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3 years ago

Mechanism of aspirin by salicyclic acid reacts with acetic acid ? Mechanism of benzoic acid from benzamide?

Chemistry

1 answer:

nexus9112 [7]3 years ago

3 0

Answer:

See explanation

Explanation:

The synthesis of aspirin is shown in the reaction scheme attached to this answer. The production of aspirin involves the reaction of acetyl salicyclic acid and acetic anhydride. HA in the reaction mechanism refers to an acid that is used in the reaction

Similarly benzamide, is converted to the carbonyl carbocation by reaction with acid. The -NH2 group is protonated and subsequently departs as a leaving group. An OH^- completes the mechanism forming a carboxylic acid. The movement of electrons is shown in the image attached.

Again, the diazotization of benzamide using sodium nitrate and concentrated HCl yields benzene diazonium chloride. Addition of water to benzene diazonium chloride yields the benzoic acid and nitrogen gas.

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The question in the picture, I really a correct answer, no cheap answers

Delvig [45]

Answer:

94.325 g

Explanation:

We'll begin by converting 350 mL to L. This can be obtained as follow:

1000 mL = 1 L

Therefore,

350 mL = 350 mL × 1 L /1000 mL

350 mL = 0.35 L

Next, we shall determine the number of mole of KC₂H₃O₂ in the solution. This can be obtained as follow:

Volume = 0.35 L

Molarity of KC₂H₃O₂ = 2.75 M

Mole of KC₂H₃O₂ =?

Molarity = mole /Volume

2.75 = Mole of KC₂H₃O₂ / 0.35

Cross multiply

Mole of KC₂H₃O₂ = 2.75 × 0.35

Mole of KC₂H₃O₂ = 0.9625 mole

Finally, we shall determine the mass of KC₂H₃O₂ needed to prepare the solution. This can be obtained as illustrated below:

Mole of KC₂H₃O₂ = 0.9625 mole

Molar mass of KC₂H₃O₂ = 39 + (12×2) +(3×1) + (16×2)

= 39 + 24 + 3 + 32

= 98 g/mol

Mass of KC₂H₃O₂ =?

Mass = mole × molar mass

Mass of KC₂H₃O₂ = 0.9625 × 98

Mass of KC₂H₃O₂ = 94.325 g

Thus, the mass of KC₂H₃O₂ needed to prepare the solution is 94.325 g

6 0

3 years ago

Balance the following chemical equation <br> __Mg+__O2–>__MgO

mario62 [17]

Answer:

2Mg^+ +O2 right arrow 2MgO

Explanation:

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3 years ago

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If you had excess chlorine, how many moles of of aluminum chloride could be produced from 19.0 g of aluminum?

SIZIF [17.4K]

The chemical reaction would be written as follows:

2Al + 3Cl2 = 2AlCl3

We are given the amount of aluminum to be used in the reaction. This will be the starting point of the calculations. We do as follows:

19.0 g Al ( 1 mol / 29.98 g ) ( 2 mol AlCl3 / 2 mol Al ) = 0.63 mol AlCl3

5 0

3 years ago

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Which is evidence that the reaction below is a redox reaction? 2Na + Cl2 → 2NaCl

Mamont248 [21]

A redox reaction --> a reaction whereby oxidation & reduction occurs
Reduction:
Charge of Cl2 = 0
Charge of Cl- in NaCl = -1
Hence, since charge of Cl2 decreased from 0 in Cl2 to -1 in NaCl, reduction occured.
Oxidation:
Charge of Na = 0
Charge of Na+ in NaCl = +1
Hence, since charge of Na increased from 0 in Na to +1 in NaCl, oxidation occured.
Since both oxidation & reduction occured in the reaction, it is a redox reaction.

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3 years ago

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9966 [12]

C.) both secrete toxins and have thorns (It simply depends on what kind of plant it is)

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