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

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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)?
Solve question 2
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?
Suppose the following reaction is at equilibrium: PCl3 + Cl2 ⇋ PCl5; (a) Are the equilibrium concentrations of PCl3, Cl2, and PCl5 necessarily equal? Explain. (b) Is the equilibrium concentration of PCl3 necessarily equal to that of Cl2? Explain.
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
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.
Acetaldehyde (CH3CHO) is an important chemical both industrially and biologically. For instance, it is a (somewhat toxic) intermediate in the body's metabolism of ethanol into acetic acid, and thus is possibly implicated in the "hungover" symptoms of someone who has had too much to drink the night before. In aqueous solution, it establishes an equilibrium with a hydrated form, shown below. CH3CHO (aq) + H2O (l) <--> CH3CH(OH)2 (aq) You start with an aqueous sample, already at equilibrium, with the CH3CH(OH)2 (the hydrated form) at a concentration of 2.60 M. You have no information about how much, if any, of the anhydrous form (CH3CHO) is initially in the flask. If you add 2.0 M of CH3CHO to the reaction flask, and as the equilibrium is being restored the amount of CH3CH(OH)2 changes by 1.13 M, what is the final amount of CH3CHO?
1

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