For each chemical reaction listed in the first column of the table below, predict the sign (positive or negative) of the reaction entropy ASxn. If it's not possible to decide with the information given, check the "not enough information" button in the last column. Note for advanced students: Assume the temperature remains constant. Assume all gases and solutions are ideal. reaction 2C₂H6 (g) + 70₂ (g) 4CO₂(g) + 6H₂O(g) 2SO₂(g) + O₂(g) 2SO3(g) MgCl₂ (s) + H₂O (1) → MgO (s) + 2HCl (g) sign of reaction entropy AS < 0 rxn Ο ΔS > 0 rxn Onot enough information. O AS < 0 rxn O AS > 0 rxn Onot enough information. O AS < 0 rxn O AS > 0 rxn

For each chemical reaction listed in the first column of the table below, predict the sign (positive or negative) of the reaction entropy ASxn. If it's not possible to decide with the information given, check the "not enough information" button in the last column. Note for advanced students: Assume the temperature remains constant. Assume all gases and solutions are ideal. reaction 2C₂H6 (g) + 70₂ (g) 4CO₂(g) + 6H₂O(g) 2SO₂(g) + O₂(g) 2SO3(g) MgCl₂ (s) + H₂O (1) → MgO (s) + 2HCl (g) sign of reaction entropy AS < 0 rxn Ο ΔS > 0 rxn Onot enough information. O AS < 0 rxn O AS > 0 rxn Onot enough information. O AS < 0 rxn O AS > 0 rxn

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter17: Chemcial Thermodynamics

Section: Chapter Questions

Problem 17.80QE

See similar textbooks

Similar questions

For one day, keep a log of all the activities you undertake that consume Gibbs free energy. Distinguish betweenGibbs free energy provided by nutrient metabolism andthat provided by other energy resources.
Explain why absolute entropies can be measured.
For each process, tell whether the entropy change of the system is positive or negative. (a) A glassblower heats glass (the system) to its softening temperature. (b) A teaspoon of sugar dissolves in a cup of coffee. (The system consists of both sugar and coffee.) (c) Calcium carbonate precipitates out of water in a cave to form stalactites and stalagmites. (Consider only the calcium carbonate to be the system.)
What is entropy? Why is entropy important?
A key component in many chemical engineering designs is the separation of mixtures of chemicals. (a) What happens to the entropy of the system when a chemical mixture is separated? (b) Are designs for chemical separation more likely to rely on spontaneous or nonspontaneous processes?
Chemists and engineers who design nuclear power plants have to worry about high-temperature reactions because it is possible for water to decompose. (a) Under what conditions does this reaction occur spontaneously? 2H2O(g) 2H2(g) + O2(g) (b) Under conditions where the decomposition of water is spontaneous, do nuclear engineers have to worry about an oxygen/hydrogen explosion? Justify your answer.
Define the following: a. spontaneous process b. entropy c. positional probability d. system e. surroundings f. universe
The standard molar entropy of methanol vapor, CH3OH(g), is 239.8 J K1 mol-1. (a) Calculate the entropy change for the vaporization of 1 mol methanol (use data from Table 16.1 or Appendix J). (b) Calculate the enthalpy of vaporization of methanol, assuming that rS doesnt depend on temperature and taking the boiling point of methanol to be 64.6C.
What is the sign of the standard Gibbs free-energy change at low temperatures and at high temperatures for the synthesis of ammonia? 3H2(g) + N2(g) 2NH3(g)
The molecular scale pictures below show snapshots of a strong acid at three different instants after it is added to water. Place the three pictures in the correct order so that they show the progress of the spontaneous process that takes place as the acid dissolves in the water. Explain your answer in terms of entropy