Amazon versus Webvan

Amazon versus Webvan AbstractBoth Amazon and Webvan were well-funded Internet startups in the 1990's. Both focused on a business model that allowed consumers to order products online that would be delivered to the consumers home. In the article, we discuss why Amazon succeeded while Webvan failed.The Two Companies' BackgroundAmazon: Amazon.com, Inc. Amazon.com, Inc. is a Website where customers can find and discover anything they may want to buy online. Jeff Bezos founded Amazon .com in 1990and in July 1995, Amazon.com, Inc. the Fortune 500 Company commenced its operations becoming one of the world most customer-centric company, and selling Worlds Biggest Selection. They offer their customers the lowest possible prices and highest quality. They sell millions of unique, new, used and collectible items in categories such as apparel and accessories, electronics, computers, kitchen and house wares, books, music, DVDs, videos, cameras and photo items, office products, toys, baby items and baby registry, softw are, computer and video games, cell phones and service, tools and hardware, travel services, magazine subscriptions and outdoor living items.Webvan Delivery VanThe Company organized its operations into four principal segments. 1. North America Books, Music and DVD/Video (BMVD); 2. North America Electronics, Tools and Kitchen (ETK); 3. International, 4. ServicesWebvan: Webvan was started in 1996 by Louis Borders and was established to sell groceries over the World Wide Web. George Shaheen resigned as CEO of Anderson Consulting to take advantage of the opportunity to become CEO of Webvan. Webvan, which originated as an online grocery service, delivers food (including its BestYet label, a co-brand with food distributor Fleming Companies) and non-prescription drugs to their customers' doors. Webvan's vision was to provide grocery-shopping solutions that would save consumers both time and effort, without sacrificing the quality, selection, and low prices of traditional brick-and-mortar s tores.Why Amazon...

How to Use French Punctuation

How to Use French Punctuation Although French and English use nearly all of the same punctuation marks, some of their uses in the two languages are considerably different. Rather than an explanation of the rules of French and English punctuation, this lesson is a simple summary of how French punctuation differs from English. One-Part Punctuation Marks These are very similar in French and English, with a few exceptions. Period or Le Point . In French, the period is not used after abbreviations of measurement:  25 m (mà ¨tres), 12 min (minutes), etc.It can be used to separate the elements of a date:  10 septembre 1973 10.9.1973.When writing numbers, either a period or a space may be used to separate every three digits (where a comma would be used in English):  1,000,000 (English) 1.000.000 or 1 000 000.Its not used to indicate a decimal point (see virgule 1). Commas , In French, the comma is used as a decimal point:  2.5 (English) 2,5 (French).Its not used to separate three digits (see point 3).Whereas in English, the serial comma (the one before and in a list) is optional, it cannot be used in French:  Jai achetà © un livre, deux stylos et du papier.  Not Jai achetà © un livre, deux stylos, et du papier. Note: When  writing numerals, the period and comma are opposites in the two languages:   French English 2,5 (deux virgule cinq)2.500 (deux mille cinq cents) 2.5 (two point five)2,500 (two thousand five hundred) Two-Part Punctuation Marks In French, a space is required both before and after all two- (or more) part punctuation marks and symbols, including : ;  «  » ! ? % $ #. Colon or Les Deux-Points : The colon is much more common in French than in English. It may introduce direct speech; a citation; or the explanation, conclusion, summary, etc. of whatever precedes it. Jean a dit :  « Je veux le faire.  » Jean said, I want to do it.Ce film est trà ¨s intà ©ressant : cest un classique. This movie is interesting: its a classic.  «  » Les Guillemets and - Le Tiret and ... Les Points de Suspension Quotation marks (inverted commas) dont exist in French; the guillemets  «  » are used.   Note that these are actual symbols; they are not just two angle brackets typed together . If you dont know how to type guillemets, see this  page on typing accents. Guillemets are usually used only at the beginning and end of an entire conversation. Unlike in English, where any non-speech is found outside of the quotation marks, in French guillemets do not end when an incidental clause (he said, she smiled, etc.) is added. To indicate that a new person is speaking, atiret (m-dash or em-dash) is added. In English, an interruption or trailing off of speech can be indicated with either atiret or des points de suspension (ellipsis). In French, only the latter is used.  « Salut Jeanne ! dit Pierre. Comment vas-tu ? "Hi Jean!" Pierre says. "How are you?" - Ah, salut Pierre ! crie Jeanne. "Oh, hi Pierre!" shouts Jeanne. - As-tu passà © un bon weekend ? "Did you have a nice weekend?" - Oui, merci, rà ©pond-elle. Mais... "Yes, thanks," she responds. "But- " - Attends, je dois te dire quelque chose d'important  ». "Wait, I have to tell you something important." The tiret can also be used like parentheses, to indicate or emphasize a comment: Paul - mon meilleur ami - va arriver demain. Paul- my best friend- will arrive tomorrow. Le Point-Virgule ; and  Le Point dExclamation ! and  Le Point dInterrogation ? The semi-colon, exclamation point, and question mark are essentially the same in French and English. Je taime; maimes-tu? I love you; do you love me?Au secours! Help!

