Please fill in the table ( for experimental values imaginary numbers can be used) Based on that can you calculate % yieldAtom economy Atom efficiency Experiment # 15Acid OrangeIntroductionDyes and pigments are among the earliest evidences of man's ability to takeadvantage of the chemical properties of materials. The range of man's chemicalcreativity is evidenced in early cave paintings, from the Han Purple used to color theTerracotta Army (210 BC), and the use of the purple dye derived from murexmollusks during the time of Alexander the Great. The first "modern" synthetic dyewas mauveine, discovered by William Henry Perkin in in 1856 when he was only 18years old, which he patented. His chemical discovery sparked the development ofthe chemical industry, fueled by the textile industry and coinciding with theindustrial revolution in mid-1800s London.In this lab, a diazo dye will be prepared. The first azo dye was chrysoidine or LondonYellow, made by coupling aniline to m-phenylenediamine, and has been used to dyewool since 1875. Diazo dyes are among the most widely-used synthetic colorants,with applications ranging from cosmetics to food coloring. Do you ever wonder whythe mac and cheese in Panda House looks very bright? It is because of Yellow #5 andYellow #6. Look up the structure of these two dyes and research their possibleeffects to human physiology.In this green experiment, the diazonium will be produced without the use of sulfuricacid, which as you already know, is highly corrosive. Production of the diazoniumion from an aryl amine requires a strong acid, in this case, the sulfanilic acid startingmaterial provides just that from its sulfonic acid (ArSO3H) functionality. No solventwill be used in the reaction except for a drop of water, and the purification will beaccomplished by washing off any remaining starting material with ethyl acetate.HONH2NaNO2+SO3HSO3HN=N-OHNaO3SyourProcedureSubstanceSulfanilic acid2-NaphtholNaNO2Acid OrangeMass (g)MW (g/mol)Mmol0.10.10.1Equivalents To a dry mortar and pestle add the three starting materials and gently mix thesolids. Do not pound dry nitrate salts as they pose a danger of explosion. Rather, usea circular motion to grind the materials. Add a very small drop of water using a glasspipette and then grind the materials slowly using circular motions to pulverize thecrystals for 10 min. Note any observations. You should obtain a wet powder. If youobtained a paste, you have added too much water and would have to let the productdry in air before proceeding.Add ethyl acetate (5 mL) to the dry powder and continue to grind to dissolve anyunreacted starting material. Assemble a vacuum filtration with a Hirsh funnelwetted with ethyl acetate. When you are ready, turn the vacuum on and transfer thereaction mixture using a glass pipette to the center of the filter paper. Use additionalethyl acetate (3 mL) to transfer the entirety of the product from the mortar, as wellas to wash the product. Discard the filtrate in the organic waste bottle and let theprecipitate air-dry for 15 min. The product is water soluble and somewhathygroscopic, avoid its exposure to humidity.Weigh the solids to obtain the percent yield and determine its melting point. Notebe that although the product was purified of the organic starting materials by the ethylacetate wash, there may be unreacted sodium nitrite left. For the purposes of thislab, we will assume that all of the nitrite reacted. However, to fully purify theproduct, the dye may be washed with saturated sodium chloride solution followedby cold methanol.guir CharacterizationObtain a UV-Vis spectrum of your product by dissolving 10 mg Acid Orange in 100mL distilled water using a volumetric flask. Calculate the molarity of this solution.Next, take 10 mL of this solution and dilute it with 100 mL of water using avolumetric flask. Transfer the solutions in labeled beakers so others may use thevolumetric flask. Use M1V1= M2V2 to calculate the concentration of the secondsolution.Follow instructions on how to run the UV-Vis spectrometer. Briefly, run a blanksample in water. Place your sample in a cuvette using a pipette. The reading on they-axis must be between 0.2 - 1.0 absorption units, otherwise your sample is toodilute or concentrated. Note the maxima of the peaks observed, both in wavelengthand absorption units (A). Calculate the molar absorptivity at the maximumwavelength (max) by using Beer's Law equation, & = A*b*cwhere & is the molar absoprtivity, A is the absortion, and c is the molarconcentration. Of course, more than one concentration must be measured to get anaccurate result. For the purposes of this lab, a single measurement will suffice. Printyour spectrum and this attach to your laboratory report.

