CH201 LAB 1 Aniline Synthesis ..................... PDF

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MELVINAMANSITA KRISHNASORGANICCHEMISTRYCH201 LAB 1Pre-Lab (2 m)number of techniques. The NO2 group will be reduced to NH2 using tin and hydrochloric acid corrosive in this experiment. In this acidic environment, the initially framed aniline quickly converts to aniline hydrochloride. By making the an...

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MELVINA MANSITA KRISHNA S11157774 ORGANIC CHEMISTRY CH201 LAB 1

Pre-Lab (2 m)

SYNTHESIS OF ANILINE Title (0.5 m) Aim (1 m) Combining aniline with nitrobenzene through aniline (Phenyl ammonium) intermediates and determining aniline yield via simple filtration and distillation as a refinement measure. Introduction (2 m) Unlike halide, the NH2 group cannot be brought into a sweet-smelling ring by an electrophilic replacement response. Alternatively, it could be framed from previous utilitarian gatherings on the benzene loop. The reduction of NO2 gatherings is one way of forming NH2 bunches. Since the NO2 bunches are quickly brought into a sweet-smelling system, and it is also quickly decreased, this is the most popular method for planning sweet-smelling amines. The NO2 swarm can be minimized by a

number of techniques. The NO2 group will be reduced to NH2 using tin and hydrochloric acid corrosive in this experiment. In this acidic environment, the initially framed aniline quickly converts to aniline hydrochloride. By making the answer blend basic, free aniline is finally released. The unrefined aniline is then separated from the fluid mixture using distillation. Basic refining is used to clean aniline, which is unavoidable.

Procedure (2 m) ➢ The protocol outlined in the lab manual was adopted with only minor modifications. ➢ Nitrobenzene (5.5cm3) and granulated tin (11g) in a 500cm3 round base carafe with reflux condenser. ➢ Little parcels were used in a 25cm3 concentrated hydrochloric corrosive. Twirled mixture. After the reaction subsided, the cup with the condenser was warmed for 30 minutes on a warming mantle with occasional whirling. ➢ The mixture was cooled by adding 25cm3 water and expanding a 17.54g NaOH solution in 30cm3 water. ➢ To see if the mixture is unmistakably antacid, Litmus paper was used. ➢ To see if the mixture is unmistakably antacid, Litmus paper was used. ➢ Steam grinding was used, and smooth distillate was collected until the distillate was clear. ➢ When the distillate was clear, it was collected for another 5 minutes before refining was stopped. A purple dark hastens (Aniline Chloride + Stannic Chloride) was formed after the 500cm3 Round base jar had been warm for 30 minutes. The litmus paper turned pale blue green instead of yellow. The structure in the round base jar was antacid, as shown by this. Since it was a suspension of aniline in water, the first distillate was silky smooth.

(3 m)

Data table (5 m)

RESULTS TABLE

Reagents

Classification (MSDS) Flammable

Mr (g/mol) 123.06

Toxic

Hydrochloric acid (HCl) Sodium Hydroxide (NaOH) Water (H₂O) Aniline (C6H5NH2)

Nitrobenzene (C6H5NO2) Tin (Sn)

6

Moles (mol) 0.049

Volume (mL) 5.5

Density (g/cm3) 1.09

118.71

11

0.093

1.51

7.3

Toxic

36.46

29.75

0.82

25

1.19

Corrosive

40.00

17.54

0.44

8.23

2.13

Neutral

18

25

1.39

25

1

Flammable

93.13

9.6

0.1

9.4

1.02

Calculation (5 m) Mass of aniline = 9.4mL x 1.02 = 9.6g (Experimental Yield) A) Find the mole ratio: Nitrobenzene: Aniline 1: 1 0.049: x Therefore, x mole is = 0.049 moles B) Mass (aniline) = n × Mr = 0.049 mol × 93.13 g/mole = 4.56g (Theoretical yield) C) Percentage yield: Experimental yield/ Theoretical yield × 100% 9.6g/4.56 g × 100%

Mass (g)

Percentage yield=210%

Data analysis and comparison (3 m) Since there were a few blunders during the labs, the average response level was discovered to be 210 percent, which can be relied upon. One of these errors is that the reactant was overheated in the main technique, and the arrangement was not whirled together as one, resulting in a portion of the reactant not fully blending in with the other compound and the way it was overheated suggests that some of the reactants responded even though we didn't need them to. Second, when we tried to use the refining interaction to refine the aniline that was formed in the arrangement, the steam hardware failed, and the arrangement cooled down much faster than it should have. Another blunder was that we failed to tow the way toward treating aniline in order to remove the water from the arrangement and leave the aniline alone as seen by the rate yield, if these errors had not occurred, the response yield would not have been as high. Post-Lab question (3 m) 1)Write an equation to show how aniline is liberate from the acidic mixture upon the addition of sodium hydroxide? C6H5NH3 + OH → C6H5NH2 + H2O

2)Why is anhydrous magnesium sulfate not a very good drying agent to dry an ether solution of aniline? Since it exists as a solid crystal, the packing fraction is extremely poor, and it is unable to accommodate water molecules. 3)The distillate collected from steam distillation has the aniline being the bottom layer, but after saturating the solution with sodium chloride, the aniline now becomes the top layer. Explain why? Due to the fact that aniline is an organic compound, it can dissolve in the ether layer. Aniline can settle on the bottom layer because ether is denser than water (ether layer). Conclusion: I learned a lot from this investigation, and I discovered that to shape an aniline, we should start with nitrobenzene and reduce it with tin and hydrochloric acid to form aniline, and then add sodium hydroxide to remove the H+ in the aniline to form aniline. Despite the fact that the rate yield we discovered was 210 percent due to the reagent being overheated, instead of twirling the mixture to combine the reagent. In addition, there isn't a lot of equipment in the lab, and the steam processing hasn't been completed as a result of this. However, taking everything into consideration, I learned a lot from this lab....