William Blake And Romanticism Essays - William Blake,

William Blake And Romanticism William Blake lived from 1757-1827. He based most of his works in the style of Romanticism. Much like William Wordsworth, Blake wrote from the heart, letting natural expression take over. Many of the writers of the Romantic period felt they had entered an imaginative climate, which some of them called "the Spirit Age." During this "Spirit Age," many authors felt that freedom and spontaneity were the key elements in poetry. Before this creative revolution, a poem was considered a classical work of art, assimilated to please an audience. In Romanticism, the "rules" hanging over poetry were dropped and a piece of work could become, as Blake described, "an embodiment of the poet's imagine vision." Blake used these free-formed ideas and concepts in his later works. These essays, All Religions Are One, There is No Natural Religion (a), and There is No Natural Religion (b), all show Blake's views against Christian Orthodox, religion based on ancient scripture and against "Natural Religion," the belief that God is as natural organism, much like man. Blake was opposed to the idea that God is only what the church believes him to be but he was also opposed to the notion that God was here before we were. Blake believed that man's "Poetic Genius," or imagination helped create the God of today. Many of the writers of the Romantic period were highly influenced by the war between England and France and the French Revolution. During the war, Blake was faced with charges of "speaking against his King and country." People of this era felt his works tested the boundaries of good art. Many of the other writers of this time also challenged previously accepted ideas. Mary Wollstonecroft wrote "A Vindication of the Rights of Women." Her work stood up against the female stereotypes and preconceived notions about women. In the midst of all these changes, Blake too was inspired to write against these ancient ideas. All Religions Are One, There is No Natural Religion (a), and There is No Natural Religion (b) were composed in hopes of bringing change to the public's spiritual life. Blake felt that, unlike most people, his spiritual life was varied, free and dramatic. Growing up he had no formal education. At the age of ten he joined a drawing school and later studied for a short time at a prestigious art school, the Royal Academy of the Arts. From this point in his life, art had the strongest influence. Later on, his work diminished and he went to a friend who was an artist, William Haley, for help. Haley attempted to change Blake's free art into conventional and breadwinning art. Blake soon rebelled, calling Haley the enemy of his spiritual life. After all of this, he began to write poetry, hoping to revive his free expression and flow. He wrote three works around 1788, to illustrate his views on religion, All Religions Are One, There is No Natural Religion (a), and There is No Natural Religion (b). He wrote All Religions Are One directed against Deism or "Natural Religion" and against Christian Orthodoxy. Blake felt that God is not a natural or organic being, he is a creation of man's imagination or "Poetic Genius." He states that "The Jewish and Christian Testaments are an original derivation from the Poetic Genius," supporting his theory that man has imagined God. In There is No Natural Religion (a), he speaks against the argument that man naturally perceives God. He states that the desires and perceptions of man are not natural or organic, but are things taught to us. In the end, Blake reminds us that is all things in this world were accepted as "natural," then "the Philosophic and Experimental would soon be at the ratio of all things, and stand still unable to do other than repeat the same dull round over again." We as humans, are too dependent upon acceptance and not enough on independence. In There is No Natural Religion (b), Blake tries to persuade his audience that our knowledge is not limited to the physical sense, it is free and unbounded, much like Blake's ideal spiritual life.

Local # portability essays

Local # portability essays On November 22, 2003 the Federal Communications Commission (F.C.C.) Mandated a law called Local Number Portability or L.N.P. On that day on which L.N.P. came into effect, wireless customers swarmed into local Verizon Wireless retail stores nationwide. The porting process can take anywhere from three hours to three days depending on the original service provider and when that service provider releases the number for use by a new carrier. One particular customer in the Verizon store where I work ported his number on the 22nd of November. However, his phone did not yet port over as late as the first week of December. This was a difficult problem because the customer had to carry two phones for two weeks and was also being billed by two carriers. At the time I realized that if I wanted this customer to continue doing business with my store. I would have to do something quick to satisfy him with our service and to his portability dilemma. First, I had to make sure the port would go through. To solve this problem, I called Verizon Wireless and spoke with a dealer support representative. I explained the problem and insisted that if the port did not go through, the customer would cancel service and return with his original service provider. Knowing that the customer would cancel, the representative made several calls and within minutes the number ported over. I also let the Verizon representative know that I believed that the customer should not have to pay for service he was not able to use . In the end, the representative gave a credit to the customer for one month service. The next thing needed to be taken care of was the bill ...

Individual Paper Assignment 2 - Frivolous Law Suits Reactions and Essay

Individual Paper Assignment 2 - Frivolous Law Suits Reactions and Analysis - Essay Example It means the person arguing the position has absolutely no idea of what he is doing, and has completely wasted the time of everyone. It doesnt denote that the case was not well argued, or that judge simply decided for the other side, but it indicates that there was no other side. The argument may turn out to be absurd and incompetent. The judge is not telling you that you are "wrong." The judge is telling you that you are out of your mind.† Yet another definition of Frivolous law was defined in the case â€Å"Texaco, Inc. v. Golart, 206 Conn. 454, 463-464, 538 A.2d 1017 (1988)†wherein it was defined as: â€Å"The definition of a frivolous appeal is set forth in the comment to Rule 3.1, wherein it is stated that â€Å"the action is frivolous if the client desires to have the action taken primarily for the purpose of harassing or maliciously injuring a person or if the lawyer is unable either to make a good faith argument on the merits of the action taken or to support the action taken by a good faith argument for an extension, modification or reversal of existing law.† Let us take the cases of Liebeck v. McDonalds Restaurants 1994, and Pearson v. Chung case filed in 2005. In February of 1992, Stella Liebeck of Albuquerque, New Mexico, was travelling in the passenger seat of her grandsons car when she was severely burned by McDonalds coffee. She was 79 years old then. The coffee was served in a Styrofoam cup at the drive through the window of a local McDonalds. After the coffee was served the grandson pulled his car forward and halted temporarily for Liebeck to add cream and sugar to her coffee. Liebeck positioned the cup in between her knees and tried to take away the plastic lid from the cup. As soon as she opened the lid, the whole contents of the cup poured forth onto her lap. Liebeck was wearing sweatpants and it absorbed the

Financial Reporting and Analysis Assignment Example | Topics and Well Written Essays - 1250 words

Financial Reporting and Analysis - Assignment Example 2) Non-cash items usually include those items which do not include the transfer of money. The most feasible way for adjusting non-cash items is by adding the same form the net income of the firm (Hung, 2000). 3) The stock market participants were able to predict the fall in the revenues of Charter. As a result the company’s stock prices began being priced low by the stock market forces. A low price allocates a low level of dividend (Berk & DeMarzo, 2013). A low share price allocation also helps a firm to attract a large number of small investor (Rioja & Valev, 2004). However a declining share price also indicates a firm’s low revenue which also repels a number of investors who expect growth and rising dividends (Chandra, 2005). The financial performance of airlines industry is generally analyzed on the basis of return on equity (ROE) or return on assets (ROA). The airline industry is immensely capital intensive and profitability is usually measured on the basis of returns available on equity or assets. Accordingly it is seen that the ROA for the airlines industry on an average is around 9.8. From the given data it is seen that firm 6 incurs a ROA ratio of 9.95. Hence this firm belongs to the airlines industry. Banking firms puts special emphasis upon the returns from operations. Hence net margin is usually one of the critical parameters for judging the efficiency of the firms in this sector. The banking industry usually incurs a net profit margin of 16. From the given data set, it is seen that firm 9 has a net profit margin of 12.82. Most brewery firms analyze their financial effectively by analyzing the gross margin ratio. Breweries usually have a gross profit margin of 60. From the given data it can therefore be analyzed that firm 8 has a gross profit of 60.21. Hence firm 8 belongs to brewery industry. Departmental stores usually experience a very high level of liquidity and hence

Should Taxpayer's Continue To Fund Welfare and Do Illegal Immigrants Research Paper

Should Taxpayer's Continue To Fund Welfare and Do Illegal Immigrants Contribute To The Welfare State - Research Paper Example The bottom line of all of this is that every group has strong points and arguments that are valid to differing degrees. But discounting a massive revolution that restructures the government completely and re-imagines a new set of core American values, the welfare system should be at very least left intact, and at best vastly restructured and better funded. It is better for American society overall, and more in line with fundamental American values, to continue to fund the welfare state. To understand the welfare state in America one must first understand a little bit about its history. Unlike Europe, patronizing liberal-democracy thinking and Christian fundamentals played little role in developing the welfare system in the United States (Trattner 