Equation of State for Benzene for Temperatures from the Melting Line up to 725 K with Pressures up to 500 Mpa†
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Geometrical Vortex Lattice Pinning and Melting in Ybacuo Submicron Bridges Received: 10 August 2016 G
www.nature.com/scientificreports OPEN Geometrical vortex lattice pinning and melting in YBaCuO submicron bridges Received: 10 August 2016 G. P. Papari1,*, A. Glatz2,3,*, F. Carillo4, D. Stornaiuolo1,5, D. Massarotti5,6, V. Rouco1, Accepted: 11 November 2016 L. Longobardi6,7, F. Beltram2, V. M. Vinokur2 & F. Tafuri5,6 Published: 23 December 2016 Since the discovery of high-temperature superconductors (HTSs), most efforts of researchers have been focused on the fabrication of superconducting devices capable of immobilizing vortices, hence of operating at enhanced temperatures and magnetic fields. Recent findings that geometric restrictions may induce self-arresting hypervortices recovering the dissipation-free state at high fields and temperatures made superconducting strips a mainstream of superconductivity studies. Here we report on the geometrical melting of the vortex lattice in a wide YBCO submicron bridge preceded by magnetoresistance (MR) oscillations fingerprinting the underlying regular vortex structure. Combined magnetoresistance measurements and numerical simulations unambiguously relate the resistance oscillations to the penetration of vortex rows with intermediate geometrical pinning and uncover the details of geometrical melting. Our findings offer a reliable and reproducible pathway for controlling vortices in geometrically restricted nanodevices and introduce a novel technique of geometrical spectroscopy, inferring detailed information of the structure of the vortex system through a combined use of MR curves and large-scale simulations. Superconductors are materials in which below the superconducting transition temperature, Tc, electrons form so-called Cooper pairs, which are bosons, hence occupying the same lowest quantum state1. The wave function of this Cooper condensate has a fixed phase. Hence, by virtue of the uncertainty principle, the number of Cooper pairs in the condensate is undefined. -
Determination of the Identity of an Unknown Liquid Group # My Name the Date My Period Partner #1 Name Partner #2 Name
Determination of the Identity of an unknown liquid Group # My Name The date My period Partner #1 name Partner #2 name Purpose: The purpose of this lab is to determine the identity of an unknown liquid by measuring its density, melting point, boiling point, and solubility in both water and alcohol, and then comparing the results to the values for known substances. Procedure: 1) Density determination Obtain a 10mL sample of the unknown liquid using a graduated cylinder Determine the mass of the 10mL sample Save the sample for further use 2) Melting point determination Set up an ice bath using a 600mL beaker Obtain a ~5mL sample of the unknown liquid in a clean dry test tube Place a thermometer in the test tube with the sample Place the test tube in the ice water bath Watch for signs of crystallization, noting the temperature of the sample when it occurs Save the sample for further use 3) Boiling point determination Set up a hot water bath using a 250mL beaker Begin heating the water in the beaker Obtain a ~10mL sample of the unknown in a clean, dry test tube Add a boiling stone to the test tube with the unknown Open the computer interface software, using a graph and digit display Place the temperature sensor in the test tube so it is in the unknown liquid Record the temperature of the sample in the test tube using the computer interface Watch for signs of boiling, noting the temperature of the unknown Dispose of the sample in the assigned waste container 4) Solubility determination Obtain two small (~1mL) samples of the unknown in two small test tubes Add an equal amount of deionized into one of the samples Add an equal amount of ethanol into the other Mix both samples thoroughly Compare the samples for solubility Dispose of the samples in the assigned waste container Observations: The unknown is a clear, colorless liquid. -
Two-Dimensional Vortex Lattice Melting Superconducting Length
Two-Dimensional Vortex Lattice Melting Superconducting Length-Scales and Vortex Lattices Flux Motion Melting Concepts Journal Paper Presentation: “Melting of the Vortex Lattice Through the Hexatic Phase in an MoGe3 Thin Film” 1 Repulsive Interaction Between Vortices Vortex Lattice 2 Vortex Melting in Superconducting Nb 3 (For 3D clean Type II superconductor) Vortex Lattice Expands on Freezing (Like Ice) Jump in the Magnetization 4 Melting Concepts 3D Solid Liquid Lindemann Criterion (∆r)2 ↵a 1st Order Transition ⇡ p 5 6 Journal Presentation Motivation/Context Results Interpretation Questions/Ideas for Future Work (aim for 30-45 mins) Please check the course site about the presentation schedule No class on The April 8, 15 Make-Ups on Ms April 12, 19 (Weekly Discussion to be Rescheduled) 7 First Definitive Observation of the Hexatic Phase in a Superconducting Film (with 8 thanks to Indranil Roy and Pratap Raychaudhuri) Two Dimensional Melting (BKT + HNY theory) 9 10 Hexatics have been observed in 2D colloidal systems Why not in the Melting of the Vortex Phase of Superconducting Films ?? 11 Quest for the Hexatic Liquid Phase in ↵ MoGe − Why Not Before ?? Orientational Coupling Hexatic Glass !! between Atomic and Vortex Lattices Solution: Amorphous Superconductor (no lattice effect) Very Weak Pinning BCS-Type Superconductor 12 Scanning Tunneling Spectroscopy (STS) Magnetotransport 13 14 15 16 17 The Resulting Phase Diagram 18 Summary First Observation of Hexatic Fluid Phase in a 2D Superconducting Film Pinning Significantly Weaker than in Previous Studies STS (imaging) Magnetotransport (“shear”) Questions/Ideas for the Future Size-Dependence of Hexatic Order Parameter ?? Low T limit of the Hexatic Fluid: Quantum Vortex Fluid ?? What happens in Layered Films ?? 19 20. -
The Basics of Vapor-Liquid Equilibrium (Or Why the Tripoli L2 Tech Question #30 Is Wrong)
The Basics of Vapor-Liquid Equilibrium (Or why the Tripoli L2 tech question #30 is wrong) A question on the Tripoli L2 exam has the wrong answer? Yes, it does. What is this errant question? 30.Above what temperature does pressurized nitrous oxide change to a gas? a. 97°F b. 75°F c. 37°F The correct answer is: d. all of the above. The answer that is considered correct, however, is: a. 97ºF. This is the critical temperature above which N2O is neither a gas nor a liquid; it is a supercritical fluid. To understand what this means and why the correct answer is “all of the above” you have to know a little about the behavior of liquids and gases. Most people know that water boils at 212ºF. Most people also know that when you’re, for instance, boiling an egg in the mountains, you have to boil it longer to fully cook it. The reason for this has to do with the vapor pressure of water. Every liquid wants to vaporize to some extent. The measure of this tendency is known as the vapor pressure and varies as a function of temperature. When the vapor pressure of a liquid reaches the pressure above it, it boils. Until then, it evaporates until the fraction of vapor in the mixture above it is equal to the ratio of the vapor pressure to the total pressure. At that point it is said to be in equilibrium and no further liquid will evaporate. The vapor pressure of water at 212ºF is 14.696 psi – the atmospheric pressure at sea level. -
Liquid-Vapor Equilibrium in a Binary System
Liquid-Vapor Equilibria in Binary Systems1 Purpose The purpose of this experiment is to study a binary liquid-vapor equilibrium of chloroform and acetone. Measurements of liquid and vapor compositions will be made by refractometry. The data will be treated according to equilibrium thermodynamic considerations, which are developed in the theory section. Theory Consider a liquid-gas equilibrium involving more than one species. By definition, an ideal solution is one in which the vapor pressure of a particular component is proportional to the mole fraction of that component in the liquid phase over the entire range of mole fractions. Note that no distinction is made between solute and solvent. The proportionality constant is the vapor pressure of the pure material. Empirically it has been found that in very dilute solutions the vapor pressure of solvent (major component) is proportional to the mole fraction X of the solvent. The proportionality constant is the vapor pressure, po, of the pure solvent. This rule is called Raoult's law: o (1) psolvent = p solvent Xsolvent for Xsolvent = 1 For a truly ideal solution, this law should apply over the entire range of compositions. However, as Xsolvent decreases, a point will generally be reached where the vapor pressure no longer follows the ideal relationship. Similarly, if we consider the solute in an ideal solution, then Eq.(1) should be valid. Experimentally, it is generally found that for dilute real solutions the following relationship is obeyed: psolute=K Xsolute for Xsolute<< 1 (2) where K is a constant but not equal to the vapor pressure of pure solute. -
