(a)
Interpretation:
The value of change in pressure required to get a value of
Concept introduction:
The Gibbs free energy of the system represents the maximum amount of non-expansion work achieved by a
Answer to Problem 4.60E
The value of change in pressure required to get a value of
Explanation of Solution
The number of moles of water is
The molar volume is
The required value
The change in Gibbs energy of the condensed system is represented as shown below.
Where,
•
•
Rearrange the equation (1) for the value of
Substitute the value of
Therefore, the value of change in pressure required to get a value of
The value of change in pressure required to get a value
(b)
Interpretation:
The value of change in pressure for
Concept introduction:
The Gibbs free energy of the system represents the maximum amount of non-expansion work achieved by a thermodynamic system at isothermal and isobaric conditions. The change in Gibbs free energy is used to predict the spontaneity of the process. The change in Gibbs energy of the gaseous system isrepresented as shown below.
Answer to Problem 4.60E
The value of change in pressure for
Explanation of Solution
The temperature of the ideal gas is
The temperature of the ideal gas in Kelvin is calculated as shown below.
The required value of
The number of moles of the ideal gas is
The change in Gibbs energy of the gaseous system is represented as shown below.
Where,
•
•
•
•
•
Rearrange the equation (3) for the value of
Substitute the value of
The above expression is further solved as shown below.
One is subtracted from both sides of the above expression.
When the initial pressure of an ideal gas is assumed to be
Therefore, the value of change in pressure for
The value of change in pressure for
(c)
Interpretation:
The difference between the two corresponding values of change in pressure is to be explained.
Concept introduction:
The Gibbs free energy of the system represents the maximum amount of non-expansion work achieved by a thermodynamic system at isothermal and isobaric conditions. The change in Gibbs free energy is used to predict the spontaneity of the process. The change in Gibbs energy of the gaseous system isrepresented as shown below.
Answer to Problem 4.60E
The value of change in pressure for
Explanation of Solution
The value of change in pressure for
The value of change in pressure for
The value of change in pressure for
The gases are easily compressible than a condensed phase system. A small increase in pressure is required for compression of gas and a large increase in pressure is required to compress water. Therefore, the compression of gas requires less pressure than the compression of water.
The value of change in pressure for
Want to see more full solutions like this?
Chapter 4 Solutions
Physical Chemistry
- 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)arrow_forwardHow is the sign of q, heat, defined? How does it relate to the total energy of the system?arrow_forwardCalculate 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?)arrow_forward
- 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.arrow_forwardSolid 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?arrow_forwardUse the data in Appendix G to calculate the standard entropy change for H2(g) + CuO(s) H2O() + Cu(s)arrow_forward
- There are millions of organic compounds known, and new ones are being discovered or made at a rate of morethan 100,000 compounds per year. Organic compoundsburn readily in air at high temperatures to form carbondioxide and water. Several classes of organic compoundsare listed, with a simple example of each. Write a balanced chemical equation for the combustion in O2ofeach of these compounds, and then use the data inAppendix J to show that each reaction is product-favoredat room temperature. From these results, it is reasonable to hypothesize thatallorganic compounds are thermodynamically unstable inan oxygen atmosphere (that is, their room-temperaturereaction with O2(g) to form CO2(g) and H2O() isproduct-favored). If this hypothesis is true, how canorganic compounds exist on Earth?arrow_forwardIndicate whether the following processes are spontaneous or nonspontaneous. (a) Liquid water freezing at a temperature below its freezing point (b) Liquid water freezing at a temperature above its freezing point (c) The combustion of gasoline (d) A ball thrown into the air (e) A raindrop falling to the ground (f) Iron rusting in a moist atmospherearrow_forward
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningGeneral Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningChemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStaxChemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning