FAH207H1 Final: Exam Study Notes - Lectures 6 to 12

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champagnealpaca141

12 Apr 2011

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Lecture six - eight: greek ceramics and vase painting from geometric to. Greek pottery: ceramics is derived from the greek word for clay (keramos), potters were called. Protogeometric (1000 - 900 bce: the only surviving material from the protogeometric period is pottery, with. Mycenaean shapes and decorations applied in few geometric patterns/lines applied with a "multiple brush" Geometric as a aristocratic reaction to incipient social instability in the 8th century. Geometric amphora from dipylon cemetery, athens (c. 750 bce) Ekphora (procession from the house to the cemetary) Important public displays of wealth and social status by an aristocrat. Olpe vase in proto-corinthian animal style, corinth (c. 650-625 bce: proper use of the "black-figure technique" (black figure silhouettes with incision with red-white detailing added later with paints, small scale and precise detailing (repetitive figures) Achilles and ajax amphora, athens (c. 540-530 bce) exekias. Attic bilingual amphora, athens (c. 520 bce) andokides.

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Part 1: The Paint Shop (20 points)

The Rookery Company, a large financial services organization,owns and occupies many facilities including a property that islisted on the National Register of Historic Places. Rookerymaintains a Paint Shop. The Paint Shop employs a dozen peopleincluding painters who are especially skilled.

Department executives in the various divisions of Rookery havethe decision rights regarding the choice of painters they engage.At Rookery, it has never been the case that all painting is done bythe in-house Paint Shop. Over the years outside paintingcontractors have been hired in various circumstances. For example,outside contractors were brought in for some major projects andwhen the Paint Shop was overwhelmed or not equipped to tacklejobs.

The Paint Shop is organized as a profit center as are all of theunits of Rookery that would engage the Paint Shop to providepainting services. When a department needs painting work, they cancontact the paint shop for an estimate. If the Paint Shop contractsto do the work, Rookeryâs accounting department charges an expenseagainst the profit of the department requesting the work andcredits the revenue of the Paint Shop. The Paint Shop is a captivesupplier, that is, the paint shop does not do work for anycustomers outside of the Rookery Company.

Department heads have not always been pleased with theturn-around times of the in-house Paint Shop. Also, some in-housecustomers have been displeased with the price charged and theattitude of some of the staff members in the Paint Shop. As aresult, department heads have increasingly been turning to outsidepainters instead of using the Paint Shop.

The CFO noticed the falling revenues and the resulting fall inprofits of the Paint Shop. They are a high fixed cost unit. Inresponse the CFO sent memos to the department executives who havedecision rights over painting contracts to strongly urge them toalways give the Paint Shop the ârightof-first-refusalâ wheneverpainting work needs to be done.

The CFO is a strong supporter of the Paint Shop and believesthat Rookery needs to maintain the inhouse paint shop. However, hisrepeated requests to the department executives to use the PaintShop have not succeeded in creating work. To be candid, many jobsare being out-sourced to independent contractors and it appearsthat the CFOâs memos are being ignored. In fact, the Paint Shopâsrevised pricing structure necessitated by the need to raise pricesto improve their bottom line has only aggravated theirsituation.

The CFO is angry. At best he feels ignored, at worst he regardsthe decision of Rookery units to use outside painters as a disloyalact. But, the CFO lacks authority to require the departmentalexecutives to use the Paint Shop. If he had the authority, he wouldrequire every department within the company to use the Paint Shopunless he decides that for some reason the Print Shop is not ableto do the work.

To put an end to the practice of Rookery units selecting outsidepainting contractors, the CFO has recently communicated to theoutside painting contractors who have been doing most of the workfor Rookery units. He indicated that he does not want the outsidecontractors to accept painting work from any Rookery departmentthat he has not authorized. Of course, the CFO will not authorizeany work to go to outside contractors unless the Paint Shop isunable to complete the work.

The consequence to an independent contractor of performing worknot authorized by the CFO as outlined by the CFO is that whenRookery does need to employ an outside contractor for a majorproject the CFO will remember those who are his friends and thosewho did cooperate with his wishes. Of course, the CFO has access toall invoices making it a simple task to identify any who do notcomply with his wishes.

Required:

1. (10 points) Speculate on why the department heads areignoring the CFOâs wishes with regards to using the services of thePrint Shop.

2. (10 points) When the volume of work declined at the PaintShop, to maintain profitability the Paint Shop increased bidprices. The increase in bid prices resulted in further decreasingthe number of jobs the Paint Shop was winning and the spiralcontinued downwards. This is an illustration of what some refer toas the âdeath spiral.â What other responses could the Paint Shop incollaboration with the CFO have made to feedback received withinthe management control system when the Paint Shop was no longercompetitive with outside contractors? Also, speculate on why itseems to be the case that the leadership of the Paint Shop did notinitiate any of the responses you discussed. Be certain to give acomprehensive response.

What element they are:

1.My appearance at standard state is a silvery-white. My density when I melt is 1.46g/cm3. I burn purple, and react violently on contact with water. I see use in atomic clocks, and sometimes in glass

2.I am a diatomic molecule with a melting point of -259.14ËC and have a lower density than any other element.I am highly flammable and commonly form compounds with non-metals and halogens.I am commonly found in a product used to clean wounds and am one of the main elements involved in making stars shine

3.I am Silver-White in colour and I am so reactive I must be stored in oil.You may find me colouring glass windows in a church or reacting with water or acids to form hydrogen gas.I also oxidize and produce a film which tarnishes my Silver-White skin and can be used with other metals to form alloys

4.My soluble compounds are toxic to mammals yet I am used in paint, I am a soft but highly reactive metal. I am used in medical imaging but I am non-radioactive.

5.I am a poor conductor of heat or electricity, and my boiling point is at 536F.I am used as a fertilizer for soil and I help extinguish fire from common combustible, liquid, gas and electricity.

6.I get my name from the greek word meaning âmoonâ.I have 6 natural isotopes.I am protective against mercury poisoning, and my salt is used to control dandruff

7.I am a solid crystal yellow at room temperature. My melting point is , and I donât dissolve in water I react with most elements when heatedI am famous for burning in air and producing a blue flame.I prevent rubber materials from melting, as they get warmer. I am also used to treat acne

8.I am useful inside the body and outside the body I help heal wounds. My boiling point is 184 degrees and my name is derived from my colour. A crystalline solid that gives off a coloured gas on heating and can be found in most seaweed

9.My alloy will chill out cast iron and colour ceramics. I can strengthen lead or make acids more corrosive. Some of my amino acids are fun guys but can be harmful in large groups.

10.I'm part of the p block, my standard state is a solid.â¨I'm a post transition metal, I'm silvery white in colour.â¨When evaporated i can produce a mirror as reflective as silver, my name means violet.

Hi, I am not well at all, and need to submit this lab as soon as possible and am busy with alot of other stuff too. Please help with it. Will be really thankful and would rate good.

Introduction

Decomposition of Sodium Chlorate Mass, Moles, and the Chemical Equation

Sodium chlorate is used as a source of oxygen in emergency oxygen generators. So- called oxygen canisters or oxygen candles are found on airplanes, submarines, even the space station â anywhere oxygen might be in short supply in case of an emergency. Sodium chlorate decomposes upon heating or in the presence of metals to give oxygen gas. What is the chemical equation for the decomposition of sodium chlorate?

Concepts

ï· Moles ï· Balanced chemical equation

ï· Molecular formula ï· Stoichiometry

Background

Sodium chlorate, NaClO₃, is a colorless, odorless, white solid that melts at 248 Â°C. When heated above 300 Â°C, it begins to lose oxygen. The ultimate products of the thermal decomposition of sodium chlorate are oxygen gas and a white solid. Based on the molecular formula of sodium chlorate, three possible reactions will account for the loss of oxygen gas upon heating (Equations 1-3). Note that equations 1-3 are not balanced.

Equation 1 2NaClO₃(s) â 2NaClO₂(s) + O₂(g)

Equation 2 NaClO₃(s) â NaClO(s) + O₂(g)

Equation 3 2NaClO₃(s) â 2NaCl(s) + 3O₂(g)

What is the actual chemical equation for the thermal decomposition of sodium chlorate? All of the possible sodium-containing products n Equations 1-2 are real compounds: sodium chlorite, NaClO₂; sodium hypochlorite, NaClO; and sodium chloride, NaCl. All are white solids at room temperature. It is possible to determine the chemical equation for the decomposition of sodium chlorate by applying the principles of stoichiometry to the masses of the reactants and products.

Safety Precautions:

Sodium chlorate is a strong oxidizing agent and a dangerous fire risk; it is slightly toxic by ingestion. Contact with metal powders or combustible organic compounds may cause fires. Keep away from contact with organic materials, including rubber stoppers, rubber tubing, etc. Avoid contact with eyes and skin. Do NOT dispose of exess sodium chlorate in the trash.

When heating sodium chlorate, use only a small amount of solid (0.25-0.40 g) in a Pyrex test tube. Inspect the test tube for chips and cracks before use and handle the test tube using a test tube clamp. Distribute the solid evenly along the bottom of the test tube and heat the test tube clamp. If any smoke is produced, remove the test tube from the flame until the reaction subsides. Do not inhale the smoke. Allow the test tube to cool completely on a wire gauze with a ceramic, heat-resistant center. Wear chemical splash goggles and chemical-resistant gloves and apron.

Procedure:

Measure all masses to the nearest 0.01 g and record all data in the data table.

Obtain two medium test tubes. Label them 1 and 2.

Measure and record the mass of each test tube.

Using a spatula, add approximately 0.2-0.4 g of sodium chlorate to the bottom of each test tube.

Measure and record the combined mass of each test tube and sodium chlorate.

Place test tube #1 in a test tube clamp. Holding the test tube in an almost horizontal position, gently tap the test tube to distribute the solid sodium chlorate evenly along the bottom one-third of the test tube.

Light a Bunsen burner.

Holding test tube #1 with the test tube clamp, slowly move the test tube back and forth through the burner flame to gently heat the solid. The solid should begin to melt and bubble slightly. Caution: Do not aim the opening of the test tube at anymore.

Quickly remove the test tube from the flame if a white smoke is given off from the open end of the test tube. The smoke represents a loss of starting material due to evaporation of molten sodium chlorate and will reduce the yield of product. A small amount of smoke may be inevitable and should not interfere with the accuracy of the results.

Continue to heat the test tube in the burner flame until no more bubbling is observed and the material in the test tube has solidified.

Allow the test tube to cool completely on a wire gauze with a ceramic center.

While test tube #1 is cooling, repeat steps 5-11 sing test tube #2.

When test tube #1 has cooled to room temperature, measure the combined mass of the test tube and its solid contents.

Reheat test tube #1 gently for an additional three minutes.

Cool the test tube on the wire gauze until it is room temperature. Measure the mass a second time. If the second mass differs from the first mass by more than 0.02 g, repeat the heating cycle a third time.

Repeat steps 13-15 using test tube #2.

Data Table:

Trial 1

Weight of beaker --- 68.1887g

Weight of test tube -- 19.3538g

Weight of NACLO3 -- 0.3341g

Everything together -- 87.9155g

1st time burning:-- 87.8851g

2nd time burning:-- 87.7630g

3rd time burning:-- 87.7626g

Trial 2

Weight of beaker --- 68.1886g

Weight of test tube -- 22.8518g

Weight of NACLO3 -- 0.3154g

Everything together -- 91.3508g

1st time burning:-- 91.2078g

2nd time burning:-- 91.2103g

Post-Lab Calculations and Analysis:

1) For each trial, find the initial mass of sodium chlorate and calculate the number of moles of sodium chlorate.

2) Based on the molar masses of the three possible solid products in Equations 1-3, and the number of moles of reactant in each case, calculate the expected masses of the three possible products for Trials 1 and 2.

3) Compare the actual mass of product obtained in Trials 1 and 2 with the calculated or expected masses. What is the balanced chemical equation for the decomposition of sodium chlorate? Explain.

4) Use the following equation to determine the percent error in the mass of solid obtained.

â (actual mass â expected mass) / expected mass

5) Consider the following potential sources of error in this experiment. Explain whether they would have caused the actual mass of solid product to be lower or higher than the expected value.

a)The sodium chlorate did not decompose completely.

b)The sodium chlorate was heated too fast, allowing considerable white smoke to escape from the test tube.

c)The sodium chlorate absorbed some moisture from the air before the experiment began and was not completely dry.

FAH207H1 Final: Exam Study Notes - Lectures 6 to 12

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