Pressure Vs Temperature (Boiling Point)
Boiling Points and Vapor Pressure Background Boiling Points and Vapor Pressure Background: Definitions Vapor Pressure: The equilibrium pressure of a vapor above its liquid; the pressure of the vapor resulting from the evaporation of a liquid above a sample of the liquid in a closed container. Boiling Point: The temperature at which the vapor pressure of a liquid is equal to the atmospheric (or applied) pressure. As the temperature of the liquid increases, the vapor pressure will increase, as seen below: https://www.chem.purdue.edu/gchelp/liquids/vpress.html Vapor pressure is interpreted in terms of molecules of liquid converting to the gaseous phase and escaping into the empty space above the liquid. In order for the molecules to escape, the intermolecular forces (Van der Waals, dipole- dipole, and hydrogen bonding) have to be overcome, which requires energy. This energy can come in the form of heat, aka increase in temperature. Due to this relationship between vapor pressure and temperature, the boiling point of a liquid decreases as the atmospheric pressure decreases since there is more room above the liquid for molecules to escape into at lower pressure. The graph below illustrates this relationship using common solvents and some terpenes: Pressure vs Temperature (boiling point) Ethanol Heptane Isopropyl Alcohol B-myrcene 290.0 B-caryophyllene d-Limonene Linalool Pulegone 270.0 250.0 1,8-cineole (eucalyptol) a-pinene a-terpineol terpineol-4-ol 230.0 p-cymene 210.0 190.0 170.0 150.0 130.0 110.0 90.0 Temperature (˚C) Temperature 70.0 50.0 30.0 10 20 30 40 50 60 70 80 90 100 200 300 400 500 600 760 10.0 -10.0 -30.0 Pressure (torr) 1 Boiling Points and Vapor Pressure Background As a very general rule of thumb, the boiling point of many liquids will drop about 0.5˚C for a 10mmHg decrease in pressure when operating in the region of 760 mmHg (atmospheric pressure). -
Sodium Spinor Bose-Einstein Condensates
SODIUM SPINOR BOSE-EINSTEIN CONDENSATES: ALL-OPTICAL PRODUCTION AND SPIN DYNAMICS By JIEJIANG BachelorofScienceinOpticalInformationScience UniversityofShanghaiforScienceandTechnology Shanghai,China 2009 SubmittedtotheFacultyofthe GraduateCollegeof OklahomaStateUniversity inpartialfulfillmentof therequirementsfor theDegreeof DOCTOROFPHILOSOPHY December,2015 COPYRIGHT c By JIE JIANG December, 2015 SODIUM SPINOR BOSE-EINSTEIN CONDENSATES: ALL-OPTICAL PRODUCTION AND SPIN DYNAMICS Dissertation Approved: Dr. Yingmei Liu Dissertation Advisor Dr. Albert T. Rosenberger Dr. Gil Summy Dr. Weili Zhang iii ACKNOWLEDGMENTS I would like to first express my sincere gratitude to my thesis advisor Dr. Yingmei Liu, who introduced ultracold quantum gases to me and guided me throughout my PhD study. I am greatly impressed by her profound knowledge, persistent enthusiasm and love in BEC research. It has been a truly rewarding and privilege experience to perform my PhD study under her guidance. I also want to thank my committee members, Dr. Albert Rosenberger, Dr. Gil Summy, and Dr. Weili Zhang for their advice and support during my PhD study. I thank Dr. Rosenberger for the knowledge in lasers and laser spectroscopy I learnt from him. I thank Dr. Summy for his support in the department and the academic exchange with his lab. Dr. Zhang offered me a unique opportunity to perform microfabrication in a cleanroom, which greatly extended my research experience. During my more than six years study at OSU, I had opportunities to work with many wonderful people and the team members in Liu’s lab have been providing endless help for me which is important to my work. Many thanks extend to my current colleagues Lichao Zhao, Tao Tang, Zihe Chen, and Micah Webb as well as our former members Zongkai Tian, Jared Austin, and Alex Behlen. -