Question

Please fill in the table ( for experimental values imaginary numbers can be used) Based on that can you calculate % yieldAtom economy Atom efficiency Experiment # 15Acid OrangeIntroductionDyes and pigments are among the earliest evidences of man's ability to takeadvantage of the chemical properties of materials. The range of man's chemicalcreativity is evidenced in early cave paintings, from the Han Purple used to color theTerracotta Army (210 BC), and the use of the purple dye derived from murexmollusks during the time of Alexander the Great. The first &#34;modern&#34; synthetic dyewas mauveine, discovered by William Henry Perkin in in 1856 when he was only 18years old, which he patented. His chemical discovery sparked the development ofthe chemical industry, fueled by the textile industry and coinciding with theindustrial revolution in mid-1800s London.In this lab, a diazo dye will be prepared. The first azo dye was chrysoidine or LondonYellow, made by coupling aniline to m-phenylenediamine, and has been used to dyewool since 1875. Diazo dyes are among the most widely-used synthetic colorants,with applications ranging from cosmetics to food coloring. Do you ever wonder whythe mac and cheese in Panda House looks very bright? It is because of Yellow #5 andYellow #6. Look up the structure of these two dyes and research their possibleeffects to human physiology.In this green experiment, the diazonium will be produced without the use of sulfuricacid, which as you already know, is highly corrosive. Production of the diazoniumion from an aryl amine requires a strong acid, in this case, the sulfanilic acid startingmaterial provides just that from its sulfonic acid (ArSO3H) functionality. No solventwill be used in the reaction except for a drop of water, and the purification will beaccomplished by washing off any remaining starting material with ethyl acetate.HONH2NaNO2+SO3HSO3HN=N-OHNaO3SyourProcedureSubstanceSulfanilic acid2-NaphtholNaNO2Acid OrangeMass (g)MW (g/mol)Mmol0.10.10.1Equivalents To a dry mortar and pestle add the three starting materials and gently mix thesolids. Do not pound dry nitrate salts as they pose a danger of explosion. Rather, usea circular motion to grind the materials. Add a very small drop of water using a glasspipette and then grind the materials slowly using circular motions to pulverize thecrystals for 10 min. Note any observations. You should obtain a wet powder. If youobtained a paste, you have added too much water and would have to let the productdry in air before proceeding.Add ethyl acetate (5 mL) to the dry powder and continue to grind to dissolve anyunreacted starting material. Assemble a vacuum filtration with a Hirsh funnelwetted with ethyl acetate. When you are ready, turn the vacuum on and transfer thereaction mixture using a glass pipette to the center of the filter paper. Use additionalethyl acetate (3 mL) to transfer the entirety of the product from the mortar, as wellas to wash the product. Discard the filtrate in the organic waste bottle and let theprecipitate air-dry for 15 min. The product is water soluble and somewhathygroscopic, avoid its exposure to humidity.Weigh the solids to obtain the percent yield and determine its melting point. Notebe that although the product was purified of the organic starting materials by the ethylacetate wash, there may be unreacted sodium nitrite left. For the purposes of thislab, we will assume that all of the nitrite reacted. However, to fully purify theproduct, the dye may be washed with saturated sodium chloride solution followedby cold methanol.guir CharacterizationObtain a UV-Vis spectrum of your product by dissolving 10 mg Acid Orange in 100mL distilled water using a volumetric flask. Calculate the molarity of this solution.Next, take 10 mL of this solution and dilute it with 100 mL of water using avolumetric flask. Transfer the solutions in labeled beakers so others may use thevolumetric flask. Use M1V1= M2V2 to calculate the concentration of the secondsolution.Follow instructions on how to run the UV-Vis spectrometer. Briefly, run a blanksample in water. Place your sample in a cuvette using a pipette. The reading on they-axis must be between 0.2 - 1.0 absorption units, otherwise your sample is toodilute or concentrated. Note the maxima of the peaks observed, both in wavelengthand absorption units (A). Calculate the molar absorptivity at the maximumwavelength (max) by using Beer's Law equation, & = A*b*cwhere & is the molar absoprtivity, A is the absortion, and c is the molarconcentration. Of course, more than one concentration must be measured to get anaccurate result. For the purposes of this lab, a single measurement will suffice. Printyour spectrum and this attach to your laboratory report.

Accepted Answer

This answer is given below.Explanation: