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Consider the following reaction and decide whether acetic acid is a suitable solvent. Show your work by drawing the reaction of acetic acid with each reactant and determining the direction of equilibrium quantitatively.
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- 1) Hydrolysis of Methyl Salicylate: Methyl Salicylate (C8H8O3) + sodium Hydroxide (NaOH) -> sodium Salicylate ( NaC7H5O3) + Methanol (CH3OH) 2) Acidification of Sodium Salicylate: Sodium salicylate (NaC7H5O3) + HCL -> Salicylic acid (C7H603) + sodium chloride (NaCL) Could you find the theoretical yield for me? 2.15g of methyl salicylate was used. 25ml of sodium hydroxide (2m solution) was used for hydrolysis and 2ml of hydrochloric acid was used for the acidification. This produced a yield of 1.53g of salicylic acid.Which 9.26 g of an unknown solid is dissolved in a coffee cup calorimeter that contains 62.0 mL of water. The measured temperature increased from 23.4 °C to 24.7 °C. The specific heat of water is 4.184Jg-1°C-1, and assume the density of the solution is 1.00 g mL-1. Calculate the molecular weight of the unknown solid if the ΔrH was determined to be -2.51kJmol-1 via another experiment.Calculate the percent yield and theoretical yield for the following reaction: oxidation of cyclododecanol to cyclododecanone. 0.2093 grams of Cyclododecanol 0.5 mL of acetone 0.20 mL of Glacial acetic acid 2.0 mL of bleach Final weight of cyclododecanone = 0.0578 g
- 1. Based from the given problem, What is the molecular weight of the tartaric acid (C4H6O6)? 2. Based from the given problem, What is the meq of the tartaric acid (C4H6O6)? 3. Based from the given problem, What is the percentage purity of the tartaric acid (C4H6O6)?Calculate the moles of the limiting reagent for the following reaction: oxidation of cyclododecanol to cyclododecanone. 0.2093 grams of Cyclododecanol 0.5 mL of acetone 0.20 mL of Glacial acetic acid 2.0 mL of bleach Final weight of cyclododecanone = 0.0578 gAcetanilide (C6H5NHCOCH3, M = 135.2) can beprepared from aniline (C6H5NH2, M = 93.1) and aceticanhydride ([CH3CO]2O, M = 102.1) according to thebalanced equation below. C6H5NH2 + (CH3CO)2O →C6H5NHCOCH3 + CH3COOH If 10.0 g acetanilide is isolated from the reaction of 10.0g aniline with 10.0 g acetic anhydride, what is the percentyield of the reaction?
- (a) benzene can potentially react with Lewis acid to form new carbon-carbon bond. Propose the starting material and stepwise mechanism to produce new chemical structure which consists of a formula molecule of C11H16.formation of tetraphenylnaphthalene Amount of tetraphenylcyclopentadienone: 0.530 g Volume of glyme: 3 mLVolume of isoamyl nitrite: 0.75 mL anthranlic acid: 0.253 g tetraphenylnaphthalene: 1.25 g theoretical yield: percent yield:Calculate the % yield of the following reaction. You have isolated 1.5g of benzil from the reaction of 1.95 of b enzoin and 1.0 g of ammonium nitrate A.75.5% B.77.6% C78.1 %
- The amount of tartaric acid is responsible for the tartness of wine and controls the acidity of the wine. Tartaric acid also plays a very significant role in the overall taste, feel and color of a wine. Tartaric acid is a diprotic organic acid The chemical formula for tartaric acid is C4H6O6 and its structural formula is HO2CCH(OH)CH(OH)CO2H. A 50.00 mL sample of a white dinner wine required 21.48 mL of 0.03776 M NaOH to achieve a faint pink color. Express the acidity of the wine in terms of grams of tartaric acid, H2C4H4O6 (M. M. = 150.10) per 100 mL of wine. Assume that the two acidic hydrogens are titrated at the end point. MM H2C4H4O6 = 150.10 MM NaOH = 40.00 Below is the balanced chemical equation for this titration.How many grams each of resorcinol and hexachloro-phene should be used in preparing 2 pounds of an acne ointment that is to contain 2% resorcinol and 0.25% of hexachlorophene?Methanogenic bacteria convert acetic acid (CH3COOH) to CO2(g) and CH4(g). ΔH°f, (kJ/mol) ΔG°f, (kJ/mol) CH3COOH -484.5 -389.9 CO2(g) -393.5 -394.4 CH4(g) -74.8 -50.8 Calculate ΔH°rxn. ΔH°rxn = ____ kJ Calculate ΔG°rxn. ΔG°rxn = ___kJ