This question deals with the vapourization of acetone:CH;COCH,() - CH,COCH,(g)Part AThe boiling point of acetone is 329.3 Kand the enthalpy of vaporization, Ava,H =29.07 kJ mol1.Compute the standard entropy of vapourization, Avan S° of acetone.O -95 JK mol1O -88.28 JK' molO 95 JK' mol1O 88.28 J K' molO -11.33 JK mol

We will use the realtion of ∆H and ∆S

CH;COCH,() = CH,COCH,(G) Part A The boiling point of acetone is 320.3 Kand the enthalpy of vaporization, Avap = 20.07 kJ mol1. Compute the standard entropy of vapourization, Avap S° of acetone. O -65 JK' mol O -88.28 JK mol 1. O 95 JK' mol O 88.28 J K mol O -11.33 JK' mol

CH;COCH,() = CH,COCH,(G) Part A The boiling point of acetone is 320.3 Kand the enthalpy of vaporization, Avap = 20.07 kJ mol1. Compute the standard entropy of vapourization, Avap S° of acetone. O -65 JK' mol O -88.28 JK mol 1. O 95 JK' mol O 88.28 J K mol O -11.33 JK' mol

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter16: Thermodynamics: Directionality Of Chemical Reactions

Section: Chapter Questions

Problem 121QRT

See similar textbooks

Similar questions

For the process A(l) A(g), which direction is favored by changes in energy probability? Positional probability? Explain your answers. If you wanted to favor the process as written, would you raise or lower the temperature of the system? Explain.
Calculate the standard Gibbs free-energy change when SO3 forms from SO2 and O2 at 298 K. Why is sulfur trioxide an important substance to study? (Hint: What happens when it combines with water?)
What is the sign of the standard Gibbs free-energy change at low temperatures and at high temperatures for the explosive decomposition of TNT? Use your knowledge of TNT and the chemical equation, particularly the phases, to answer this question. (Thermodynamic data for TNT are not in Appendix G.) 2C7H5N3O6(s) 3N2(g) + 5H2O() + 7C(s) + 7CO(g)
Billions of pounds of acetic acid are made each year, much of it by the reaction of methanol with carbon monoxide. (AssumeT= 298 K.) CH3OH() + CO(g) CH3COOH() (a) By calculating the standard Gibbs free energy change, rG, for this reaction, show that it is product-favored. (b) Determine the standard Gibbs free energy change, rG,for the reaction of acetic acid with oxygen to form gaseous carbon dioxide and liquid water. (c) Based on this result, is acetic acid thermodynamicallystable compared with CO2(g) and H2O()? (d) Is acetic acid kinetically stable compared with CO2(g)and H2O()?
What is the sign of the standard Gibbs free-energy change at low temperatures and at high temperatures for the formation of hydrogen sulfide from the elements? H2(g)+18S8(s)H2S(g)
Determine the standard Gibbs free energy change, rG, for the reactions of liquid methanol, of CO(g), and ofethyne, C2H2(g), with oxygen gas to form gaseous carbondioxide and (if hydrogen is present) liquid water at298 K. Use your calculations to decide which of thesesubstances are kinetically stable and which are thermodynamically stable: CH3OH(), CO(g), C2H9(g), CO2(g),H2O().
Would the amount of heat absorbed by the dissolution in Example 5.6 appear greater, lesser, or remain the same if the heat capacity of the calorimeter were taken into account? Explain your answer.
It has been demonstrated that buckminsterfullerene (C60), another allotrope of carbon (Section 2.3), may be converted into diamond at room temperature and 20,000 atmospheres pressure (about 2 GPa). The standard enthalpy of formation, fH, for buckminsterfullerene is 2320 kJ/mol at 298.2 K. a. Calculate rH for the conversion of C60 to diamond at standard state conditions and 2982 K. b. Assuming that the standard entropy per mole of carbon in both C60 and diamond is comparable (both about 23 J/K mol), is the conversion of C60 to diamond product-favoredat room temperature?
Explain why absolute entropies can be measured.
Use data from Appendix D to calculate the standardentropy change at 25°C for the reaction CH3COOH(g)+NH3(g)CH3NH2(g)+CO2(g)+H2(g) Suppose that 1.00 mol each of solid acetamide, CH3CONH2(s), and water, H2O(l), react to give thesame products. Will the standard entropy change belarger or smaller than that calculated for the reactionin part (a)?
Appendix J lists standard molar entropies S, not standard entropies of formation rS. Why is this possible forentropy but not for internal energy, enthalpy, or Gibbsfree energy?
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)