5). Instead, the welfare system in the United States has always been developed, cut or expanded depending on economic circumstances. It was born out of the Great Depression as part of the New Deal Program (Trattner 7). The basic premise at t his time was that there were massive numbers of people who were willing to work, but far too few jobs available even after the expansion of federal work programs. President Roosevelt essentially either had the choice of instituting a welfare system or letting people starve (Tratter 102). The Great Society period of the 1960s saw welfare expand so that someone who was neither infirm, young nor elderly could get enough to live on through welfare payments from the US government (Lawrence and Strakey 19). The last major change in welfare occurred during the booming economy of the 1990s under Bill Clinton. In this first massive cut of the welfare state, which saw welfare return to the states rather than the federal government, and become a smaller and more temporary program than it had been in the past. At the time of record-low unemployment, booming compensation and a robust economy under Clinton, it seemed inconceivable that anyone who wanted to work would be unable to in the long term , so it seemed that the only people on welfare were people unwilling to work, so the cuts seemed justified. This change has been lauded as one of the best in the history of welfare in the United States, because poverty levels dropped substantially and welfare rolls decreased along with this change (78). The problem, however, is that the decrease in poverty was largely a function of a robust and booming economy, not the changes in welfare law. Though the economic affairs of the US have shifted drastically in the last decade, the welfare system instituted by the Clinton administration in 1996 is essentially the same one in operation now. Welfare obviously has a long history in the United States, but this does not explain the arguments for keeping or further funding welfare. There are two main sets of arguments, ideological and some practical. The first ideological argument comes from some of the founding documents of the United States. The Declaration of Independence argues that †Å"all men are created equal.† The problem, however, is that this is self-evidently not true. Some people are born with a brain that is incapable of accomplishing many tasks whereas others are born geniuses who can unlock the mysteries of science and technology. This fundamental problem has been explained away by saying that this passage means that everyone should have equality of opportunity

Using Recrystallisation Improve The Purity Of Aspirin Biology Essay

Using Recrystallisation Improve The Purity Of Aspirin Biology Essay In this experiment I have investigated the research question How does the process of recrystallisation improve the purity of Aspirin. I used a well documented method of preparing Aspirin. Having obtained the Aspirin I performed several recrystallisation processes on it. I then determined accurately the quantity of Aspirin in each of my sample by volumetric analysis. I was then able to determine purity and percentage yield by comparing it to an original tablet Aspirin in the market. I also used melting point to assess purity. I learnt about Aspirin when we did the chapter medicine and drugs in our class. Aspirin is a very common drug used in our daily lives. The common chemical name is  acetylsalicylic acid. Salicylic acid was identified and isolated from the bark of a willow tree but it could not be synthesised in laboratory. In 1893, Felix Hoffman Jr., a chemist found out a practical way for synthesizing an ester derivative of salicylic acid, acetylsalicylic acid. Acetylsalicylic acid, a weaker acid than salicylic acid, was found to have the medicinal properties of salicylic acid without having the objectionable taste or producing the stomach problems as a side effect. The acetyl group effectively masks the acidity of the drug during its ingestion and after it passes into the small intestine, it is converted back to salicylic acid where it can enter the bloodstream and do its pain relieving action  [1]  . Acetylsalicylic acid is powerful as a pain reliever, fever reducer, and swelling-reducing dru g but it also has faults, it causes stomach irritation to some individuals and also may lead to Reye syndrome in young children. I was excited to see if this drug we use has the same purity when prepared in lab and when bought from outside. Aspirin is an important analgesic therefore methods of improving purity are essential. The preparation of Aspirin involves organic synthesis and I learnt about this process when I studied organic chemistry and it an interesting topic to research about. The preparation of drugs that I use in my daily lives excited me particularly as I want to do biochemistry in university and also work in a pharmaceutical company for drug designing. Hence, I decided upon making aspirin in the lab and researching about it. BACKGROUNG INFORMATION 2.1 Synthesis of Aspirin The above is the reaction for the formation of Aspirin. This organic synthesis is an esterification reaction between a compound containing a OH group (ester) and an acid. Esters are a type of organic acid in which the hydroxide groups are replaced. The H from the OH group is replaced by a carboxyl carbon C=O group.  Esterification is the  acid catalyzed reaction of a carboxyl (-COOH) group and an -OH group of an alcohol or phenol  to form a carboxylate ester. A catalyst is required for the reaction for example concentrated H2SO4.In the synthesis of Aspirin the -OH group is the phenolic -OH  group attached to ring of the salicylic acid  [2]  . 2.2 Purification of Aspirin using the process of recrystallisation I used the process of recrystallisation to investigate how effective this process is in making Aspirin pure. The process of recrystallisation takes advantage of the relative solubilities of contaminants compared to that of Aspirin  [3]  . The technique is to use a solvent in which the solid is sparingly soluble at low temperature and quite soluble at higher temperature (at the boiling point of the solvent). In my research Aspirin is insoluble in cold water and hence in the process of recrystallisation I first dissolved Aspirin crystals into hot water and then let it cool down so that it would crystallize out. The solid is dissolved in the minimum quantity of solvent required to produce a solution at the boiling point of the solvent. Upon cooling the solution to room temperature or below, the solid crystallizes out of solution due to its lower solubility at the lower temperature  [4]  . Impurities (i.e., any foreign substance) in a solid are classified as soluble or insoluble. The removal of insoluble impurities is accomplished by filtering the hot solution. The insoluble impurities remain on the filter paper. Ideally, soluble impurities remain in solution when the solid being purified crystallizes. (Depending upon concentration and solubility of the impurity in the selected solvent it may sometimes be necessary to recrystallise more than one time. That is some of the soluble impurity might also crystallize. If any soluble impurity crystallizes, the melting point of your product will be depressed). When recrystallisation is complete the purified solid is isolated by filtration and the crystals are washed with a small quantity of cold solvent (to rinse off the solution of soluble impurities coating the freshly filtered solid)  [5]  . 2.3 Determination of purity using melting point apparatus I also used melting point determination to give further evidence towards the purity of aspirin. Melting point is a useful measure for the purity of a solid. Melting point apparatus is commonly used for this purpose. It consists of a heated metal block with holes for a thermometer and melting point tubes. The capillary tubes are provided open-ended and the crystalline solid can be transferred into the tube and forced to the bottom with gentle tapping. The compound is heated slowly especially around its melting point for accuracy. There are attractive forces (intermolecular interactions) between the molecules in a solid that keep them together in an ordered crystalline structure. If enough heat energy is added to the solid the internal kinetic energy of the molecules causes them to move in the solid. At the temperature where the energy of molecular motion overcomes the attractive forces between molecules the compound begins to melt. When a solid is pure the molecules are all identical and thus the interactions between molecules are similar and thus the sample will melt at a distinct temperature. Impure compounds, on the other hand, have a range of intermolecular interactions between molecules and will melt over a range of temperatures.  [6]   3. APPARATUS  [7]  :- 3.1 Equipments: The apparatus listed below does not list quantities for repeat readings. Conical flask (100 cm3) (ÃÆ'-1) Measuring cylinders (10 cm3) ( ±0.5cm3) (ÃÆ'-2) Beaker (100 cm3) (ÃÆ'-2) Glass rod (ÃÆ'-1) Vacuum filtration flask (ÃÆ'-1) Rubber tubing for vacuum flask (ÃÆ'-1) Hirsch funnel (ÃÆ'-1) Water bath containing crushed ice (ÃÆ'-1) Source of hot water (ÃÆ'-1) Test-tubes (ÃÆ'-4) Meltemp apparatus for finding the melting point of Aspirin Burette (50cm3) (ÃÆ'-1) Clamp stand (ÃÆ'-1) Spatula (ÃÆ'-2) Watch glass (ÃÆ'-1) Melting point capillary tube (ÃÆ'-1) Filter paper to fit Hirsch funnel (ÃÆ'-1) 3.2 Chemicals: 2-hydroxybenzoic acid (salicylic acid) (2g) Ethanoic anhydride (4cm3) Concentrated sulphuric acid (5 drops) Ethanoic acid (glacial) (4cm3) (1)Aspirin tablet Phenolphthalein solution Sodium hydroxide solution (0.1 mol dm-3) 95% alcohol 4. DIAGRAM: 4.1 Hirsch Funnel: 4.2 Melting Point Apparatus: 5. METHOD  [8]  :- Shake 2g of 2-hydroxybenzoic acid (salicylic acid) (CARE Irritant) with 4 cm3 of ethanoic anhydride (CARE Corrosive) in a 100 cm3 conical flask. Add 5 drops of concentrated sulphuric acid (CARE Corrosive) and continue agitating the flask for about 10 minutes. Crystals of