Match terms of AG, AG, and AG'with the statements that best describes them. Use each term only once. the free energy difference under conditions of standard state (T = 298K; P = 1 atm; [] of all solutes = 1 M). the free energy difference between products and reactants under actual reaction conditions. the free energy difference between products and reactants under the conditions of biochemical standard state. 1. AG 2. AG 3. AG⁰¹

Match terms of AG, AG, and AG'with the statements that best describes them. Use each term only once. the free energy difference under conditions of standard state (T = 298K; P = 1 atm; [] of all solutes = 1 M). the free energy difference between products and reactants under actual reaction conditions. the free energy difference between products and reactants under the conditions of biochemical standard state. 1. AG 2. AG 3. AG⁰¹

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

For the reaction 2H₂O(1) -> 2H₂(g) + O₂(g) AG = 472 kJ and AH = 572 kJ at 306 K and 1 atm. This reaction is e favored under standard conditions at 306 K. The entropy change for the reaction of 1.51 moles of H₂O(1) at this temperature would be J/K.
For the reaction2 H2O2(l) 2 H2O(l) + O2(g)G° = -227.8 kJ and H° = -196.0 kJ at 253 K and 1 atm.This reaction is (reactant, product) _______ favored under standard conditions at 253 K.The entropy change for the reaction of 1.94 moles of H2O2(l) at this temperature would be_____ J/K.
The standard reaction free energy AG =-1105. kJ for this reaction: Sg(s) + 24 F,(9)→8 SF ,(g) Use this information to complete the table below. Round each of your answers to the nearest kJ. reaction AG x10 4SF, (&) - s,) + 12F,le) S(s) + 12F, (g) |kJ 8SF,(g) → S, (s) + 24F, (g) 6. 3S, (s) + 72F, (g) 24SF, (g) | kJ
Obbs Free E... 2 Consider the following equilibrium: 5.3 Enthalpies of... W S ENTROPY AND FREE ENERGY Using reaction free energy to predict equilibrium composition Under these conditions, will the pressure of NO tend to rise or fall? 2NOCI (g) 2NO(g) + Cl₂ (g) AG-41. KJ Now suppose a reaction vessel is filled with 1.42 atm of nitrosyl chloride (NOCI) and 0.768 atm of nitrogen monoxide (NO) at 928. °C. Answer the following questions about this system: Is it possible to reverse this tendency adding Cl₂? In other words, if you said the pressure of NO will tend to rise, can that be changed to a tendency to fall by adding Cl₂? Similarly, if you said the pressure of NO will tend to fall, can that be changed to a tendency to rise by adding Cl₂? If you said the tendency can be reversed in the second question, calculate the minimum pressure of Cl₂ needed to reverse it. Round your answer to 2 significant digits. Explanation # 3 Check с E 18.5 Gibbs Free E... D 27 $ 4 R F % 5 Ⓒ V Reading Schedule…
G.59.
the free energy for a reaction can be related to the equilibriumconstant through the formula below.K = e (-ΔG° / RT)Therefore if Kc for a reaction is known, Go can be determined, or vice versa. Furthermore, ifyou have the value for Go at two different temperatures, you can calculate H and S throughthe familiar equation for Gibbs energy below, since you have two unknowns but also twoequations.G = H – T SIn this lab you will be studying the solubility of borax (Na2B4O5(OH)4*8H2O), a slightly solublesodium salt, at two different temperatures. When solid borax is added to water, theequilibrium below is established.Na2B4O5(OH)4*8H2O (s) 2 Na+ (aq) + B4O5(OH)42- (aq) + 8 H2O(l)If you measure the concentrations for those substances that show up in the reaction quotient,then the Kc for the reaction at that temperature can be calculated. In this lab, theconcentration of borate ion (B4O5(OH)42-) in solution will be measured by titration with standardhydrochloric acid according to the…
7. FREE GIBBS ENERGY RELATING TO KP ⚫ Consider the decomposition of barium carbonate BaCO3(s) BaO (s)+CO (g) Use data in Appendix A to calculate the equilibrium pressure of CO at a) 298 K and b) 1100 K.
3. - the free energy under the biochemical standard states. Select all that apply. O AG O AG O AG O AG 4. is the free energy of the transition state. O AGt CAG OAG OAG"
Consider the following reaction at 25 * C : 2N2O (g) +O2(g) <—> 4 NO (g) a. At equilibrium, [N2O]=1.00M,[NO]=1.00M, and [O2 ]=0.50 M. Determine the standard Gibbs free energy at the given temperature. b. Using information from part a determine the delta S* when Delta H* =197.7 kJ at 25 degrees * C c. At the given temperature, will products or reactants be favored at equilibrium? Explain two reasons why
6. Who is the proponent of the Gibbs free energy? A. William Friedrich B. Guglielmo Marconi C. William Gibbs D. Janno Gibbs 7. When AG 2H1 (g) if the entropy values for each substance is as follows: H2(g) = 130.6, 12 (s) = 116.7 and HI (g) = 206.3 A. AS = +165.3 J/K B. AS-165.3 J/K C. AS = -41 J/K D. AS = +453.6 J/K 9. What value of Gibbs free energy can we safely predict that the reaction is spontaneous at all temperatures? A. a negative value C. a positive value at a low temperature B. a positive value D. a positive value at a high temperature 10. What will be the value of the entropy change of the system in the reaction: 6CO₂(g) + 6H₂O(g) → C6H12O6(g) + 602(g) ? C. no change D. cannot be determined A. positive B. negative 11. Ozone (03) in the atmosphere can react with nitric oxide (NO): Os(g) + NO(g) -> NO2(g) + O2(g) Calculate the G for this reaction at 25°C. (AH = -199 kJ/mol, AS = -4.1 J/K-mol) A. -198 kJ/mol B. +198 kJ/mol C.-301.5 kJ/mol D. +301.5 kJ/mol 12. Which of the…
Explain pleaseeeeeeeeeee