Electrophilic Aromatic Substitution – Nitration of Bromobenzene

questions 1,2, and 3 only pls disregard the experiment results

only the questions pls disregard the experiment results thank you

Answer last 3

What factors during the experiment caused the percent yield to be different than 100%? What impurities may be present in the final product (look at the spectroscopic data for evidence of this), and how does that effect the percent yield calculation? I got 64% for the percent yield.

How do we detect organic compounds and inorganic compounds used in GC analysis?

Write the reaction involved in Ferrox Test. What is the species responsible? Why is phenol negative in Ferrox Test?

35-38. Ethanol is freely soluble in water, but ethane is insoluble. Using principles of Нн Н-С-С-н Н-С-С-О: нн intermolecular forces describe... 35. ...what is needed for a solute to dissolve in a solvent. нн ннн ethane ethanol 35. ...why ethanol dissolves in water. 36. . why ethane does not dissolve in water. ... 38. Draw the IMF that is formed between water and ethanol.

Answer the question below directly. Why methanol is a good solvent for UV but not for IR?

I need answer within 20 minutes please please with my best wishes

b. When added to an immiscible mixture of dichloromethane and water, which layer would you expect the following compounds to primarily be found in? Explain. i. limonene CH3 CH3 CHM 2070 Lab Fall 2020 ii. acetic acid HOCH3 i. benzaldehyde

Question 6 Question 6-1: Aromatic ethers can lose a neutral alkene molecule during fragmentation in a mass spectrometer as shown in Figure 6. What is the structure of the alkene formed by phenyl ethyl ether? [Give a SMILES notation.] Your answer Figure 6 H Your answer 0 Question 6-2: The loss of the alkene generates a fragment that registers the base * peak in the mass spectrum. What is the m/z value of the base peak?

A common lab experiment is the dehydration of cyclohexanol to cyclohexene. Explain why mass spectrometry might not be a good way to distinguish cyclohexene from cyclohexanol.

The unknown organic substances which were critric acid, acetone, urea, beazaldehyda, glycerol, and MTBE was done in an experiment- use this to answer the questions. (Note: there was no boiling point or melting point done in this experiment however their reaction to NaHCO3 was done)   a)Compare what you originally expected to identify at each step of the flow chart to what you identified. Were your predictions close to what you expected? Elaborate on your response. b)What was the biggest challenge you faced in differentiating between the functional groups? Were there any that were difficult to distinguish between? Why? b) Do you think this flow chart could be used to identify functional groups in a molecule that contains multiple different functional groups? Discuss. And how would you improve this flow chart procedure to better identify the organic compoun? (Flow Chart Below)

A mixture of tert-butylbenzene and acetophenone is adsorbed onto a silica gel chromatography column and eluted with a moderately polar solvent such as dichloromethane. Match each statement to the appropriate category. least polar tert-Butylbenzene elutes first most polar elutes last Answer Bank Acetophenone

A student use the same protocol as in the lab manual to extract 4 chloroanilline, benzoic acid and naphthalene. Below are the steps he took Step 1 - Dissolve all three in 15 ml ether and place in separatory funnel Step 2- Add 15 ml of hydrochloric acid and mix well Step 3 - Isolate the aqueous layer and add sodium hydroxide which resulted in a precipitate Step 4- Add 15 ml of sodium carbonate to the ether layer and mix Step 5- Isolate the aqueous layer and add hydrochloric acid, which resulted in a precipitate. Step 6- dry the ether layer and collect the solid that is left

To determine the purity of a synthetic preparation of methylethyl ketone, C4H8O, it was reacted with hydroxylamine hydrochloride, liberating HCl (reaction: NH2OH.HCl + C4H8O -> C4H9NO + H20 + HCl). In a typical analysis a 3.00-mL sample was diluted to 50.00 mL and treated with an excess of hydroxylamine hydrochloride. The liberated HCl was titrated with 1.2149 M NaOH, requiring 35 mL to reach the end point. A. Write the acid base reaction involved in the titration. B. Report the percent purity of the sample given that the density of methylethyl ketone is 0.805 g/mL.

only do number 4 please

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In IR absorption spectra of a compound, strong absorptions at 3300 cm and 2100 to 2260 cm were observed. What functional group might the compound contain? a. Alkyne b. Alkene с. Alcohol d. Carboxylic acid

Electronic cinfiguration of carbon

True or False1. When FeCl3 is used in visualizing aspirin in thin layer chromatography, the resulting spot is red in color 2. Chlorination of phenol occurs even if the reagent AlCl3 is missing3. The molecule 2,4,6-trinitrophenol, being a phenolic compound, tests positive for the FeCl3 test

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1. What should you do if H;SO4 contacts your skin? pyright Cata Education 220 2. When should you stop the distillation process for this procedure? 3. With 85 % H;SO, by volume in water being used in the reaction, how many moles of water will be added to the reaction when 1.25 mL of 85 % H;SO, is added? 4. What peaks in the IR spectrum would indicate the loss of 1-hexene and the formation of 2-hexanol?

Which compounds are water soluble? find the attached file ?

An analyst was told to determine the amount of glucose in blood using a colorimetric method. The analyst prepared a series of standards containing known amounts of glucose and obtained the results given in the table below by UV/visible spectroscopy. Concentration of Glucose/mmol L-¹ 0.0 2.0 4.0 6.0 8.0 10.0 12.0 Absorbance 0.11 0.25 0.45 0.63 0.87 1.05 1.24 Use the data in the table to plot a graph of absorbance against glucose concentration. a) Is Beer's Law obeyed? b) From the best fit line, calculate the molar absorptivity, &, and its units. c) If a urine sample has absorbance = 0.53, use your graph (not any individual data points) to determine its glucose concentration.

How should molar mass, dipole moment, dielectric, and charge on oxygen effect evaporation rate in acetone, pentane, methanol, ethanol, 1-Butanol, and 1-Propanol?

How iso-butane is used to ionize the given sample.