Question 1 Which of the following is NOT true for AGrxn? A) If AG°rxn> 0, the reaction is spontaneous in the forward direction. B) If Q=1, then AGrxn= AGᵒrxn. C) If AG°rxn< 0, the reaction is spontaneous in the forward direction. D) If AGºrxn> 0, the reaction is spontaneous in the reverse direction. E) Under equilibrium conditions, AGrxn= 0. OA ОВ OC OD OE Question 2 Determine the equilibrium constant for the following reaction at 498 K. A) 1.87 x 1010 B) 8.10 × 1031 C) 2.31 x 10-22 D) 5.34 x 10-11 E) 4.33 x 1021 OA OB OC 2 Hg(g) + O2(g) → 2 HgO(s) AH° = -304.2 kJ; AS° = -414.2 J/K OD

Question 1 Which of the following is NOT true for AGrxn? A) If AG°rxn> 0, the reaction is spontaneous in the forward direction. B) If Q=1, then AGrxn= AGᵒrxn. C) If AG°rxn< 0, the reaction is spontaneous in the forward direction. D) If AGºrxn> 0, the reaction is spontaneous in the reverse direction. E) Under equilibrium conditions, AGrxn= 0. OA ОВ OC OD OE Question 2 Determine the equilibrium constant for the following reaction at 498 K. A) 1.87 x 1010 B) 8.10 × 1031 C) 2.31 x 10-22 D) 5.34 x 10-11 E) 4.33 x 1021 OA OB OC 2 Hg(g) + O2(g) → 2 HgO(s) AH° = -304.2 kJ; AS° = -414.2 J/K OD

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

Chapter17: Spontaneity, Entropy, And Free Energy

Section: Chapter Questions

Problem 27Q: Consider the reaction N2O2(g) 2NO2(g) where PNO2=0.29 atm and PN2O4=1.6. For this reaction at these...

See similar textbooks

Similar questions

At 298 K, G = 70.52 kJ for the reaction 2NO(g) + O2(g) 2NO2(g) (a) Calculate _G at the same temperature when PNO = 1.0 104 atm, PO2=2.0103 atm, and PNO2=0.30 atm. (b) Under the conditions in part a, in which direction is the reaction spontaneous?
On the basis of your experience, predict which of the following reactions are spontaneous. (a) CO2(s)CO2(g) at 25C (b) NaCl(s)NaCl(l) at 25C (c) 2NaCl(s)2Na(s)+Cl2(g)(d) CO2(g)C(s)+O2(g)
On the basis of your experience, predict which of the following reactions are spontaneous. (a) CO2(s)CO2(g) at 25°C (b) NaCl(s)NaCl(l) at 25°C (c) 2NaCl(s)2Na(s)+Cl2(g) (d) CO2(g)C(s)+O2(g)
Consider the decomposition of red mercury(II) oxide under standard state conditions.. 2HgO(s,red)2Hg(l)+O2(g) (a) Is the decomposition spontaneous under standard state conditions? (b) Above what temperature does the reaction become spontaneous?
Many plastic materials are organic polymers that contain carbon and hydrogen. The oxidation of these plastics in air to farm carbon dioxide and water is a spontaneous process; however, plastic materials tend to persist in the environment. Explain.
Show by calculation, using Appendix 1, whether dissolving lead(II) chloride PbCl2(s)Pb2+(aq)+2Cl(aq) is spontaneous at 25C (a) when [ Pb2+ ]=1.0M;[ Cl ]=2.0M. (b) when [ Pb2+ ]=1.0105M;[ Cl ]=2.0105M.
Given that H f for HF(aq) is -320.1 kJ/mol and S for HF(aq) is 88.7 J/mol K, find Ka for HF at 25C.
Calculate S for the dissolution of magnesium chloride: MgCl2(s)Mg2+(aq)+2Cl(aq) . Use your understanding of the solvation of ions at the molecular level to explain the sign of S .
In a spontaneous process, S(universe) is (a) 0 (b) = 0 (c) 0
Calculate H and G for the following reactions at 25C, using thermodynamic data from Appendix C; interpret the signs of H and G. a 2PbO(s)+N2(g)2Pb(s)+2NO(g)\ b CS2(l)+2H2O(l)CO2(g)+2H2S(g)
The free energy change, G, for a process at constant temperature and pressure is related to Suniv and reflects the spontaneity of the process. How is G related to Suniv? When is a process spontaneous? Nonspontaneous? At equilibrium? G is a composite term composed of H, T, and S. What is the G equation? Give the four possible sign combinations for H and S. What temperatures are required for each sign combination to yield a spontaneous process? If G is positive, what does it say about the reverse process? How does the G = H TS equation reduce when at the melting-point temperature of a solid-to-liquid phase change or at the boiling-point temperature of a liquid-to-gas phase change? What is the sign of G for the solid-to-liquid phase change at temperatures above the freezing point? What is the sign of G for the liquid-to-gas phase change at temperatures below the boiling point?
Explain why absolute entropies can be measured.