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How much of the excess reactant will be left after the reaction is complete?
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- In the molecular weight determination by the Dumas method, several grams of an organic liquid was drawn into a bulb. The bulb was then immersed in a water bath at 87 degrees C and kept there until all the liquid was vaporized and the air in the bulb was replaced by the vapor. The tip was then sealed shut and the bulb removed from the vapor was 36.127g; the weight of the empty (evacuated) bulb was 35.427g; the bulb’s volume was 200.0mL; room temperature was 25 degrees C, and the barometric pressure was 720 mm Hg. Calculate the molecular weight of the organic liquid. Calculate the molecular weight of the organic liquid.Given the balanced reaction between salicylic acid (C7H6O3) and acetic anhydride (C4H6O3) to produce ASA or acetylsalicylic acid (C9H8O4) and acetic acid (C2H4O2), the following experimental materials are provided: 5.00 g of pure salicylic acid, 7.14 g of acetic anhydride and 8 drops concentrated sulfuric acid as catalyst. After successful synthesis, the group was able to collect 5.25 grams of acetylsalicylic acid. (Atomic weights: C= 12 amu; H = 1 amu; O= 16 amu; density acetic anhydride = 1.08 g/mL). What is the THEORETICAL yield of ASA in the experiment?Given the balanced reaction between salicylic acid (C7H6O3) and acetic anhydride (C4H6O3) to produce ASA or acetylsalicylic acid (C9H8O4) and acetic acid (C2H4O2), the following experimental materials are provided: 5.00 g of pure salicylic acid, 7.14 g of acetic anhydride and 8 drops concentrated sulfuric acid as catalyst. After successful synthesis, the group was able to collect 5.25 grams of acetylsalicylic acid. (Atomic weights: C= 12 amu; H = 1 amu; O= 16 amu; density acetic anhydride = 1.08 g/mL). What is the PERCENTAGE in the experiment?
- Given the balanced reaction between salicylic acid (C7H6O3) and acetic anhydride (C4H6O3) to produce ASA or acetylsalicylic acid (C9H8O4) and acetic acid (C2H4O2), the following experimental materials are provided: 5.00 g of pure salicylic acid, 7.14 g of acetic anhydride and 8 drops concentrated sulfuric acid as catalyst. After successful synthesis, the group was able to collect 5.25 grams of acetylsalicylic acid. (Atomic weight: C = 12 amu; H = 1 amu; O = 16 amu; density acetic anhydride = 1.08 g/mL). a. How much of the EXCESS reagent is left unused after the reaction? b. What is the PERCENTAGE in the experiment? c. What is the THEORETICAL yield of ASA in the experiment?Stoichiometric calculations. (show computations)K, a pharmaceutical scientist aims to synthesize paracetamol by reacting 3.075 mg of p-aminophenol and 2.25 milliliters of acetic anhydride to produce paracetamol and acetic acid. C6H7NO + C4H6O3 à C8H9NO2 + C2H4O2 Is the chemical reaction balanced? If yes, write YES. If not, what should be the balanced equation? What is the molecular weight of p-aminophenol? What is the molecular weight of acetic anhydride? What is the molecular weight of paracetamol? What is the limiting reactant? How many grams of paracetamol was formed? K was able to produce 1.88 grams of paracetamol. What is the percentage yield?IDENTIFICATION: Acetylsalicylic acid commonly known as Aspirin (C9H8O4) is used to treat fever, inflammation, and acts as a blood-thinning agent. A group of STEM students experimented on the synthesis of this compound using recrystallization technique. The following are the initial materials for the experiment: 5.00 g of pure salicylic acid (C7H6O3), 7.14 g of acetic anhydride (C4H6O3) and 8 drops concentrated sulfuric acid as catalyst. After successful synthesis, the group was able to collect 5.25 grams of Aspirin (C9H8O4) and acetic acid (C2H4O2). Atomic weights: C= 12 amu; H = 1 amu; O= 16 amu; density acetic anhydride = 1.08 g/mL How much of the excess reactant (in grams) will be left unconsumed after the reaction?
- A 0.9000-g of KIO3 is dissolved in 500-mL distilled water. A 50.0-mL aliquot portion was run down into an Erlenmeyer flask and 2-g of KI and 2-mL of 6M HCl were added to it. Directly after, the solution was titrated with a 24.80-mL Na2S2O3 solution to a faint yellow solution. Starch TS was added to the resulting solution and the titration with the Na2S2O3 solution continued wherein an additional 1.33-mL was required to bring the blue color of the solution to disappear completely. MW: KIO3 = 214.0 g/mol ; Na2S2O3 = 158.1 g/mol Compute the N of the Na2S2O3 solution. None of the choices 0.09657 N 0.1075 N 0.1017 NCan you calculate the limiting reagent, theoretical yield and% Reaction Yield shown using reaction stoichiometry? The calculations given in the benzalacetone synthesis experiment were the volume of 3mL of benzaldehyde, 1mL of acetone and the mass of dibenzalacetone 2.69g. With this data I calculated the other data shown in the table. Thank you! Psd.Where it says " Que deseas hacer?" in the photo that is the Benzaldehyde data.A 0.9134-g of KIO3 is dissolved in 500-mL distilled water. A 50.0-mL aliquot portion was run down into an Erlenmeyer flask and 2-g of KI and 2-mL of 6M HCl were added to it. Directly after, the solution was titrated with a 24.47-mL Na2S2O3 solution to a faint yellow solution. Starch TS was added to the resulting solution and the titration with the Na2S2O3 solution continued wherein an additional 1.33-mL was required to bring the blue color of the solution to disappear completely. MW: KIO3 = 214.0 g/mol ; Na2S2O3 = 158.1 g/mol Compute the M of the Na2S2O3 solution. 0.1047 M None of the choices 0.1107 M 0.09926 M
- The stock erythrosine B solution is 8.5 × 10-5 M. Calculate the volume of this solution that you must pipet into a 50-mL volumetric flask, which, when diluted to mark with deionized water, will give a final concentration of 1.7 × 10-5 M. Show your calculation setup.A 25 mL liquid bleach sample is diluted with water to 1000 mL in a bubble gel. 25 mL of the diluted sample is transferred to the flask with a pipette, excess KI is added to it, and thus OCl- ion turns into Cl- ion and I2 is formed. The released iodine is titrated with 0.09892 M Na2S2O3 using the starch reagent, and 8.96 mL is required for the endpoint. Find the % NaOCl (w/v; w/v) in the bleach sample. (Na=23 g/mol, O= 16 g/mol, Cl = 35.44 g/mol) (Warning: solving the necessary reaction equations by writing is necessary to see the stoichiometric relationship) A. 0.132% B. 0.264% C. 5.28% D. 10.56%1) The case study screenshot has been attached down below and the last sentence of the story is written down below and answer ques a,b,c which is written down below as well step-by-step. The last sentence of the case study is to save money and had been reducing monitoring, inspections, and maintenance. a) Use the following reaction to determine how much of each product would be released if 42 000 kg (42 tonnes) of methyl isocyanate reacted with excess water. This is the reaction methyl isocyanate + water -> 1,3-dimethyl urea + carbon dioxide b) Create a list of mistakes that led to the Bhopal disaster; you should be able to find at least eight. Evaluate the list of mistakes. Identify the three mistakes you think were most significant in causing the disaster, and justify your choice in a short (2-3 senstence) statement. c) What are some reasons it would have been safer to store the methyl isocyanate in smaller containers? Identify at least three reasons.