A) This reaction will be spontaneous only at high temperatures. B) This reaction will be spontaneous at all temperatures. c) This reaction will be nonspontaneous at all temperatures. D) This reaction will be nonspontaneous only at high temperatures. E) It is not possible to determine without more information. 27. If solid barium hydroxide octahydrate is mixed in a beaker with solid ammonium chloride, they react in a highly endothermic process that absorbs so much heat from the surroundings that water on the outside of the beaker freezes: This reaction is: Ba(OH)2*8H2O(s) + 2NH4Cl(s) → BaCl2(aq) + 2NH3(g) + 10 H2O(l) A) Never spontaneous B) Always spontaneous C) Spontaneous because of the large increase in entropy D) Spontaneous because of the large decrease in entropy F) Spontaneous herause of the large negative AH

A) This reaction will be spontaneous only at high temperatures. B) This reaction will be spontaneous at all temperatures. c) This reaction will be nonspontaneous at all temperatures. D) This reaction will be nonspontaneous only at high temperatures. E) It is not possible to determine without more information. 27. If solid barium hydroxide octahydrate is mixed in a beaker with solid ammonium chloride, they react in a highly endothermic process that absorbs so much heat from the surroundings that water on the outside of the beaker freezes: This reaction is: Ba(OH)2*8H2O(s) + 2NH4Cl(s) → BaCl2(aq) + 2NH3(g) + 10 H2O(l) A) Never spontaneous B) Always spontaneous C) Spontaneous because of the large increase in entropy D) Spontaneous because of the large decrease in entropy F) Spontaneous herause of the large negative AH

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...

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Consider a reaction that has a negative AH and a positive AS. Which of the following statements is true? A) This reaction will be spontaneous only at high temperatures. B) This reaction will be spontaneous at all temperatures. c) This reaction will be nonspontaneous at all temperatures. D) This reaction will be nonspontaneous only at high temperatures. E) It is not possible to determine without more information. If solid barium hydroxide octahydrate is mixed in a beaker with solid ammonium chloride, they reac highly endothermic process that absorbs so much heat from the surroundings that water on the out the beaker freezes: This reaction is: Ba(OH)2*8H2O(s) + 2NH4Cl(s) → BaCl2(aq) + 2NH3(g) + 10 H₂O(1) A) Never spontaneous B) Always spontaneous C) Spontaneous because of the large increase in entropy
2. Define and give an example: Spontaneous, exergonic 3. Define and give an example: Non-spontaneous, endergonic
please help
28. Define free energy, and how heat and entropy play a role in the equation. What is the relationship between the free energy and the equilibrium constant with regards to how a reaction will proceed?
1. A potential chemical reaction at 25.0 °C has a ΔHrxn of 147.5 kJ and a ΔSrxn of -386.9 J/K. What is the ΔGrxn in kJ. (Enter answer to 3 significant figures and include no units in your answer) Also, what is true about the potential reaction in the previous problem? a. spontaneous b. illegal c. combustive d. nonspontaneous
If this has a negative value for a process, then the process occurs spontaneously. A. Free energy change (ΔG) B. Entropy change (ΔS) C. Enthalpy change (ΔH) D. Heat of vaporization
if the enthalpy change is negative and the entropy change is positive this reaction would be a) spontaneous at all temperatures b) spontaneous at high temperatures only c) nonspontaneous at all temperatures d) spontaneous at low temperatures only
A process that takes place so slowly as to be capable of reversing direction in response to an infinitesimally small change in conditions is defined as which of the following terms? O Nonspontaneous process Spontaneous change O Irreversible process Reversible process
For a given reaction, dH = 32 kJ/mol and dS = 117 J/mol. At approximately what temperature would this reaction become spontaneous?