Human Resource Management in Practice Essay Example | Topics and Well Written Essays - 3500 words - 1

Human Resource Management in Practice - Essay Example eed to know how human resources (HR) are managed in different regions of the world and how their counterparts in different parts of the globe perceive or react to similar concepts and pressures. It is also important to have an understanding about the main determinants of HRM policies and practices in different regional and national settings. Academics have responded positively to meet the challenges raised by the globalization of business by investigating a number of issues and problems related to international business . They have attempted to examine management from a cross-national viewpoint. This comparison of HRM policies and practices at a national level helps to test the convergence–divergence thesis. The typical questions pursued by comparative researchers are: (1) how is HRM structured in individual countries. (2) What strategies are discussed? (3) What is put into practice? (4) What are the similarities and differences? (5) What is the influence of national factors such as culture, government policy, and education systems? Scholars have also developed and proposed different models of HRM both between and within nations ((Mullins P.97–99, 2002)). Interestingly, most models of HRM have an Anglo–Saxon base. As such, from a global perspective, principles of HRM have been developed from a restricted sample of human experience. During the infancy stage of HRM literature, such an ethnocentric approach was understandable and unavoidable. However, with the growth of a â€Å"global business village,† firms operating in different countries need appropriate information and guidance to develop their HRM policies and practices. Under such dynamic business conditions, the relevance of lessons learned from the Anglo–Saxon experience is questionable. It is therefore important to examine the extent to which Anglo–Saxon models of HRM are applicable in other parts of the world. It has now become clear that the study of HRM needs a cross-national comparative

Horizon Automation System Essay Example | Topics and Well Written Essays - 1500 words

Horizon Automation System - Essay Example The standards based system provides an interface for remote public access and inter library operations like ILL (Inter Library Loaning). The main features of the library automation system are described as: Online Catalogs - Anglo American Cataloguing Rules (AACR) are used for constructing catalogues in the library system. The cataloguing is done based on the two classes of materials: monographs and continuing resources. AACR2 (AACR 2nd edition) defines "monograph" as: The serial is a continuing resource issued in a succession of discrete parts, usually bearing numbering, that has no predetermined conclusion. E.g. journals, magazines, newspapers, and monographic series. The integrating resource is the work that is updated and integrated into the whole. E.g. updating web sites. Authority Record - provide information about individual names, subjects and uniform titles that are used in the bibliographic records, e.g. Author, Publisher, etc. Authority records provide cross-references in the catalogues. Record Creation - The bibliographic record is created in the library system when CIP (Catalogue-In-Publication) record is received from the bibliography publishing agency or is locally entered. The holdings and item records are created when the physical object is received. Record Edit - The record is edited when either an update to t... The bibliographic record must exist before holdings record is created. Item Record - identifies a physical piece - book, CD, etc and links it to a barcode number that is used for circulation. Authority Record - provide information about individual names, subjects and uniform titles that are used in the bibliographic records, e.g. Author, Publisher, etc. Authority records provide cross-references in the catalogues. Record Creation - The bibliographic record is created in the library system when CIP (Catalogue-In-Publication) record is received from the bibliography publishing agency or is locally entered. The holdings and item records are created when the physical object is received. Record Edit - The record is edited when either an update to the CIP record is received (any modifications in the published information), the item is made available to the library, or if there are any modifications to any of the field information in the item catalogue. Record Import - The import of a record is performed when the requested information is not available in the local library system. The search request is submitted through the Z39.50 client to the preferred partners (OCLC server) who can loan the desired item. The server returns the requested record. MARC Record Management The MARC formats are the standards for the representation and communication of bibliographic and related information in machine-readable form. The cataloguing information is maintained on the typed cards and in online bibliographic records as: Author Title Edition Place of Publication Publisher Date of Publication Subject Headings, Etc. The Library of Congress needed to develop software which allowed cataloguers to enter their

Artist Statement (Describe the photographies) Assignment

Artist Statement (Describe the photographies) - Assignment Example He has adopted a classic ruminating pose. In Math Problem (05_lee.jpg), we have the clear case of a student apparenetly solving a math problem in the library. He is taking help from an online source via a laptop, as well as referring to his notebook for writing the solution. He seems tired. Care has been taken to include as much of the setting as possible. In Group Session (06_lee.jpg), we have the case for a frontal photo representation of a group of students that appear to be working on a joint problem or in a group. They are looking at their laptops, which are a ubiquitous symbol of American life and indeed of education and the youth. An everpresent Pepsi lies on the table for refreshment. In Photograph 8 (08_lee.jpg), the emphasis shifts outside in the open air, as our subject is a female student sitting crosslegged in a public park, her schoolbag tossed by her side. The angle of the photography is rather unique and accentuates the lights in the park among the trees, as well as in the spectacles worn by the subjet. She seems hard at work and is apparently a nature lover or prefers the quiet of this venue compared to a noisy and closeted library. In Photograph 9 (09_lee.jpg), we see another image of the same subject. She has been interrupted and looks up with surprise. She seems a little taken aback, although there is a glimpse of a smile as her picture is being taken. It is obvious that she was not ready for this. In Photograph 10 (10_lee.jpg), we see a very happy student near the door of a dormitory or study area in a college or university. He has turned to face the camera. It is obvious that he has heard some very good news and we can only wonder what it is as there are no other visual cues. We can imagine that he has got A grades in one or more exams. In Photograph 11(11_lee.jpg), we have the camera looking down towards many subjects in the library area. It is just to show a new focus from a new angle. The subjects are doing different things,

Partial Molar Properties And Their Application

Partial Molar Properties And Their Application Thermodynamics deals with energy changes and its relationship with work. It is based on three laws of thermodynamics which are used as axioms just as Newtons laws motion from the basis of classical mechanics. The first two laws are based on facts observed in every day life. The predictions based on these laws have been verified in most cases and so far no case has been reported where the laws break down. The laws can be stated in mathematical form. Hence, thermodynamics is an exact science. The thermodynamic theory can be developed without gaps in the argument using only moderate knowledge of mathematics. [B.]ABOUT PARTIAL MOLAR PROPERTY: Thermodynamic relations derived earlier are applicable to closed systems. In a system where not only the work and heat but also several kinds of matter are being exchanged, a multicomponent open system has to be considered. Here, the amounts of the various substances are treated as variables like any other thermodynamic variables. For example, the gibbs free energy of a system is a function not only of temperature and pressure , but also of the amount of each substance in the system,such that G=f(T,p,n1,n2à ¢Ã¢â€š ¬Ã‚ ¦Ãƒ ¢Ã¢â€š ¬Ã‚ ¦.nk) Where n1,n2,à ¢Ã¢â€š ¬Ã‚ ¦.,nk represent the amounts of each of the K components in the system . for simplicity, let a system contain only two components. The total differential of G is dG=(?G/?T)P,n1,n2 dT+(?G/?p)T,n1,n2 dp+(?G/?n1)T,p,n2 dn+(?G/?n2)T,p,n1 dn2 In this eq., the partial derivatives (?G/?n1)T,P,n2 and (?G/?n2)T,P,n1 are known as partial molar free energies of components one and two , respectively. In genral, the partial derivative of a thermodynamic function Y with respect to the amount of component i of a mixture when T,p and amounts of other constituents are kept constant , is known as the partial molar property of the ith component and is represented as Yi,pm. Thus Yi,pm=(?Y/?ni)T,p,njs i=!j [C.]DEFINITION OF PARTIAL MOLAR PROPERTY: The partial molar property may be defined in either of the following two ways: 1. it is the change in Y when 1 mole of component i is added to a system which is so large that this addition has a negligible effect on the composition of the system. 2. Let dY be the change in value of Y when an infinitesimal amount dni of component i is added to a sysem of definite composition. By an infinitesimal amount dni we mean that its addition does not cause any appreciable change in the composition of the system. If we divide dY by dni , we get the partial molar property (?Y/?ni). thus, the partial molar property of the component i may be defined as the change in Y per mole of component i when an infinitesimal amount of this component is added to a system of definite composition. [D.]TYPES OF MOLAR PROPERTIES: (a.) Partial molar volume: The partial molar volume is broadly understood as the contribution that a component of a mixture makes to the overall volume of the solution. However, there is rather more to it than this: When one mole of water is added to a large volume of water at 25 °C, the volume increases by 18cm3. The molar volume of pure water would thus be reported as 18cm3 mol-1. However, addition of one mole of water to a large volume of pure ethanol results in an increase in volume of only 14cm3. The reason that the increase is different is that the volume occupied by a given number of water molecules depends upon the identity of the surrounding molecules. The value 14cm3 is said to be the partial molar volume of water in ethanol. In general, the partial molar volume of a substance X in a mixture is the change in volume per mole of X added to the mixture. The partial molar volumes of the components of a mixture vary with the composition of the mixture, because the environment of the molecules in the mixture changes with the composition. It is the changing molecular environment (and the consequent alteration of the interactions between molecules) that results in the thermodynamic properties of a mixture changing as its composition is altered. The partial molar volume, VJ, of any substance