Melting of Lamellar Phases in Temperature Sensitive Colloid-Polymer Suspensions
PHYSICAL REVIEW LETTERS week ending VOLUME 93, NUMBER 5 30 JULY 2004 Melting of Lamellar Phases in Temperature Sensitive Colloid-Polymer Suspensions A. M. Alsayed, Z. Dogic, and A. G. Yodh Department of Physics and Astronomy, University of Pennsylvania, Philadelphia, Pennsylvania 19104-6396, USA (Received 10 March 2004; published 29 July 2004) We prepare a novel suspension composed of rodlike fd virus and thermosensitive polymer poly(N-isopropylacrylamide) whose phase diagram is temperature and concentration dependent. The system exhibits a rich variety of stable and metastable phases, and provides a unique opportunity to directly observe melting of lamellar phases and single lamellae. Typically, lamellar phases swell with increasing temperature before melting into the nematic phase. The highly swollen lamellae can be superheated as a result of topological nucleation barriers that slow the formation of the nematic phase. DOI: 10.1103/PhysRevLett.93.057801 PACS numbers: 64.70.Md, 61.30.–v, 64.60.My Melting of three-dimensional (3D) crystals is among lamellar phases and coexisting isotropic or nematic the most ubiquitous phase transitions in nature [1]. In phases. contrast to freezing, melting of 3D crystals usually has The fd=NIPA solutions are unusual new materials no associated energy barrier. Bulk melting is initiated at a whose lamellar phases differ from those of amphiphilic premelted surface, which then acts as a heterogeneous molecules. The lamellar phase can swell considerably and nucleation site and eliminates the nucleation barrier for melt into a nematic phase, a transition almost never the phase transition [2]. In this Letter, we investigate observed in block-copolymer lamellar systems. -
Freezing and Boiling Point Changes
Freezing Point and Boiling Point Changes for Solutions and Solids Lesson Plans and Labs By Ranald Bleakley Physics and Chemistry teacher Weedsport Jnr/Snr High School RET 2 Cornell Center for Materials Research Summer 2005 Freezing Point and Boiling Point Changes for Solutions and Solids Lesson Plans and Labs Summary: Major skills taught: • Predicting changes in freezing and boiling points of water, given type and quantity of solute added. • Solving word problems for changes to boiling points and freezing points of solutions based upon data supplied. • Application of theory to real samples in lab to collect and analyze data. Students will describe the importance to industry of the depression of melting points in solids such as metals and glasses. • Students will describe and discuss the evolution of glass making through the ages and its influence on social evolution. Appropriate grade and level: The following lesson plans and labs are intended for instruction of juniors or seniors enrolled in introductory chemistry and/or physics classes. It is most appropriately taught to students who have a basic understanding of the properties of matter and of solutions. Mathematical calculations are intentionally kept to a minimum in this unit and focus is placed on concepts. The overall intent of the unit is to clarify the relationship between changes to the composition of a mixture and the subsequent changes in the eutectic properties of that mixture. Theme: The lesson plans and labs contained in this unit seek to teach and illustrate the concepts associated with the eutectic of both liquid solutions, and glasses The following people have been of great assistance: Professor Louis Hand Professor of Physics. -
Methods for the Determination of the Normal Boiling Point of a High
Metalworking Fluids & VOC, Today and Tomorrow A Joint Symposium by SCAQMD & ILMA South Coast Air Quality Management District Diamond Bar, CA, USA March 8, 2012 Understanding & Determining the Normal Boiling Point of a High Boiling Liquid Presentation Outline • Relationship of Vapor Pressure to Temperature • Examples of VP/T Curves • Calculation of Airborne Vapor Concentration • Binary Systems • Relative Volatility as a function of Temperature • GC Data and Volatility • Everything Needs a Correlation • Conclusions Vapor Pressure Models (pure vapor over pure liquid) Correlative: • Clapeyron: Log(P) = A/T + B • Antoine: Log(P) = A/(T-C) + B • Riedel: LogP = A/T + B + Clog(T) + DTE Predictive: • ACD Group Additive