(a)
Interpretation:
Change in
Concept introduction:
Gibbs free energy change
Gibbs free energy change
Equilibrium constant: The relative concentration of reactants and products at equilibrium can be expressed by equilibrium constant.
For a general reaction
Gibbs free energy change: The difference between the free energy of the products and the free energy of reactants under standard conditions is called Gibbs free energy change.
(b)
Interpretation:
The variation of
Concept introduction:
Gibbs free energy change
Gibbs free energy change
(c)
Interpretation:
The variation of
Concept introduction:
Gibbs free energy change
Gibbs free energy change
Want to see the full answer?
Check out a sample textbook solutionChapter 5 Solutions
Organic Chemistry (8th Edition)
- 24. At 460 K, ∆G = -11.2 kJ/mol for the reaction 2 A (g) → B (g). If the partial pressures of A and B are 7.20 atm and 0.420 atm respectively, what is ∆G° for this reaction?arrow_forward1. For the reaction at 25̊ C, find ∆G° and determine what type of reaction/processtakes place.a. C2H6(g) C2H4(g) + H2(g)Given: ∆H° = +137 kJ and ∆S° = 120 J/Kb. 2H2(g) + O2(g) 2H2O(g)Given: ∆H° = -241.82 kJ and ∆S° = -233.7 J/Karrow_forwardWhat is the equilibrium constant for a reaction that is carried out at 25 °C (298 K) with ∆H° = 20 kcal/mol and ∆S° = 5.0 * 10-2 kcal mol -1 K-1? What is the equilibrium constant for the same reaction carried out at 125 °C?arrow_forward
- From the values of ∆H and ∆S, what would be the value of ∆G at 25.0°C? Reaction B: ∆H = -15.80 kJ/mol ∆S = - 125.0 J/K . mol ∆G = ? At what specific temperature would the ∆G be equal to zero (0); ∆G = 0? T = ? * 1 kJ/mol = 1000 J/mol * 1.0 °C =273.15 Karrow_forwardWhat is the value of ∆G°(kJ mol–1 ) for this reaction at 175.4 oC ? The data refer to 25 oC: 2 NO(g) + Cl2(g) ⟶ 2 NOCl(g) Substance NO(g) Cl2(g) NOCl(g) ∆H°f (kJ mol–1) 90.29 0 51.71 ∆G°f (kJ mol–1) 86.60 0 66.07 S° (J K–1 mol–1) 210.65 223.0 261.6 (the answer should be entered with 3 significant figures; do not enter units; give answer in normal notation--examples include 1.23 and 120. and -123 and 123. and 12.3) Calculate ΔG in kJ•mol-1 at 298 K for the following reaction: under the following conditions: (the answer should be entered with 3 significant figures; do not enter units; give answer in scientific notation--valid notation examples include 1.23e-8 and 1.23e8 and -1.23e-4 and 1.23e0) P(A) = 0.397 atm, P(AB) = 0.792 atm 2 A(g) + B2(s) → 2 AB(g) ΔGo = -182 kJ•mol-1 The redox reaction below has a ΔG° value of 209. kJ. Determine the standard cell potential(E°cell) for…arrow_forwardPredict the spontaneity of a reaction (and the temperaturedependence of the spontaneity) for each possible combination ofsigns for ∆H and ∆S (for the system).a. ∆H negative, ∆S positiveb. ∆H positive, ∆S negativec. ∆H negative, ∆S negatived. ∆H positive, ∆S positivearrow_forward
- What is the overall standard free energy change when the following two reactions are coupled? A + B → C ; ∆G°rxn = ∆G1 C + D → E ; ∆G°rxn = ∆G2 Options: A. ∆G1/∆G2 B. ∆G1 – ∆G2 C. ∆G1 + ∆G2 D. ∆G2 – ∆G1 E. ∆G1∆G2arrow_forwardConsider 8 the following reaction: 2NH3(g) + CO2(g) → NH2CONH2(aq) + H2O(l) ∆G° = -13.6 kJ at 25°C What is the value of ∆G at 25°C for this reaction under the following set of conditions? 25.0 atm NH3 (g) 0.500 atm CO2 (g) 1.00 M NH2CONH2 (aq) Group of answer choices -18.1 kJ 0.63 kJ -27.8 kJ 14.2 kJ -20.0 kJarrow_forwardThe reaction: A + B going to C + D has a ∆Go of +64 kJ/mol. A. What is the ∆G for the reaction if the cellular concentrations of A and B are 10 μM and the concentration of C and D are 1mM? B. Can hydrolysis of ATP to AMP drive this reaction forward? Why? (∆G for the hydrolysis of phosphoanhydride bonds is -33Kj/mol).arrow_forward
- The ∆Ssur, depends on temperature and a. ∆Suniv b. ∆H0sys c. ∆Ssys d. ∆G0sysarrow_forwardA 0.15 M aqueous solution of a weak acid (HA) has a pH of 4.55 at 25 C. What is the ∆G for the ionization of this acid?arrow_forward1. Which of the relationships between the free energy change of a system and associated entropy changes is true? a. ∆Gsys = +T∆Ssys b. ∆Gsys = -T∆Ssys c. ∆Gsys = +T∆Suniv d. ∆Gsys = -T∆Sunivarrow_forward
- Chemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningWorld of Chemistry, 3rd editionChemistryISBN:9781133109655Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCostePublisher:Brooks / Cole / Cengage Learning
- Chemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning