1.00 x 10⁻² atm, and P NH₃ = 1.00 atm.
- Multiple ChoiceEstimate the value of the equilibrium constant at 660 K for the reaction 2NO2(g) ⇌ N2O4(g) given that ΔG°f for BrCl(g) is -1.0 kJ/mol and the standard molar entropy, S°, for BrCl(g) is 240.0 J/mol⋅K. Assume ΔH°f for N2O4(g) is -9.2 kJ/mol and ΔH°f for NO2(g) is 33.2 kJ/mol.