(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; Modified MasteringChemistry with Pearson eText -- ValuePack Access Card; Study Guide and Student Solutions Manual for Organic Chemistry, Books a la Carte Edition (7th Edition)
- At 25 oC an antibody binds a protein with a ∆H = -87.9 kJ/mol and ∆S = -118.9 J mol-1 K-1 Which of the following is/are true? (Choose all that are correct) a. The process is exergonic b. The process is endothermic c. The entropy of the binding process increases d. The binding process is exothermic e. The entropy during the binding process decreasesarrow_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_forwardWhat 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_forward
- Consider 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_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_forwardThe ∆Ssur, depends on temperature and a. ∆Suniv b. ∆H0sys c. ∆Ssys d. ∆G0sysarrow_forward
- A 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_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_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