Concept explainers
(a)
Interpretation: It should be predicted that whether the given process is reversible or not.
Concept introduction: Reversible process are those process in which it is possible to return to the initial point, by the same path along which the change is carried out.
For a reversible process, the system should remain in equilibrium. However, spontaneous process involve non-equilibrium constants and are therefore irreversible.
For an irreversible process, the system can be brought to the initial point but there occurs a change in the surroundings.
(b)
Interpretation: It should be predicted that wheter the given process is reversible or not.
Concept introduction: Reversible process are those process in which it is possible to return to the initial point, by the same path along which the change is carried out.
For a reversible process, the system should remain in equilibrium. However, spontaneous process involves non-equilibrium constants and is therefore irreversible.
For an irreversible process, the system can be brought to the initial point but there occurs a change in the surroundings.
(c)
Interpretation: It should be predicted that wheter the given process is reversible or not.
Concept introduction: Reversible process are those process in which it is possible to return to the initial point, by the same path along which the change is carried out.
For a reversible process, the system should remain in equilibrium. However, spontaneous process involves non-equilibrium constants and is therefore irreversible.
For an irreversible process, the system can be brought to the initial point but there occurs a change in the surroundings.
(d)
Interpretation: It should be predicted that wheter the given process is reversible or not.
Concept introduction: Reversible process are those process in which it is possible to return to the initial point, by the same path along which the change is carried out.
For a reversible process, the system should remain in equilibrium. However, spontaneous process involves non-equilibrium constants and is therefore irreversible.
For an irreversible process, the system can be brought to the initial point but there occurs a change in the surroundings.
Want to see the full answer?
Check out a sample textbook solutionChapter 18 Solutions
Chemistry & Chemical Reactivity
- The formation of aluminum oxide from its elements is highly exothermic. If 2.70 g Al metal is burned in pure O2 to give A12O3, calculate how much thermal energy is evolved in the process (at constant pressure).arrow_forwardFrom data in Appendix J, estimate (a) the boiling point of titanium(IV) chloride. (b) the boiling point of carbon disulfide, CS2, which is a liquid at 25 C and 1 bar.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
- 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)arrow_forwardWhat determines Ssurr for a process? To calculate Ssurr at constant pressure and temperature, we use the following equation: Ssurr = H/T. Why does a minus sign appear in the equation, and why is Ssurr inversely proportional to temperature?arrow_forwardCalculate H when a 38-g sample of glucose, C6H12O6(s), burns in excess O2(g) to form CO2(g) and H2O() in a reaction at constant pressure and 298.15 K.arrow_forward
- Silver carbonate, Ag2CO3, is a light yellow compound that decomposes when heated to give silver oxide and carbon dioxide: Ag2CO3(s)Ag2O(s)+CO2(g) A researcher measured the partial pressure of carbon dioxide over a sample of silver carbonate at 220C and found that it was 1.37 atm. Calculate the partial pressure of carbon dioxide at 25C. The standard enthalpies of formation of silver carbonate and silver oxide at 25C are 505.9 kJ/mol and 31.05 kJ/mol, respectively. Make any reasonable assumptions in your calculations. State the assumptions that you make, and note why you think they are reasonable.arrow_forwardReword the statement in Question 109 so that it is always true. Criticize this statement: Provided it occurs at an appreciable rate, any chemical reaction for which rG 0 will proceed until all reactants have been converted toproducts.arrow_forwardWhat 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_forward
- For a liquid, which would you expect to be larger, Sfusion or Sevaporation? Why?arrow_forwardWhat 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)arrow_forwardWhy is it usually easier to use G to determine the spontaneity of a process rather than Su ?arrow_forward
- Chemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry for Today: General, Organic, and Bioche...ChemistryISBN:9781305960060Author:Spencer L. Seager, Michael R. Slabaugh, Maren S. HansenPublisher:Cengage Learning
- General 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 LearningChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning