5) Of the following, the entropy of gaseousis the largest at 25 °C and 1 atm.A) C2H2B) H₂C) C2H6D) CH4E) C2H2Use the table below to answer the questions that follow.Thermodynamic Quantities for Selected Substances at 298.15 K (25°C)SubstanceAH (kJ/mol) AGO (kJ/mol) S (J/K-mol)CarbonC (s, diamond)1.882.842.43C (s, graphite)05.69C2H2 (g)226.7209.2200.8C2H4 (g)52.3068.11219.4C2H6 (g)-84.68-32.89229.5CO (g)-110.5-137.2197.9CO2 (g)-393.5-394.4213.6HydrogenH2(g)00130.58OxygenO2 (g)00205.0H₂O (1)-285.83-237.1369.91

Step 1:Entropy is a measure of system's disorderliness or randomness. In more microstates system can…

Answered: 5) Of the following, the entropy of…

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 10.73PAE

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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.)
What is entropy? Why is entropy important?
Which contains greater entropy, a quantity of frozen benzene or the same quantity of liquid benzene at the same temperature? Explain in terms of the dispersal of energy in the substance.
10.45 Calculate G at 45°C for reactions for which (a) H = 293 kJ; S= -695 J/K (b) H= -1137 kJ; S = 0.496 kJ/K (c) H = -86.6 kJ; S = -382 J/K
Through photosynthesis, plants build molecules of sugar containing several carbon atoms from carbon dioxide. In the process, entropy is decreased. The reaction of CO2with formic acid to form oxalic acid provides a simple example of a reaction in which the number of carbon atoms in a compound increases: CO2(aq)+HCOOH(aq)H2C2O4(aq) (a) Calculate the standard entropy change for this reaction and discuss the sign of S . (b) How do plants carry out reactions that increase the number of carbon atoms in a sugar, given the changes in entropy for reactions like this?
For the reaction at 298 K, 2NO2(g)N2O4(g) the values of H and S are 58.03 kJ and 176.6 J/K, respectively. What is the value of G at 298 K? Assuming that H and S do not depend on temperature, at what temperature is G = 0? Is G negative above or below this temperature?
Without doing a calculation, predict whether the entropy change will be positive or negative when each of the following reactions occurs in the direction it is written. (a) CH3OH(l)+3/2O2(g)CO2(g)+2H2O(g) (b) Br2(l)+H2(g)2HBr(g) (c) Na(s)+l/2F2(g)NaF(s) (d)CO(g)+2H2(g)CH3OH(l) (e) 2NH3(g)N2(g)+3H2(g)
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.
Consider the reaction of 2 mol H2(g) at 25C and 1 atm with 1 mol O2(g) at the same temperature and pressure to produce liquid water at these conditions. If this reaction is run in a controlled way to generate work, what is the maximum useful work that can be obtained? How much entropy is produced in this case?
What happens to the entropy of the universe during a spontaneous process?
What is the third law of thermodynamics? What are standard entropy values, S, and how are these S values (listed in Appendix 4) used to calculate S for a reaction? How would you use Hesss law to calculate S for a reaction? What does the superscript indicate? Predicting the sign of S for a reaction is an important skill to master. For a gas-phase reaction, what do you concentrate on to predict the sign of S? For a phase change, what do you concentrate on to predict the sign of S? That is, how are Ssolid, Sliquid, and Sgas related to one another? When a solute dissolves in water, what is usually the sign of S for this process?
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.

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