J at a general composition, is defined as: Fig: the partial molar volumes of water and ethanol at 25degree C where the subscript n indicates that the amount of all the other substances is held constant. The partial molar is the slope of the plot of the total volume as the amount of J is changed with all other variables held constant: Note that it is quite possible for the partial molar volume to be negative, as it would be at II in the above diagram. For example, the partial molar volume of magnesium sulphate in water is -1.4cm3 mol-1. i.e. addition of 1 mol MgSO4 to a large volume of water results in a decrease in volume of 1.4 cm3. (The contraction occurs because the salt breaks up the open structure of water as the ions become hydrated.) Once the partial molar volumes of the two components of a mixture at the composition and temperature of interest are known, the total volume of the mixture can be calculated from: The expression may be extended in an analogous fashion to mixtures with any number of components. The most common method of measuring partial molar volumes is to measure the dependence of the volume of a solution upon its composition. The observed volume can then be fitted to a function of the composition (usually using a computer), and the slope of this function can be determined at any composition of interest by differentiation. (b.) Partial molar gibbs energies: The concept of a partial molar quantity can be extended to any extensive state function. For a substance in a mixture, the chemical potential is a defined as the partial molar gibbs energy: i.e. the chemical potential is the slope of a plot of the Gibbs energy of the mixture against the amount of component J, with all other variables held constant: In the above plot, the partial molar Gibbs energy is greater at I than at II. The total Gibbs energy of a binary mixture is given by: The above expression may be generalised quite trivially to a mixture with an arbitrary number of components: where the sum is across all the different substances present in the mixture, and the chemical potentials are those at the composition of the mixture. This indicates that the chemical potential of a substance in a mixture is the contribution that substance makes to the total Gibbs energy of the mixture. In general, the Gibbs energy depends upon the composition, pressure and temperature. Thus G may change when any of these variables alter, so for a system that has components A, B, etc, it is possible to rewrite the equation dG = Vdp SdT (which is a general result that was derived here) as follows: which is called the fundamental equation of chemical thermodynamics. At constant temperature and pressure, the equation simplifies to: Under these conditions, dG = dwn,max (as was demonstrated here), where the n indicates that the work is non-expansion work. Therefore, at constant temperature and pressure: The idea that the changing composition of a system can do work should be familiar this is what happens in an electrochemical cell, where the two halves of the chemical reaction are separated in space (at the two electrodes) and the changing composition results in the motion of electrons through a circuit, which can be used to do electrical work. On a final note, it is possible to use the relationships between G and H, and G and U, to generate the following relations: Note particularly the conditions (the variables that must be held constant) under which each relation applies. Fig: the partial molar volumes of water and ethanol at 25degree C where the subscript n indicates that the amount of all the other substances is held constant. The partial molar is the slope of the plot of the total volume as the amount of J is changed with all other variables held constant: Note that it is quite possible for the partial molar volume to be negative, as it would be at II in the above diagram. For example, the partial molar volume of magnesium sulphate in water is -1.4cm3 mol-1. i.e. addition of 1 mol MgSO4 to a large volume of water results in a decrease in volume of 1.4 cm3. (The contraction occurs because the salt breaks up the open structure of water as the ions become hydrated.) Once the partial molar volumes of the two components of a mixture at the composition and temperature of interest are known, the total volume of the mixture can be calculated from: The expression may be extended in an analogous fashion to mixtures with any number of components. The most common method of measuring partial molar volumes is to measure the dependence of the volume of a solution upon its composition. The observed volume can then be fitted to a function of the composition (usually using a computer), and the slope of this function can be determined at any composition of interest by differentiation. (C.)PARTIAL MOLAR THERMAL PROPERTIES: 1. Partial molar heat capacities: the heat capacity at constant pressure Cp of a solution containing n1 moles of solvent and n2 moles of solute is given by Cp=(?H/?T)P,N à ¢Ã¢â€š ¬Ã‚ ¦Ãƒ ¢Ã¢â€š ¬Ã‚ ¦Ãƒ ¢Ã¢â€š ¬Ã‚ ¦Ãƒ ¢Ã¢â€š ¬Ã‚ ¦Ãƒ ¢Ã¢â€š ¬Ã‚ ¦Ãƒ ¢Ã¢â€š ¬Ã‚ ¦eq(1) The pressure and compostion being constant. Upon differentiation with respect to n1,maintaining n2 constant,it follows that CP1=(?CP/?n1)T,P,n2 =?H/?T?n1 .eq(2) Where Cp1 is the partial molar heat capacity,at constant pressure,of the constituent 1 of the given solution. The partial molar heat constant H1 of this constituent is defined by H1=(?H/?n1)T,P,n2 And hence differentiation with respect to temp. gives (?H1/?T)P,N=?H/?T?n1 =CP1 à ¢Ã¢â€š ¬Ã‚ ¦Ãƒ ¢Ã¢â€š ¬Ã‚ ¦Ãƒ ¢Ã¢â€š ¬Ã‚ ¦Ãƒ ¢Ã¢â€š ¬Ã‚ ¦Ãƒ ¢Ã¢â€š ¬Ã‚ ¦Ãƒ ¢Ã¢â€š ¬Ã‚ ¦.eq(3) The result being identical with CP1 by eq.(3). The partial molar heat capacity of the solvent is any particular solution thus be defined by either eq(1) and eq(2). Similarly,i.e.,constituent 2, Cp2=(?CP/?n2)T,P,n1 =(?H2/?T)P,N à ¢Ã¢â€š ¬Ã‚ ¦Ãƒ ¢Ã¢â€š ¬Ã‚ ¦Ãƒ ¢Ã¢â€š ¬Ã‚ ¦Ãƒ ¢Ã¢â€š ¬Ã‚ ¦Ãƒ ¢Ã¢â€š ¬Ã‚ ¦Ãƒ ¢Ã¢â€š ¬Ã‚ ¦Ãƒ ¢Ã¢â€š ¬Ã‚ ¦..eq(4) We know, Li=H1-H10 Is differentiated with respect to temp.,at constant pressure and composition,it follows that (?L1/?T)P,N=(?H1/?T)P,N-(?H10/?T)P,N = Cp1-Cp10 à ¢Ã¢â€š ¬Ã‚ ¦Ãƒ ¢Ã¢â€š ¬Ã‚ ¦Ãƒ ¢Ã¢â€š ¬Ã‚ ¦Ãƒ ¢Ã¢â€š ¬Ã‚ ¦Ãƒ ¢Ã¢â€š ¬Ã‚ ¦Ãƒ ¢Ã¢â€š ¬Ã‚ ¦Ãƒ ¢Ã¢â€š ¬Ã‚ ¦Ãƒ ¢Ã¢â€š ¬Ã‚ ¦eq(5) Where Cp1,identical with Cp1 or Cp1o, is the molar heat capacity of the pure solvent or the partial molar heat capacity of the solvent in a solution at infinite dilution. Thus, Cp10 may be regarded as an experimental quantity, and if the variation of the relative partial molar heat content of the solvent with temperature,i.e. (?L1/?T)P,N, is known , it is possible to determine Cp1 at the corresponding composition of the solution. The necessary data are rarely available from direct thermal measurements of L1, such as thus described in 44f,at several temperatures, but the information can often be obtained, although not very accurately from E.M.F measurements. By differentiating the expression for the relative partial molar heat content of the solute it is found, in an exactly similar manner to that used above , that (?L2/?T)P,N=(?H2/?T)P,N-(?H02/?T)P,N =CP2-CP20 à ¢Ã¢â€š ¬Ã‚ ¦Ãƒ ¢Ã¢â€š ¬Ã‚ ¦Ãƒ ¢Ã¢â€š ¬Ã‚ ¦Ãƒ ¢Ã¢â€š ¬Ã‚ ¦Ãƒ ¢Ã¢â€š ¬Ã‚ ¦Ãƒ ¢Ã¢â€š ¬Ã‚ ¦Ãƒ ¢Ã¢â€š ¬Ã‚ ¦Ãƒ ¢Ã¢â€š ¬Ã‚ ¦Ãƒ ¢Ã¢â€š ¬Ã‚ ¦Ãƒ ¢Ã¢â€š ¬Ã‚ ¦Ãƒ ¢Ã¢â€š ¬Ã‚ ¦Ãƒ ¢Ã¢â€š ¬Ã‚ ¦eq(6) In this expression,Cp20 is the partial molar heat capacity of the solute in the infinitely dilute solution. Although the experimentel significance of the quantity is not immediately obvious.thus from a knowledge of the variation of L2, the partial molar heat content of the solute with temprature it should be possible to derive, with the aid of equation(6) , the partial molar heat capacity of the solute Cp2 