Chemistry The heat of vaporization AH, of dichloromethane (CH2C₁₂) is 28.0 kJ/mol. Calculate the change in entropy AS when 9.1 g of dichloromethane condenses at39.8 °C.Be sure your answer contains a unit symbol and the correct number of significant digits.☐Ox10μ5

Step 1:The relationship between heat of vaporization and condensation is ∆Hv = - ∆Hc Equal in…

Answered: The heat of vaporization AH, of…

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter18: Principles Of Chemical Reactivity: Entropy And Free Energy

Section: Chapter Questions

Problem 9PS

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Solid NH4NO3 is placed in a beaker containing water at 25 C. When the solid has completely dissolved, the temperature of the solution is 23.5 C. (a) Was the process exothermic or endothermic? (b) Was the process spontaneous? (c) Did the entropy of the system increase? (d) Did the entropy of the universe increase?
2. Which of the following is true for a spontaneous process but not for a nonspontaneous process? Energy in the universe is concentrated conserved dispersed not conserved
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?
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.
Define the following: a. spontaneous process b. entropy c. positional probability d. system e. surroundings f. universe
How is the sign of q, heat, defined? How does it relate to the total energy of the system?
What is the sign of the standard Gibbs free-energy change at low temperatures and at high temperatures for the combustion of acetaldehyde? CH3CHO(l)+52O2(g)2CO2+2H2O(l)
When 1.000 g of ethylene glycol, C2H6O2, is burned at 25C and 1.00 atmosphere pressure, H2O(l) and CO2(g) are formed with the evolution of 19.18 kJ of heat. a Calculate the molar enthalpy of formation of ethylene glycol. (It will be necessary to use data from Appendix C.) b Gf of ethylene glycol is 322.5 kJ/mol. What is G for the combustion of 1 mol ethylene glycol? c What is S for the combustion of 1 mol ethylene glycol?
What is the second law of thermodynamics? For any process, there are four possible sign combinations for Ssys and Ssurr. Which sign combination(s) always give a spontaneous process? Which sign combination(s) always give a non-spontaneous process? Which sign combination(s) may or may not give a spontaneous process?
It takes 2260 J to vaporize a gram of liquid water to steam at its normal boiling point of 100C. What is H for this process?What is the work, given that the water vaporexpands against a pressure of 0.988atm? What is U for thisprocess?
What is the sign of the work when a refrigerator compresses a gas (the system) to a liquid during the refrigeration cycle?
Enthalpy changes often help predict whether or not a process will be spontaneous. What type of reaction is more likely to be spontaneous: an exothermic or an endothermic one? Provide two examples that support your assertion and one counterexample.

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The heat of vaporization AH, of dichloromethane (CH2C₁₂) is 28.0 kJ/mol. Calculate the change in entropy AS when 9.1 g of dichloromethane condenses at 39.8 °C. Be sure your answer contains a unit symbol and the correct number of significant digits. ☐ Ox10 μ 5