Aspirin will appear and soon the whole will form a crystalline mush. Dilute by stirring in 4cm3 of cold glacial ethanoic acid (CARE Corrosive) and cool by placing in a water bath containing crushed ice. Filter off the crystals using a Hirsch funnel (a small funnel for vacuum filtration), washing once with ice cold water to remove residual acid. Place the crude Aspirin in a 100cm3 beaker. Add hot, but not boiling, water until it dissolves. A mass of very pure Aspirin crystals will form; cool the flask by surrounding it with cold water. Filter them again and rinse the crystals with the chilled water. The insoluble impurities remain on the filter paper and the filtrate contains the product. Aspirin can be recovered from this solution by evaporation of the recrystallisation.  [9]   Leave the crystals overnight on a watch glass to dry completely. This process is known as recrystallisation and is a way of purifying a solid product (Aspirin). Do the recrystallisation process three times and after every recrystallisation remove some sample of Aspirin and store in a test tube to test later. Now do titration of the samples stored after each recrystallisation. Take some of Aspirin for each sample and leave some in the test tube for testing the melting point. For the process of titration, take the Aspirin from each sample into a 50 cm3 conical flask and dissolve it in 5 cm3 of 95% alcohol and add two drops of phenolphthalein solution to it. Titrate the solution in the conical flask with 0.1 mol dm-3 sodium hydroxide from a burette (CARE Eye protection must be worn). Record the volume needed to produce the first tinge of pale pink colour in the indicator. This measure the end-point of the titration. Take a capillary tube and gently press the open end into the pile of Aspirin crystals on the paper so that a  few  crystals of Aspirin  enter the capillary tube. Tap the closed end of the capillary onto the bench top, so that the Aspirin  crystals work their way to the bottom.   The Aspirin crystals should be firmly packed, and fill the capillary tube to a depth of  no more than  1-2 mm.   Insert the capillary tube containing the sample into the melting point apparatus.   Record the temperature where the melting point is first observed and when it becomes a liquid completely.   This is your melting point range.  [10]   Then do the titration of an original tablet of Aspirin available in the market. Then test the melting point of the original tablet of Aspirin by the method described above. Compare the melting point which you get from the samples and the original tablet of Aspirin with the one given in the data booklet. 6. OBSERVATIONS:- When I mixed salicylic acid with ethanoic anhydride, the solution turned milky. When to the solution I added concentrated sulphuric acid, the solution turns colourless and then after agitating for 10 minutes the solution again turns milky white. The beaker is hot and hence we can say that the reaction between concentrated sulphuric acid and the solution (ethanoic anhydride + salicylic acid) is exothermic. When I was doing my melting point I saw that the solid obtained after the first recrystallisation actually turned black before actually getting close to the melting point of the original Aspirin. As the number of recrystallisation increased I could see that the melted Aspirin was still white and was getting closer to the melting point of the original Aspirin (135 °C) as mentioned in the data book. 7. DATA COLLECTION AND PROCESSING:- 7.1 The data of titrations of different recrystallisation samples of Aspirin:- 7.1.1 Original Aspirin tablet Burette solution (cm3) 0.1 mol dm-3 sodium hydroxide solution Indicator Phenolphthalein solution Trial 1st reading 2nd reading 3rd reading Burette readings (cm3) Final ( ±0.1) 44.5 44.0 44.0 44.3 Initial ( ±0.1) 69.0 69.0 69.0 69.0 Volume used (titre) cm3 ( ±0.2) 25.0 25.0 I have not used as they are not concordant. I have used these reading for my mean titre. Mean titre (cm3) ( ±0.2) 25.0 + 25.0 = 50.0 50.0 à · 2 = 25.0 (mean titre) Volumetric calculations Volume of NaOH used = 25.0 cm3. Moles of NaOH n = CV V = 25.0 cm3 = 25.0 à · 1000 = 0.025 dm3 n = 0.1 ÃÆ'- 0.025 = 0.0025 mol So, moles of Aspirin will also be equal to 0.0025mol because the reaction ratio between NaOH and Aspirin is 1:1. Weighed out sample of Aspirin = 0.62 g How many grams of Aspirin reacted with NaOH? Aspirin = C9H8O4 g = n ÃÆ'- Mr = 0.0025 ÃÆ'- Mr [(12.01 ÃÆ'- 9) + (1.01 ÃÆ'- 8) + (16.00 ÃÆ'- 4)] = 0.0025 ÃÆ'- 180.17 = 0.45 g Percentage of Aspirin reacted = (0.45 à · 0.62) ÃÆ'- 100 = 73% 7.1.2 Aspirin after 1st recrystallisation Burette solution (cm3) 0.1 mol dm-3 sodium hydroxide solution Indicator Phenolphthalein solution Trial 1st reading 2nd reading 3rd reading Burette readings (cm3) Final ( ±0.1) 3.4 3.6 3.7 3.8 Initial ( ±0.1) 0.0 0.0 0.0 0.0 Volume used (titre) cm3 ( ±0.2) 3.6 3.7 3.8 I have used these reading for my mean titre. Mean titre (cm3) ( ±0.2) 3.6 + 3.7 + 3.8 = 11.1 11.1 à · 3 = 3.7 (mean titre) Volumetric calculations Volume of NaOH used = 3.7 cm3. Moles of NaOH n = CV V = 3.7 cm3 = 3.7 à · 1000 = 0.0037 dm3 n = 0.1 ÃÆ'- 0.0037 = 0.00037 mol So, moles of Aspirin will also be equal to 0.00037mol because the reaction ratio between NaOH and Aspirin is 1:1. Weighed out sample of Aspirin = 0.30 g How many grams of Aspirin reacted with NaOH? Aspirin = C9H8O4 g = n ÃÆ'- Mr = 0.00037 ÃÆ'- Mr [(12.01 ÃÆ'- 9) + (1.01 ÃÆ'- 8) + (16.00 ÃÆ'- 4)] = 0.00037 ÃÆ'- 180.17 = 0.066 g Percentage of Aspirin reacted = (0. 066 à · 0.30) ÃÆ'- 100 = 22% 7.1.3 Aspirin after 2nd recrystallisation Burette solution (cm3) 0.1 mol dm-3 sodium hydroxide solution Indicator Phenolphthalein solution Trial 1st reading 2nd reading 3rd reading Burette readings (cm3) Final ( ±0.1) 12.6 12.1 12.1 12.3 Initial ( ±0.1) 9.2 9.2 9.2 9.2 Volume used (titre) cm3 ( ±0.2) 2.9 2.9 I have not used as they are not concordant. I have used these reading for my mean titre. Mean titre (cm3) ( ±0.2) 2.9 + 2.9 = 5.8 5.8 à · 2 = 2.9 (mean titre) Volumetric calculations Volume of NaOH used = 2.9 cm3. Moles of NaOH n = CV V = 2.9 cm3 = 2.9 à · 1000 = 0.0029 dm3 n = 0.1 ÃÆ'- 0.0029 = 0.00029 mol So, moles of Aspirin will also be equal to 0.00029mol because the reaction ratio between NaOH and Aspirin is 1:1. Weighed out sample of Aspirin = 0.15 g How many grams of Aspirin reacted with NaOH? Aspirin = C9H8O4 g = n ÃÆ'- Mr = 0.00029 ÃÆ'- Mr [(12.01 ÃÆ'- 9) + (1.01 ÃÆ'- 8) + (16.00 ÃÆ'- 4)] = 0.00029 ÃÆ'- 180.17 = 0.052 g Percentage of Aspirin reacted = (0. 052 à · 0.15) ÃÆ'- 100 = 35% 7.1.4 Aspirin after 3rd recrystallisation Burette solution (cm3) 0.1 mol dm-3 sodium hydroxide solution Indicator Phenolphthalein solution Trial 1st reading 2nd reading 3rd reading Burette readings (cm3) Final ( ±0.1) 17.2 17.6 17.9 17.9 Initial ( ±0.1) 13.1 13.1 13.1 13.1 Volume used (titre) cm3 ( ±0.2) I have not used as they are not concordant. 4.8 4.8 I have used these reading for my mean titre. Mean titre (cm3) ( ±0.2) 4.8 + 4.8 = 9.6 9.6 à · 2 = 4.8 (mean titre) Volumetric calculations Volume of NaOH used = 4.8 cm3. Moles of NaOH n = CV V = 4.8 cm3 = 4.8 à · 1000 = 0.0048 dm3 n = 0.1 ÃÆ'- 0.0048 = 0.00048 mol So, moles of Aspirin will also be equal to 0.00048mol because the reaction ratio between NaOH and Aspirin is 1:1. Weighed out sample of Aspirin = 0.15 g How many grams of Aspirin reacted with NaOH? Aspirin = C9H8O4 g = n ÃÆ'- Mr = 0.00048 ÃÆ'- Mr [(12.01 ÃÆ'- 9) + (1.01 ÃÆ'- 8) + (16.00 ÃÆ'- 4)] = 0.00048 ÃÆ'- 180.17 = 0.086 g Percentage of Aspirin reacted = (0. 086 à · 0.15) ÃÆ'- 100 = 57% 7.1.5 Aspirin after 4th recrystallisation Burette solution (cm3) 0.1 mol dm-3 sodium hydroxide solution Indicator Phenolphthalein solution Trial 1st reading 2nd reading 3rd reading Burette readings (cm3) Final ( ±0.1) 21.3 20.9 21.0 21.1 Initial ( ±0.1) 16.9 16.9 16.9 16.9 Volume used (titre) cm3 ( ±0.2) 4.0 4.1 4.2 I have used these reading for my mean titre. Mean titre (cm3) ( ±0.2) 4.0 + 4.1 + 4.2 = 12.3 12.3 à · 3 = 4.1 (mean titre) Volumetric calculations Volume of NaOH used = 4.1 cm3. Moles of NaOH n = CV V = 4.1 cm3 = 4.1 à · 1000 = 0.0041 dm3 n = 0.1 ÃÆ'- 0.0041 = 0.00041 mol So, moles of Aspirin will also be equal to 0.00041mol because the reaction ratio between NaOH and Aspirin is 1:1. Weighed out sample of Aspirin = 0.10 g How many grams of Aspirin reacted with NaOH? Aspirin = C9H8O4 g = n ÃÆ'- Mr = 0.00041 ÃÆ'- Mr [(12.01 ÃÆ'- 9) + (1.01 ÃÆ'- 8) + (16.00 ÃÆ'- 4)] = 0.00041 ÃÆ'- 180.17 = 0.074 g Percentage of Aspirin reacted = (0. 074 à · 0.10) ÃÆ'- 100 = 74% 7.2 The data of melting points of different recrystallisation samples of Aspirin:- 7.2.1 Melting point after first recrystallisation Number of recrystallisation Temperature ( °C) ( ± 0.1 °C) Original melting point of Aspirin ( °C) Trial 1st reading 2nd reading 3rd reading Average 1 155.0 152.5 151.9 151.7 152.0 135.0 2 154.1 150.0 148.5 148.2 148.9 135.0 3 115.2 120.9 122.8 122.9 122.2 135.0 4 124.7 125.4 126.1 126.9 126.1 135.0 Original tablet 128.0 128.8 129.2 129.9 129.3 135.0 7.2.2 Graph showing the difference between melting points of Aspirin which was prepared and recrystallised in lab and melting of Aspirin from the data book Y-axis = temperature (in à ¢Ã‚ Ã‚ °C) X-axis = number of recrystallisations of aspirin samples prepared in lab and aspirin available in market 8. INTERPRETATION OF THE DATA I will now explain the results of melting point and titration. From the results of titrations we can see a trend flowing and how after each recrystallisation the sample gets purer. As the quantity of Aspirin decreased after each recrystallisation, the mass of Aspirin in that quantity was more compared to the previous recrystallisation. When compared to the original tablet which we get in the market, I could speculate that the producer has done almost four recrystallisations to get that purity of Aspirin. More pure Aspirin can be obtained if more recrystallisations are done. We could say that the difference in melting point might be higher because it might contain impurities like unreacted salicylic acid or other