Methods • Riedel: LogP = A/T + B + Clog(T) + DTE Coefficients defined, Reduced T = T/Tc • Variations: Frost-Kalkwarf-Thodos, etc. Two Parameters: Log(P) = A/T + B Vaporization as an CH OH(l) CH OH(g) activated process 3 3 G = -RTln(K) = -RTln(P) K = [CH3OH(g)]/[CH3OH(l)] G = H - TS [CH3OH(g)] = partial P ln(P) = -G/RT [CH3OH(l)] = 1 (pure liquid) ln(P) = -H/RT+ S/R K = P S/R = B ln(P) = ln(K) H/R = -A Vapor pressure Measurement: Direct versus Distillation • Direct vapor pressure measurement (e.g., isoteniscope) requires pure material while distillation based determination can employ a middle cut with a relatively high purity. Distillation allows for extrapolation and/or interpolation of data to approximate VP. • Direct vapor pressure measurement requires multiple freeze-thaw cycles to remove atmospheric gases while distillation (especially atmospheric distillation) purges atmospheric gases as part of the process. • Direct measurement OK for “volatile materials” (normal BP < 100 oC) but involved for “high boilers” (normal BP > 100 oC). -
Liquid Equilibrium Measurements in Binary Polar Systems
DIPLOMA THESIS VAPOR – LIQUID EQUILIBRIUM MEASUREMENTS IN BINARY POLAR SYSTEMS Supervisors: Univ. Prof. Dipl.-Ing. Dr. Anton Friedl Associate Prof. Epaminondas Voutsas Antonia Ilia Vienna 2016 Acknowledgements First of all I wish to thank Doctor Walter Wukovits for his guidance through the whole project, great assistance and valuable suggestions for my work. I have completed this thesis with his patience, persistence and encouragement. Secondly, I would like to thank Professor Anton Friedl for giving me the opportunity to work in TU Wien and collaborate with him and his group for this project. I am thankful for his trust from the beginning until the end and his support during all this period. Also, I wish to thank for his readiness to help and support Professor Epaminondas Voutsas, who gave me the opportunity to carry out this thesis in TU Wien, and his valuable suggestions and recommendations all along the experimental work and calculations. Additionally, I would like to thank everybody at the office and laboratory at TU Wien for their comprehension and selfless help for everything I needed. Furthermore, I wish to thank Mersiha Gozid and all the students of Chemical Engineering Summer School for their contribution of data, notices, questions and solutions during my experimental work. And finally, I would like to thank my family and friends for their endless support and for the inspiration and encouragement to pursue my goals and dreams. Abstract An experimental study was conducted in order to investigate the vapor – liquid equilibrium of binary mixtures of Ethanol – Butan-2-ol, Methanol – Ethanol, Methanol – Butan-2-ol, Ethanol – Water, Methanol – Water, Acetone – Ethanol and Acetone – Butan-2-ol at ambient pressure using the dynamic apparatus Labodest VLE 602. -
Physical Changes
How Matter Changes By Cindy Grigg Changes in matter happen around you every day. Some changes make matter look different. Other changes make one kind of matter become another kind of matter. When you scrunch a sheet of paper up into a ball, it is still paper. It only changed shape. You can cut a large, rectangular piece of paper into many small triangles. It changed shape and size, but it is still paper. These kinds of changes are called physical changes. Physical changes are changes in the way matter looks. Changes in size and shape, like the changes in the cut pieces of paper, are physical changes. Physical changes are changes in the size, shape, state, or appearance of matter. Another kind of physical change happens when matter changes from one state to another state. When water freezes and makes ice, it is still water. It has only changed its state of matter from a liquid to a solid. It has changed its appearance and shape, but it is still water. You can change the ice back into water by letting it melt. Matter looks different when it changes states, but it stays the same kind of matter. Solids like ice can change into liquids. Heat speeds up the moving particles in ice. The particles move apart. Heat melts ice and changes it to liquid water. Metals can be changed from a solid to a liquid state also. Metals must be heated to a high temperature to melt. Melting is changing from a solid state to a liquid state.