a) Calculate the entropy of this gas at its boiling temperature of T₁=27.1 K under 1.00 atmosphere of pressure. There are 10 protons and 10 neutrons in the nucleus of a neon atom. mp=1.67x10-27 kg, h=1.05 x10-34 J-s . b) Use the result of part a) to determine the latent heat of vaporization L of neon. Ignore the entropy of neon in the liquid phase (S₁20). c) Starting from the (Clasius-Clapeyron) equation given below, find the boiling temperature T10 of neon under a pressure of 10.0 atm. You may assume the latent heat to be constant. If the experimentally measured boiling temperature at the higher pressure is 37.6 K, how much is the relative error in your answer? R=8.31 J/(mol*K).

a) Calculate the entropy of this gas at its boiling temperature of T₁=27.1 K under 1.00 atmosphere of pressure. There are 10 protons and 10 neutrons in the nucleus of a neon atom. mp=1.67x10-27 kg, h=1.05 x10-34 J-s . b) Use the result of part a) to determine the latent heat of vaporization L of neon. Ignore the entropy of neon in the liquid phase (S₁20). c) Starting from the (Clasius-Clapeyron) equation given below, find the boiling temperature T10 of neon under a pressure of 10.0 atm. You may assume the latent heat to be constant. If the experimentally measured boiling temperature at the higher pressure is 37.6 K, how much is the relative error in your answer? R=8.31 J/(mol*K).

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter16: Thermodynamics: Directionality Of Chemical Reactions

Section16.3: Measuring Dispersal Of Energy: Entropy

Problem 16.3CE

See similar textbooks

Similar questions

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)
Use data from Appendix D to calculate the standardentropy change at 25°C for the reaction CH3COOH(g)+NH3(g)CH3NH2(g)+CO2(g)+H2(g) Suppose that 1.00 mol each of solid acetamide, CH3CONH2(s), and water, H2O(l), react to give thesame products. Will the standard entropy change belarger or smaller than that calculated for the reactionin part (a)?
For the process A(l) A(g), which direction is favored by changes in energy probability? Positional probability? Explain your answers. If you wanted to favor the process as written, would you raise or lower the temperature of the system? Explain.
Consider planet Earth as a thermodynamic system. Is Earth thermodynamically or kinetically stable? Discuss your choice, providing as many arguments as you can tosupport it.
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?
Define the term entropy, and give an example of a sample of matter that has zero entropy. What are the units of entropy? How do they differ from the units of enthalpy?
Billions of pounds of acetic acid are made each year, much of it by the reaction of methanol with carbon monoxide. (AssumeT= 298 K.) CH3OH() + CO(g) CH3COOH() (a) By calculating the standard Gibbs free energy change, rG, for this reaction, show that it is product-favored. (b) Determine the standard Gibbs free energy change, rG,for the reaction of acetic acid with oxygen to form gaseous carbon dioxide and liquid water. (c) Based on this result, is acetic acid thermodynamicallystable compared with CO2(g) and H2O()? (d) Is acetic acid kinetically stable compared with CO2(g)and H2O()?
a Calculate K1, at 25C for sulfurous acid: H2SO3(aq)H+(aq)+HSO3(aq) b Which thermodynamic factor is the most significant in accounting for the fact that sulfurous acid is a weak acid? Why?
Indicate whether each statement is true or false. (a) Thethird law of thermodynamics says that the entropy of aperfect, pure crystal at absolute zero increases with themass of the crystal. (b) “Translational motion” of moleculesrefers to their change in spatial location as a functionof time. (c) “Rotational” and “vibrational” motionscontribute to the entropy in atomic gases like He and Xe.(d) The larger the number of atoms in a molecule, themore degrees of freedom of rotational and vibrationalmotion it likely has.
Two moles of liquid water at 25 ° C is placed in a freezer having a temperature of – 10 ° C. Calculate the change in entropy.Cp,m for liquid water = 75.3 J K-1 mol-1Cp,m for ice = 37.7 J K-1 mol-1For water, ΔΗfusion = 6.01 kJmol-1
Three moles of an ideal gas at 500 K expand quasi-statically and isothermally from an initial volume of 20 L to a final volume 50 L. (a) What is the entropy change of the gas? (b) What is the entropy change of the universe for this process?
Gibbs free energy (G) is a measure of the spontaneity of a chemical reaction. It is the chemical potential for a reaction, and is minimized at equilibrium. It is defined as G=H-TS where H is enthalpy, T is temperature, and S is entropy. The chemical reaction that causes iron to corrode in air is given by 4Fe +302-2Fe2O3 in which at 298 K, AH = - 1684 kJ and ASixn - 543.7 J/K. = Part C At what temperature Teq do the forward and reverse corrosion reactions occur in equilibrium? Express your answer as an integer and include the appropriate units. ► View Available Hint(s) Teq = Submit 14 μÅ Value Units ?