by-products of the reaction or decomposition products. We can see that the difference in the melting point is getting less as the number of recrystallisation increase and closer to the melting point of Aspirin published in the data booklet. Further evidence to my theory that the number of recrystallisations increases the purity is my melting point data. From my graph it can be seen clearly that as the number of recrystallisations increase the closer to the melting point of pure aspirin we get in the market. My data shows that the percentage purity of aspirin increased with each recrystallisation process. For example, after the first recrystallisation the percentage purity was only 22%, however when fourth recrystallisation was done the percentage purity was 74% showing a significant increase. This can be seen in the following graph:- 9. CONCLUSION In answer to my research question, How does the process of recrystallisation improve the purity of Aspirin? I have found significantly that the percentage purity increases with each recrystallisation and this is evident in my graph under the heading Interpretation of the data. Recrystallisation is an important technique in organic Chemistry. The general method is to find a solvent that dissolves the product more readily at high temperature than at low temperature, make a hot solution, and allow to crystallise on cooling. The crude product might contain; impurities which are insoluble in the solvent; impurities which are slightly soluble in the solvent; and impurities which dissolve readily in the solvent. The solvent itself has also to be removed or it behaves as an impurity in its own right. It must not leave behind any residue. One simple way to tell whether an organic compound is pure is to measure its melting (or boiling) point. A pure compound melts sharply: if impurities are present it melts slowly (over a range of temperature).  [11]   The process of recrystallisation in my experiment increased the purity of Aspirin but with a decrease in the quantity produced. The solid will readily dissolve in a larger quantity of solvent; the larger the volume of solvent the greater the loss of product  [12]  . This is the reason why after every recrystallisation I lose Aspirin. The process of recrystallisation removes the impurities present and this can be concluded from the fact that the difference between the melting point of the sample and the melting point of Aspirin from data booklet decreases with each recrystallisation. I could conclude that a pharmaceutical company should always have a balance between producing a very pure product, which means many recrystallisation processes and producing enough quantity of the product to make it a profitable industry. 10. EVALUATION 10.1 Random error The apparatus I used had uncertainties like the measuring flask has an uncertainty of  ±0.5cm3, the burette had an uncertainty of  ±0.1cm3 and the melting point apparatus also had an uncertainty of  ± 0.1 °C. This results in errors in my results. The equipment error could be reduced by using equipments with less error. For example, I could use a burette with an error of  ±0.05 cm3 instead of a burette with error of  ±0.1 cm3. 10.2 Systematic error In the process of titration there could a parallax error caused if the reading from the burette is not read at eye-level. So, when taking the reading from the burette, the level of the eye should be same as the level of the meniscus. When we are titrating different samples of recrystallisations the colour of the indicator changes from pale pink to dark and it is difficult to know the end-point of the titration process. 10.3 Modifications in the method of preparation of Aspirin and its recrystallisation I modified the method to improve it in the following ways: After each recrystallisation there was loss of Aspirin and the decrease in the mass of Aspirin limited the number of recrystallisations needed to get the most pure form of Aspirin. So, if I doubled the mass of reactants I can get doubled the mass of Aspirin produced and an increase in the number of recrystallisations. When I mixed salicylic acid and ethanoic anhydride solution in concentrated sulphuric acid it is hard to get the formation of a crystalline mush of Aspirin by agitating the flask. Hence, instead I used a magnetic stirrer which gives a uniform stirring and all the chemicals are mixed properly. I found this to be more effective at producing the mush. During the process of recrystallisation a lot of Aspirin is lost. When I used the filter paper, I cut it the same size as the Hirsh funnel. Instead I could have used a bigger filter paper in the funnel so that the impurities do not leak out of the edges of the filter paper and I could get a purer sample of Aspirin. When the Aspirin is left overnight to dry in an evaporating dish, there could be many contaminants which would get mixed in the Aspirin and if this is not taken into consideration in pharmaceutical industries then this could lead to serious health problems. Hence, the Aspiring should be covered when left overnight to dry. I could use different methods of purification of Aspirin like thin layer chromatography which is a sensitive and quick way of detecting impurities in an organic product (Aspirin). I could also use spectroscopy which provides a very good method for analyzing an organic compound. By comparing the infra-red spectrum for Aspirin with the spectrum of compound in a database I can check on its purity. 