Collected Lab Data Density of 3,3-dimethyl-1-butene (g/mL) Volume of 3,3-dimethyl-1-butene (μL) Mass of empty conical vial (g) Mass of empty conical vial + product (g) Mass of product (g) Percent yield (%) Boiling point of product (°C) Is your collected product, 3,3-dimethyl-1-butanol? 0.650 150. 22.991 23.099 0.108 110.77 145.0 Yes, but slightly impure
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Please help give the correct percent yield with the correct amount of significant digits.
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- O Search Animations Slide Show Review View Help & Viewing v Share A A A ... halla Identify primary / secondary / tertiary alcohols CH5 H, H2 H -C- H2 -CH3 H,C- C-C CHH,C H2 С —СН. H;C- OH OH H. R-C-OH R-C-OH R, -HO- H 10 primary alcohol 20 secondary alcohol 30 tertiary alcohol Help Improve Office Notes cohols.pptx -. scroll pause f6 f7 f8 f9 f10 f12 m breakHg(OAc)2, H20 -CH3 NABH4 Hg(OAc)2, H20 NABH4 BH3 H202 CH3 THE OH" PHCO3H CH2CI2 (solvent) Cl2Please describe the primary reason for the different solubilities of the alcohols in the table below: Formula Name Solubility in H2O (g/100g) CH3OH Methanol infinitely soluble CH3CH2OH Ethanol infinitely soluble CH3(CH2)2OH Propanol infinitely soluble CH3(CH2)3OH Butanol 9 CH3(CH2)4OH Pentanol 2.7 CH3(CH2)5OH Hexanol 0.6
- Curved arrows are used to illustrate the flow of electrons. Using the provided starting and product structures, draw the curved electron-pushing arrows for the following reaction or mechanistic steps. Be sure to account for all bond-breaking and bond-making steps. H Na → Select to Add Arrows acetone/ water H I :I: :6: Na Ⓒ H :CI:O acetone/water Please select a drawing or reagent from the question areaYou begin the reaction with 6.5 mL of t-butyl alcohol (density= 0.775 grams/mL) and 15 mL of concentrated HCl (1.189 grams/mL, 38% HCl) in a distillation flask. Calculate the limiting reagent and the theroretical yield of the product (t-butyl chloride) for this reaction. (Hint:Your starting amount of HCl is 38% of the starting smount).1-butanol yields 1-bromobutane in the presence of concentrated sulfuric acid and an excess of sodium bromide. CH3CH2CH,CH2OH (I) → CH3 CH2CH2CH2Br (1) If 13.55 mL of 1-butanol produced 13.23 g of 1-bromobutane, the percentage yield of the product equals: (Assume the density of 1-butanol is 0.81 g/mL, the molar mass of 1-butanol is 74 g/mol, and the molar mass of 1-bromobutane is 137 g/mol.) %
- 1. 250.0 g each of toluene (CoHsCH:) and benzene (CsHs) are mixed together. Answer the following questions. C&H6 C6HSCH3 Compound M (g/mol) Kr (°C/m) | TP (°C) | Kb(C/m) 5.12 7.27 78.108 93.142 5.55 -95.0 2.53 3.29 To (°C) 81.1 110.7 (a) In this solution, which is the solute and which is the solvent? (b) What is the freezing point of this solution, in °C? (c) What is the boiling point of this solution, in °C? (d) Calculate the osmotic pressure of this solution in kPa. Assume that the masses are additive and the density of the final solution at 25°C is 0.867 g/mL.Experimental procedure. Be sure to wear gloves throughout this reaction. Place a magnetic stir bar, 2.0 g of trans- stilbene, and 40 mL of ethanol in a 125-mL Erlenmeyer flask. Note the shape and color of the crystals in your lab notebook. Clamp the flask in place on a magnetic stir/heat plate. With heating and stirring, dissolve the trans-stilbene. Be careful not to heat too quickly. Add 4.0 g of pyridinium tribromide. If solid material adheres to the interior walls of the flask, use a little ethanol to rinse it down. Heat with stirring for 5 minutes after the addition of reagents is complete. Remove the flask from the hot plate. Use caution to avoid getting burned by the hot flask. The product should quickly begin to precipitate or crystallize. Let the reaction mixture cool to room temperature. Chill the mixture in an ice bath. Collect the product by vacuum filtration in a pre-weighed fritted funnel or fritted crucible. Alternatively, use a ceramic Büchner funnel and filter paper. If…b) Will the sample be contaminated with any of the impurities? Calculate the percent purity of the initial sample (in terms of compound A) - ( i.e. express the amount of compound A in the initial sample as a percentage of the mass of initial sample). Calculate the percent purity of the final sample (in terms of compound A) - (i.e. express the amount of compound A in the final sample as a percentage of the mass of final sample). Did the recrystallization procedure result in an increase of the percent purity of compound A in the sample? Comment on the results.
- Concentration of Reagents (NH4)2S2O8 KI Na2S2O3 0.25 M 0.22 M 0.19 M Volumes of Solutions S₂082 (mL) Starch soln (mL) KNO3 (mL) EDTA soln (mL) KI (mL) S₂O32- (mL) x 5 9.7 0.9 26.4 0.5 9.9 1.1 Using the above data determine the concentration of I at the moment the reaction begins. HINT: This is a mixing problem. Determine the total number of moles of I and divide this amount by the total volume (in L). Be careful... If you go back and try this exercise again the values will change. Read the question carefully! Answer:Rank a series of molecules by expected solubility in water based on polarity and hydrogen bonding. Some slightly soluble compounds are included in this exercise. Rank the organic compounds from most soluble to least soluble. To rank items as equivalent, overlap them. View Available Hint(s) Reset Help Η Η Η Η H H H H ннно Н-С-С — С —С— ОН Н-С-С-С —С -Н Н-С—С—С — С -ОН Η Η Η Η Η Η Η Η Η Η Η нн Η Η Н-С—С— О—С—С — Н нн нн Most soluble Least solubleCyclohexanol 10 ml Mass of cyclohexanol 9.62 g – 0.053 mol Theroretical yield cyclohexene–7.89g - ? mol Therotical mass of cyclohexene- Actual yield- 6.8ml –4.055 g –? mol Percent yield- 51.04% Boiling point of cyclohexene -83 degree Celsius Theroretical boling point -83 degree Celsius can i get some clarification pls