Thermodynamic Quantities for Selected Substances at 298.15 K (25 °C) Substance AH°f (kJ/mol) AG°f (kJ/mol) S(K-mol) Calcum Ca (s) CaCl2 (s) 41.4 -795.8 -748.1 104.6 Caz* (aq) 226.7 209.2 200.8 Chlorine Cl2 (8) 222.96 Cl- (aq) -167.2 -131.2 56.5 Oxygen 02 (8) 205.0 H20 (1) -285.83 -237.13 69.91 Phosphorus P2 (g) PC13 (g) POC13 (g) 144.3 103.7 218.1 -288.1 -269.6 311.7 -542.2 -502.5 325 Sulfur 31.88 S (s, rhombic) -269.9 -300.4 248.5 90 3(g) -395.2 -370.4 256.2 The value of A G° at 25 °C for the decomposition of phosphorous trichloride into its constituent elements as shown. 2PCI3(g) --> P2(g) + 3CI2(g) is kJ/mol. A. -539.2 B. +539.2 C. -642.9 D. +642.9 O E. -373.3

Thermodynamic Quantities for Selected Substances at 298.15 K (25 °C) Substance AH°f (kJ/mol) AG°f (kJ/mol) S(K-mol) Calcum Ca (s) CaCl2 (s) 41.4 -795.8 -748.1 104.6 Caz* (aq) 226.7 209.2 200.8 Chlorine Cl2 (8) 222.96 Cl- (aq) -167.2 -131.2 56.5 Oxygen 02 (8) 205.0 H20 (1) -285.83 -237.13 69.91 Phosphorus P2 (g) PC13 (g) POC13 (g) 144.3 103.7 218.1 -288.1 -269.6 311.7 -542.2 -502.5 325 Sulfur 31.88 S (s, rhombic) -269.9 -300.4 248.5 90 3(g) -395.2 -370.4 256.2 The value of A G° at 25 °C for the decomposition of phosphorous trichloride into its constituent elements as shown. 2PCI3(g) --> P2(g) + 3CI2(g) is kJ/mol. A. -539.2 B. +539.2 C. -642.9 D. +642.9 O E. -373.3

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter10: Entropy And The Second Law Of Thermodynamics

Section: Chapter Questions

Problem 10.8PAE: In the thermodynamic definition of a spontaneous process, why is it important that the phrase...

See similar textbooks

Similar questions

Explain why absolute entropies can be measured.
In the thermodynamic definition of a spontaneous process, why is it important that the phrase “continuous intervention” be used rather than just “intervention?”
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)
The synthesis of glucose directly from CO2 and H2O and the synthesis of proteins directly from amino acids are both non-spontaneous processes under standard conditions. Yet it is necessary for these to occur for life to exist. In light of the second law of thermodynamics, how can life exist?
Liquid water at 25C is introduced into an evacuated, insulated vessel. Identify the signs of the following thermodynamic functions for the process that occurs: H, S, Twater, Ssurr,, Suniv.
In a spontaneous process, S(universe) is (a) 0 (b) = 0 (c) 0
The evaporation of one mole of water at 298 K has a standard free allergy change of 8.58 kJ. H2O(l)H2O(g)G298=8.58kJ (a) Is the evaporation of water under standard thermodynamic conditions spontaneous?. (b) Determine the equilibrium constant, KP, for this physical process. (c) By calculating G, determine if the evaporation of water at 298 K is spontaneous when the partial pressure of water, PH2O, is 0.011 atm.. (d) If the evaporation of water were always nonspontaneous at room temperature, wet laundry would never dry when placed outside. In order for laundry to dry, what must be the value of PH2O in the air?
Calculate the entropy change for the vaporization of liquid methane and liquid hexane using the following data. Boilling point (1atm) Hvap Methane 112K 8.20 KJ/mol Hexane 342K 28.9 KJ/mol Compare the molar volume of gaseous methane at 112 K with that of gaseous hexane at 342 K. How do the differences in molar volume affect the values of Svap for these liquids?
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?
For ammonia (NH3), the enthalpy of fusion is 5.65 kJ/mol and the entropy of fusion is 28.9 J/K mol. a. Will NH3(s) spontaneously melt at 200. K? b. What is the approximate melting point of ammonia?