All I'm given Using tabulated values of S°, calculate the standard entropy per mole of atoms for the following.Incorrect.Ar. The S° for Ar is 154.843 J/(mol*K).1.54840E2J'mol 1"K-1ieTextbook and MediaHintX Incorrect.02. The S° for 02 is 205.152 J/(mol*K).1.02570E2J*mol1•K*1iCorrect.03. The S° for 03 is 238.9 J/(mol*K).79.63J'mol 1"K1X Incorrect.C2H6. The S° for C2H6 is 229.2 J/(mol*K).iJ*mol1"K-1 X Incorrect.Explain the trend that bond formation does to atomic order by selecting those that apply.Larger molecules have higher entropies than smaller molecules.O Larger molecules have larger entropies on a per atom basis.O Larger molecules have lower entropies than smaller molecules.Larger molecules have smaller entropies on a per atom basis.

Answered: Image /qna-images/answer/d516b2a5-6131-45b5-aa41-8948499f2fdc.jpg

Using tabulated values of S°, calculate the standard entropy per mole of atoms for the following. X Incorrect. Ar. The S° for Ar is 154.843 J/(mol*K). 1.54840E2 J*mol"1•K*1 i eTextbook and Media Hint X Incorrect. 02. The S° for O2 is 205.152 J/(mol*K). 1.02570E2 J'mol 1K-1 i Correct. 03. The S° for 03 is 238.9 J/(mol*K). 79.63 J'mol 1"K-1 X Incorrect. C2H6. The S° for C2H6 is 229.2 J/(mol*K). J'mol"1"K1 i

Using tabulated values of S°, calculate the standard entropy per mole of atoms for the following. X Incorrect. Ar. The S° for Ar is 154.843 J/(molK). 1.54840E2 Jmol"1•K1 i eTextbook and Media Hint X Incorrect. 02. The S° for O2 is 205.152 J/(molK). 1.02570E2 J'mol 1K-1 i Correct. 03. The S° for 03 is 238.9 J/(molK). 79.63 J'mol 1"K-1 X Incorrect. C2H6. The S° for C2H6 is 229.2 J/(molK). J'mol"1"K1 i

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 6CO

See similar textbooks

Similar questions

10.104 (a) When a chemical bond forms, what happens to the entropy of the system? (b) Thermodynamically, what allows any bond formation to occur? (c) What do your answers to parts (a) and (b) suggest must be true about the formation of chemical bonds for the octet rule to hold?
How does the second law of thermodynamics explain a spontaneous change in a system that becomes more ordered when that process is exothermic?
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 reaction CO2(g)+H2(g)CO(g)+H2O(g) is not spontaneous at room temperature but becomes spontaneous at a much higher temperature. What can you conclude from this about the signs of H and S , assuming that the enthalpy and entropy changes are not greatly affected by the temperature change? Explain your reasoning.
Define the following: a. spontaneous process b. entropy c. positional probability d. system e. surroundings f. universe
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?
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?
For the reaction NO(g)+NO2(g)N2O3(g) , use tabulated thermodynamic data to calculate H and S. Then use those values to answer the following questions. (a) Is this reaction spontaneous at 25°C? Explain your answer. (b) If the reaction is not spontaneous at 25°C, will it become spontaneous at higher temperatures or lower temperatures? (c) To show that your prediction is accurate, choose a temperature that corresponds to your prediction in part (b) and calculate G . (Assume that both enthalpy and entropy are independent of temperature.)
For each process, tell whether the entropy change of the system is positive or negative. Water vapor (the system) deposits as ice crystals on a cold windowpane. A can of carbonated beverage loses its fizz. (Consider the beverage but not the can as the system. What happens to the entropy of the dissolved gas?) A glassblower heats glass (the system) to its softening temperature.
At 100C and 1.00 atm, H = 40.6 kJ/mol for the vaporization of water. Estimate G for the vaporization of water at 90.C and 110.C. Assume H and S at 100.C and 1.00 atm do not depend on temperature.
For each process, tell whether the entropy change of the system is positive or negative, (a) A glassblower heats glass (the system) to its softening temperature, (b) A teaspoon of sugar dissolves in a cup of coffee. (The system consists of both sugar and coffee.) (c) Calcium carbonate precipitates out of water in a cave to form stalactites and stalagmites. (Consider only the calcium carbonate to be the system.)