at the given composition. [E.]Determination of partial molar properties: 1.Direct method: in view of the definition of the partial molar properties Gi as Gi=(?G/?ni)T,P,n1,à ¢Ã¢â€š ¬Ã‚ ¦.. à ¢Ã¢â€š ¬Ã‚ ¦Ãƒ ¢Ã¢â€š ¬Ã‚ ¦Ãƒ ¢Ã¢â€š ¬Ã‚ ¦Ãƒ ¢Ã¢â€š ¬Ã‚ ¦Ãƒ ¢Ã¢â€š ¬Ã‚ ¦.eq(1) An obvious method ffor its determination is to plot the value of the extensive properties G,at constant temperature and pressure, for various mixtures of the two components against the number of moles,e.g.,n2,of the one of them,the value of n1 being kept constant. The slope of the curve at any particular composition,which maybe determined by drawing a tengent to the curve, gives the value of G2 at that comoposition. Since the molality of a solution represents the number of moles of solute associated with a constant mass,and hence a constant number of moles,the plot of the property G against the molality can be used for the evaluation of the partial molar property of the solute. Once G2 at any composition has been determined, the corresponding value of G1 is readily derived by means of the relationship, G=n1G1+n2G2 In view of the difficulty of determining the exact slope of the curve at all points, it is preferable to use an analytical procedure instead of the graphical one just described. The property G is then expressed as a function of the number of moles of one component,e.g.,the molality, associated with a constant amount of the other component. Upon differentiation with respect to n,i.g.,the molality, an expression for the partial molar property is obtained. 2.from apparent molar properties: a method that is often more convenient and accuarate than that described above,makes use of the apparent molar property. We know G-n1G1=n2à ¶2 If n1 is maintained constant,so that n1G1 is constant, differentiation with respect to n2 , constant temp. and pressure being understood,gives G2 =(?G/?n2)n1 = (?à ¶G/?n2)n1 + à ¶G à ¢Ã¢â€š ¬Ã‚ ¦Ãƒ ¢Ã¢â€š ¬Ã‚ ¦Ãƒ ¢Ã¢â€š ¬Ã‚ ¦Ãƒ ¢Ã¢â€š ¬Ã‚ ¦Ãƒ ¢Ã¢â€š ¬Ã‚ ¦Ãƒ ¢Ã¢â€š ¬Ã‚ ¦Ãƒ ¢Ã¢â€š ¬Ã‚ ¦eq(2) G2 = ((?à ¶G/? ln n2)n1+ à ¶G à ¢Ã¢â€š ¬Ã‚ ¦Ãƒ ¢Ã¢â€š ¬Ã‚ ¦Ãƒ ¢Ã¢â€š ¬Ã‚ ¦Ãƒ ¢Ã¢â€š ¬Ã‚ ¦Ãƒ ¢Ã¢â€š ¬Ã‚ ¦Ãƒ ¢Ã¢â€š ¬Ã‚ ¦Ãƒ ¢Ã¢â€š ¬Ã‚ ¦Ãƒ ¢Ã¢â€š ¬Ã‚ ¦Ãƒ ¢Ã¢â€š ¬Ã‚ ¦Ãƒ ¢Ã¢â€š ¬Ã‚ ¦..eq(3) Since the molality m is equivalent to n2, with n1 constant, eq(2) and eq(3) may be written as G2= m (d à ¶G/dm)+ à ¶G à ¢Ã¢â€š ¬Ã‚ ¦Ãƒ ¢Ã¢â€š ¬Ã‚ ¦Ãƒ ¢Ã¢â€š ¬Ã‚ ¦Ãƒ ¢Ã¢â€š ¬Ã‚ ¦Ãƒ ¢Ã¢â€š ¬Ã‚ ¦eq(4) G2=( d à ¶G/d ln m)+ à ¶G à ¢Ã¢â€š ¬Ã‚ ¦Ãƒ ¢Ã¢â€š ¬Ã‚ ¦Ãƒ ¢Ã¢â€š ¬Ã‚ ¦Ãƒ ¢Ã¢â€š ¬Ã‚ ¦Ãƒ ¢Ã¢â€š ¬Ã‚ ¦..eq(5) Respectively. If the apparent molar property à ¶G is determined for various values of n2 , with n1 constant , or at various molalities, the partial molar property G2 can be calculated from the slope, at any given composition, of the plot of à ¶G against n2 or against ln n2. The method based on the use of eqs(3)(5) is usally more accurate than that involving the logarithmic plot,since it does not give undue importance to result obtained in dilute solutions. An analytical method can, of course, be used in place of the graphical procedure if à ¶G can be expressed as a function of n2 or of the molality. For use in a later connection, an alternative form of eq(4) is required and it will be derived here. The right hand side of this equation is equivalent to d(m à ¶G)/dm, that is, m (d à ¶G/dm)= G2 and upon integration, m varying between the limits of zero and m, and mdà ¶G between zero and mà ¶G, it is found that mà ¶G=?0m G2 dm à ¶G=1/m?0m G2 dm for dilute solutions,the molality is proportional to the molar concentration c, and hence it is permissible to put this result in the form à ¶G=1/c?0m G2 dm [F.] APPLICATION OF PARTIAL MOLAR PROPERTIES: These properties are very useful since each and every reaction in chemistry occurs at a constant temperature and pressure and under these conditions we can determine these with the help of partial