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Zielflug [23.3K]
3 years ago
9

Draw the structure of the organic product(s) of the grignard reaction between phosgene (clcocl) and excess phenylmagnesium bromi

de, followed by aqueous workup.

Chemistry
2 answers:
Jobisdone [24]3 years ago
8 0
Phosgene on reacting with <span>phenylmagnesium bromide generates benzoyl chloride. 

Since, </span>phenylmagnesium bromide is added in excess. It would further react with benzoyl chloride to form benzophenone.

Benzophenone on further reacting with phenylmagnesium bromide, and aqueous treatment, gives triphenylmethanol. 

Entire reaction pathways is shown below:

Vikentia [17]3 years ago
4 0
<span>This is a three step reaction.
 
Step 1:
           In first step when Phenyl Magnesium Bromide (Grignard Reagent) is treated with phosgene it produces Benzoyl Chloride. In this step Grignard reagent act as a nucleophile while phosgene acts as electrophile.

Step 2:
           The Benzoyl chloride formed in first step still has an electrophillic carbon, therefore, another grignard reagent (which is present in excess) is added to the carbonyl group and results in the elimination of chloride ion (good leaving group) and formation of Benzophenone.

Step 3:
           The benzophenone (ketone) formed in second step contains a carbonyl group with electrophilic carbon. Hence, the grignard reagent is added through nucleophilic addition reaction and forms a tetrahedral intermediate, which upon hydrolysis yields triphenylmethanol (tertiary alcohol). This tertiary alcohol formed can not undergo reaction with grignard reacgent because it does not contain any electrophilic center.</span>
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1. Take the reaction: NH3 + O2 + NO + H2O. In an experiment, 3.25g of NH3 are allowed
Rudiy27

Answer:

5.74g of NO

Explanation:

Step 1:

The balanced equation for the reaction. This is given below:

4NH3 + 5O2 —> 4NO + 6H2O

Step 2:

Determination of the masses of NH3 and O2 that reacted and the mass of NO produced from the balanced equation. This is illustrated below:

Molar Mass of NH3 = 14 + (3x1) = 14 + 3 = 17g/mol

Mass of NH3 from the balanced equation = 4 x 17 = 68g

Molar Mass of O2 = 16x2 = 32g/mol

Mass of O2 from the balanced equation = 5 x 32 = 160g

Molar Mass of NO = 14 + 16 = 30g/mol

Mass of NO from the balanced equation = 4 x 30 = 120g

From the balanced equation above,

68g of NH3 reacted with 160g of O2 to produce 120g of NO.

Step 3:

Determination of the limiting reactant.

We need to determine the limiting because it will be used to calculate the maximum yield of the reaction. This is illustrated below:

From the balanced equation above,

68g of NH3 reacted with 160g of O2.

Therefore, 3.25g of NH3 will react with = (3.25 x 160)/68 = 7.65g of O2.

From the simple illustration above, we can see that lesser mass of O2 is needed to react with 3.25g of NH3. Therefore, NH3 is the limiting reactant while O2 is the excess reactant.

Step 4:

Determination of the mass of NO produced from the reaction.

In this case the limiting reactant will be used because all of it were used in the reaction.

The limiting reactant is NH3.

From the balanced equation above,

68g of NH3 reacted to produce 120g of NO.

Therefore, 3.25g of NH3 will react to produce = (3.25 x 120)/68 = 5.74g of NO.

From the calculations made above, 5.74g of NO is produced.

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Serga [27]

Answer:

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Explanation:

Hello,

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