2) The equilibrium constant Keq for the reaction A B is 1 x 105 at room temperature (25°C). a) You make a solution containing compound A at a concentration of 1 M and compound B at a concentration of 1 mM of B, and let the reaction proceed to equilibrium. What are the equilibrium concentrations of A and B? b) Calculate the standard free-energy change (AG) for this reaction. c) What is the standard free-energy change (AG) for the inverse reaction (BA)? d) With the provided information, can you estimate how long will it take this reaction to reach equilibrium? e) In a reaction cell that has not reached equilibrium, we have the following instantaneous concentrations: [A] = 0.05 mM; [B] = 15 mM. Calculate the actual free-energy change (AG) for the system as it reaches equilibrium at 25°C.

2) The equilibrium constant Keq for the reaction A B is 1 x 105 at room temperature (25°C). a) You make a solution containing compound A at a concentration of 1 M and compound B at a concentration of 1 mM of B, and let the reaction proceed to equilibrium. What are the equilibrium concentrations of A and B? b) Calculate the standard free-energy change (AG) for this reaction. c) What is the standard free-energy change (AG) for the inverse reaction (BA)? d) With the provided information, can you estimate how long will it take this reaction to reach equilibrium? e) In a reaction cell that has not reached equilibrium, we have the following instantaneous concentrations: [A] = 0.05 mM; [B] = 15 mM. Calculate the actual free-energy change (AG) for the system as it reaches equilibrium at 25°C.

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter17: Chemcial Thermodynamics

Section: Chapter Questions

Problem 17.79QE

See similar textbooks

Similar questions

2) The equilibrium constant Ke for the reaction A B is 1 x 105 at room temperature (25°C). a) You make a solution containing compound A at a concentration of 1 M and compound B at a concentration of 1 mM of B, and let the reaction proceed to equilibrium. What are the equilibrium concentrations of A and B? b) Calculate the standard free-energy change (AG) for this reaction. c) What is the standard free-energy change (AG) for the inverse reaction (BA)?
For the reaction: PC15(g) + heat <> PCI3(g) + CI2 (g). How will the following affect the equilibrium? a) Reduction of PCI5, b) Increase in pressure, c) Removal of heat, d) Addition of CI2
The difference in standard free energy between reactant R and product P is + 7.5 kJ/mol. What’s the ratio of P to R at equilibrium? P to R ratio =
Consider the following equilibrium reaction: 2 CH3OH + CH2O ⇌CH2(OCH3)2+ H2O ΔH = + 46 cal Indicate the direction that the equilibrium will shift when the following changes are made.(No states are provided because the solvent for the reaction is not water, so aq for aqueous would not be appropriate.) (d)How does the equilibrium constant (Keq) change when temperature is decreased?
5. One of the key steps in the tricarboxylic acid (TCA) cycle is the hydration of fumarate to malate: Fumarate-² + H₂O = Malate-2 The standard reaction Gibbs free energy and enthalpy for this reactions are -880 cal/mol and 3560 cal/mol, respectively. (a) What is the equilibrium constant for this reaction (25 °C)? (b) Is the reaction favorable (spontaneous) at 25 °C? (c) What is the equilibrium constant of this reaction under physiological conditions (37 °C)? (d) Is this reaction favorable at 37 °C?
Consider the following reaction at equilibrium: CO(g) + H₂O(g) ⇌ CO₂(g) + H₂(g) If CO(g) is removed, how will K(eq) change?
1. Calculate the standard reaction free energy of the following chemical reaction:
A student determines the value of the equilibrium constant to be 8.18x10-37 for the following reaction. H₂S(g) + 2H₂O(l)—3H₂(g) + SO₂(g) Based on this value of Keq: AG° for this reaction is expected to be (greater, less) zero. than Calculate the free energy change for the reaction of 1.68 moles of H₂S(g) at standard conditions at 298K. AG rxn= kJ
9. For the reaction: 2 CH,OH(g) + H2(g) - C2H(g) + 2 H2O(g) a) Calculate AG° for this reaction using free energy values in your text book. b) Calculate AG at standard temperature when the pressure of CH3OH is 4.97 atm, H2 is 3.56 atm, C2H6 is 4.85 atm, and H20 is 2.18 atm. c) Calculate Kp for this reaction
A student determines the value of the equilibrium constant to be 3.67×10-18 for the following reaction. Fe3O4(s) + 4H₂(g) →→→3Fe(s) + 4H₂O(g) Based on this value of Keq: AGO for this reaction is expected to be (greater, less) than zero. Calculate the free energy change for the reaction of 1.67 moles of Fe3O4(s) at standard conditions at 298K. AGᵒrxn KJ
The following equilibrium constants have been determined for hydrosulfuric acid at 25ºC: H2S(aq) ⇌ H+(aq) + HS–(aq) K′c = 9.5 × 10–8 HS–(aq) ⇌ H+(aq) + S2–(aq) K″c = 1.0 × 10–19 Calculate the equilibrium constant for the following reaction at the same temperature. H2S(aq) ⇌ 2H+(aq) + S2–(aq)
4. Ethylene reacts with bromine to produce 1,2,- dibromoethane. At equilibrium, the concentration of each compound were found to be: C₂H4 = 0.5M; Br₂ = 4M; C₂H4Br2 = 1.7M Calculate the value of the equilibrium constant.

SEE MORE QUESTIONS

Recommended textbooks for you

Chemistry: Principles and Practice

Chemistry

ISBN:

9780534420123

Author:

Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:

Cengage Learning

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

Chemistry: The Molecular Science

Chemistry

ISBN:

9781285199047

Author:

John W. Moore, Conrad L. Stanitski

Publisher:

Cengage Learning

Chemistry: Principles and Practice

Chemistry

ISBN:

9780534420123

Author:

Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:

Cengage Learning

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

Chemistry: The Molecular Science

Chemistry

ISBN:

9781285199047

Author:

John W. Moore, Conrad L. Stanitski

Publisher:

Cengage Learning

SEE MORE TEXTBOOKS