molar properties. They are highly useful when specific properties of pure substances and properties of mixing are considered. By definition, properties of mixing are related to those of the pure substance by: Here * denotes the pure substance M the mixing property z corresponds to the specific property From the definition of partial molar properties, substitution yields: Hence if we know the partial molar properties we can derive the properties of mixing.For the internal energy U, enthalpy H, Helmholtz free energy A, and Gibbs free energy G, the following hold: whereP is the pressure V is the volume T is temperature S is the entropy [G.] BIBLIOGRAPHY: 1. THERMODYNAMICS AND CHEMICAL EQUILIBRIUM AUTHOR: K L KAPOOR 2. THERMODYNAMICS FOR CHEMISTS AUTHOR: SAMUEL GLASSTONE 3. http://www.everyscience.com/Chemistry/Physical/Mixtures/a.1265.php 4. http://www.everyscience.com/Chemistry/Physical/Mixtures/b.1266.php 5. http://www.chem.ntnu.no/nonequilibrium-thermodynamics/pub/192-Inzoli-etal.pdf 6. http://physics.about.com/od/thermodynamics/p/thermodynamics.htm 7. http://www.chem.boun.edu.tr/webpages/courses/chem356/EXP5-Determination%20of%20Partial%20Molar%20Quantities.pdf

Shakespeares Hamlet †Ophelia Discussed Essays -- GCSE English Litera

Hamlet – Ophelia Discussed Courtney Lehmann and Lisa S. Starks in "Making Mother Matter: Repression, Revision, and the Stakes of 'Reading Psychoanalysis Into’ Kenneth Branagh's Hamlet" make a statement regarding the effect of Ophelia’s words, even though she was considered mad at the time: Hamlet's own disgust toward the body and sexual behaviour, coupled with Ophelia's erotically-charged songs, did not suddenly become "about" sexuality after Freud. On the contrary, censorship of the play in performance during various historical time periods indicates that the tragedy has always been perceived of as highly erotic, and often dangerously so. Even in the context of twentieth-century interpretations of Hamlet, critics have been reluctant to engage in genuine confrontations with the problem of the play's sexuality and its underlying anxiety. For this reason, Jacqueline Rose has claimed that critics writing on Hamlet, beginning with T. S. Eliot, have conflated their puzzlement over the play with the Western notion of "woman" as the bearer of an impenetrable secret. (2) Shakespeare’s tragedy, Hamlet, presents almost a dozen male characters for every one female character. The only prominent female characters are two: Ophelia, Laertes’ sister and Polonius’ daughter; and Gertrude, the queen and wife of Claudius and mother of Hamlet. This essay will explore the character, role, and importance of Ophelia. The protagonist of the tragedy, Prince Hamlet, initially appears in the play dressed in solemn black, mourning the death of his father supposedly by snakebite while he was away at Wittenberg as a student. Hamlet laments the hasty remarriage of his mother to his father’s brother, an incestuous act; thus in his first soliloqu... ...akes of 'Reading Psychoanalysis Into' Kenneth Branagh's Hamlet." Early Modern Literary Studies 6.1 (May, 2000): 2.1-24   http://purl.oclc.org/emls/06-1/lehmhaml.htm Pennington, Michael. â€Å"Ophelia: Madness Her Only Safe Haven.† Readings on Hamlet. Ed. Don Nardo. San Diego: Greenhaven Press, 1999. Rpt. From Hamlet: A User’s Guide. New York: Limelight Editions, 1996. Pitt, Angela. â€Å"Women in Shakespeare’s Tragedies.† Readings on The Tragedies. Ed. Clarice Swisher. San Diego: Greenhaven Press, 1996. Rpt. from Shakespeare’s Women. N.p.: n.p., 1981. Shakespeare, William. The Tragedy of Hamlet, Prince of Denmark. Massachusetts Institute of Technology. 1995. http://www.chemicool.com/Shakespeare/hamlet/full.html Wilkie, Brian and James Hurt. â€Å"Shakespeare.† Literature of the Western World. Ed. Brian Wilkie and James Hurt. New York: Macmillan Publishing Co., 1992.