The chemical potentials of two phases, a and ß, of a pure substance areshown as a function of pressure at constant temperature.A) Which phase is the more stable at high pressure?_B) Will transformation B→a occur as the pressure is raised? Yes/ No_C) On graph, mark point(s) at which these phases are in equilibriumD) Substance in which phase has higher molar volume, a or B?_HaWhat is equal to zero at 298 K?A) A:H (F, g)C) S° (F2, g)D) A;H° (F2, g)B) S° (F, g)

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Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter17: Equilibrium

Section: Chapter Questions

Problem 13ALQ

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Two phases "a" and "b" of a pure substance are in equilibrium at some temperature and pressure. Which must be true? A)Molar enthalpies of both phases are equal. B)Chemical potentials of both phases are equal C) Molar entropies of both phases are equal D) Volumesof both phases are equal
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The chemical potentials of two phases, alpha and beta, of a pure substance are shown as a function of pressure at constant temperature. A) Which phase is the more stable at high pressure? _______ B) Will transformation beta -> alpha occur as the pressure is raised? Yes/ No____ C) On graph, mark point(s) at which these phases are in equilibrium D) Substance in which phase has higher molar volume,  or ?_______
A metal salt with the formula MCl2MCl2 crystallizes from water to form a solid with the composition MCl2⋅6H2OMCl2⋅6H2O. The equilibrium vapor pressure of water above this solid at 298 KK is 17.5 mbarmbar . What is the value of ΔrG∘Δr�∘? Express your answer with the appropriate units.
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Vacancies and Self-Interstitials 1. For some hypothetical metal the equilibrium number of vacancies at 750°C is 2.8×1024?−3. If the density and atomic weight of this metal are 5.60 ? ??3⁄ and 65.6 ?/???, respectively, calculate the fraction of vacancies for this metal at 750°C.
Estimate whether theentropy of the system increases or decreases during eachprocess: (a) photodissociation of O2(g), (b) formation ofozone from oxygen molecules and oxygen atoms, (c) diffusionof CFCs into the stratosphere, (d) desalination ofwater by reverse osmosis.
What are the chemical potentials of Au and Ag at 500°C? Express you’re answer in eV per atom. 15 g of gold (Au) and 25 g of silver (Ag) are mixed to form a single-phase ideal solid solution. By how much will the free energy of the solution change at 500°C if one Au atom is added? Express your answer in eV per atom. Hint: You will need to find the specific heats of Au and Ag as functions of temperature to fix the free energies of the pure phases. In doing so, please pay attention to the units and cite the reference you pick the data from.
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The phase diagram for the nearly ideal mixture of benzene and toluene is shown below. Consider a mixture with a mole fraction of 0.6 in toluene A. What phase(s) will be present if this mixture is kept at a pressure of 35 kPa? B. What phase(s) will be present if this mixture is kept at a pressure of 18 kPa? C. What phase(s) will be present if this mixture is kept at a pressure of 10 kPa?
1.Thermodynamics of polymerization determines the position of the equilibrium between polymer and monomer(s). What is the impact of thermodynamic in polymers? Give examples to support your answer. 2.Explain the significance of Gibbs energy in thermodynamics of polymerization. Show the equations to support your answer.
A student determines the molar mass of a liquid unknown by the method used in thisexperiment. She found that the equilibrium temperature of a mixture of ice and water was1.0°C on her thermometer. When she added 12.3 g of her unknown sample to the mixture, thetemperature, after thorough stirring, fell to -4.0°C. She then poured off the solution through ascreen into a beaker. The mass of the solution was 93.4 g. Kf = 1.86°C/m What was the molality of the unknown solution? ______________ m How much unknown liquid was in the decanted solution? ______________ gHow much water was in the decanted solution? ______________ gWhat did she find to be the molar mass of the unknown liquid, assuming she made thecalculation properly?______________ g

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