11. UNANSWERED QUESTIONS Unfortunately, not all my questions could be answered in this experiment. It would have been interesting in further researching and comparing more brands of Aspirin available in the market, if the producers just recrystallised the sample of Aspirin twice so that they do not lose a lot of their product in the process of recrystallisation or the producers actually tried to produce a pure sample of Aspirin ignoring the decrease in yield after each recrystallisation and considering the fact that this can affect the health of humans. When an organic compound has been made it needs to be purified, particularly if it is a  pharmaceutical chemical. This is because most organic reactions produce by-products but, even if the reaction is a clean one, the purity standards for many products are so stringent that small amounts of other compounds have to be removed. In particular the catalyst used in this reaction is concentrated sulphuric acid and must all be removed.

20,00 Leagues Under the Sea Essay -- essays research papers

My book starts out with a naturalist named Pierre Arronax. He’s a man that is fascinated by underwater life, and enjoys watching and studying underwater creatures. News spread worldwide about a serpent-like creature, part of the whale family, had been ramming ships and seeking them with ease. Pierre was very interested in this issue.   Ã‚  Ã‚  Ã‚  Ã‚  One day, while Pierre was staying the night in a hotel in Paris, he received a letter. The letter said that the American government was going to build a frigate to chase down and kill the sea monster. The letter also said that they would be more than happy to have him come along. Pierre and his trustworthy servant, Conseil, we’re going to attend this expedition. They packed up the belongings that were necessary, and then headed out to the dock to meet the ship, named the Abraham Lincoln. He gets aboard the ship, and the crew set sail to kill the monster.   Ã‚  Ã‚  Ã‚  Ã‚  On the ship they meet a Canadian harpooner, Ned Land. He is the one who is supposed to kill the monster when they find it. The crew goes on for about four weeks without finding any sign of the monster. Just as they are about to give up, Ned spots the monster! The monster proved to be 100 times faster than the Abraham Lincoln. After chasing the monster for a long period of time, they finally get close to the monster. They thought that maybe the creature was now sleeping, because it wasn’t running from them like the previous times. The monster seemed to be letting off a radiant glow in which nobody had seen before. The crew decides they are going to go for the kill. The men start firing guns at it, and start shooting different weapons trying to kill the beast. Nobody seemed to get close to hitting the beast, and if they were, it wasn’t effecting it. One elderly man steps up with his gun, and he decides that he is going to take a shot at it. The old man proves his marksmanship by hitting the beast dead on. The crew celebrated, but it still showed it wasn’t taking any effect. Ned Land steps up and decides to take a shot as well. He decides to try to create a serious injury to it. He grabs his harpoon, and he then takes the shot. Pierre saw the harpoon soar and then hit the monster, but it made a sound as if it had hit some kind of metal. The light from the animal then went out, and the object could be seen moving at the s... ...w life aboard the Nautilus. He was determined to escape.   Ã‚  Ã‚  Ã‚  Ã‚  Captain Nemo took them to many wonderful places. They experienced hunting and searching for pearls. They went to Viglo Bay, a hollowed out volcano, and the underwater city of Atlantis. Captain Nemo took them to the South Pole, where no man had ever been before. That made Captain Nemo the first person ever there. They almost died leaving the Great Ice Barrier. Then they also got in a fight with a giant squid! The only bad parts about their voyages were that Captain Nemo seemed to be seeking revenge on ships from his own country. He used the powerful Nautilus as a weapon to sink many ships. After ten months of being aboard the Nautilus, they completed their underwater exploration covering 20,000 leagues under the sea.   Ã‚  Ã‚  Ã‚  Ã‚  Later on, a maelstrom hit the Nautilus. The prisoners had then planned their escape. Professor Aronnax, Conseil, and Ned Land, already in the dinghy ready to escape, were thrown from the submarine. They then floated to safety, and returned to their homeland. The mystery remains. Nobody knows what happened to the Nautilus, and it’s infamous Captain Nemo.