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Agata [3.3K]
3 years ago
6

Match the procedural step to its purpose in the written procedure for the Fischer esterification of benzoic acid with methanol i

n the presence of mineral acid.
a. Flat-bottomed flasks transfer heat in an uneven fashion, and may fracture if heated strongly.
b. Methanol, which is used as a reagent and solvent, is flammable.
c. The unreacted carboxylic acid was neutralized under mild conditions.
d. Water needs to be removed before the liquid ester product is collected.

1. Magnesium sulfate is added to the dichloromethane layer before the solvent is distilled off.
2. The reagents were added to a round bottom flask prior to the reaction being heated under reflux.
3. The solution of benzoic acid and methanol was heated on a steam bath.
4. The reaction mix was washed with sodium carbonate solution.
Chemistry
1 answer:
Art [367]3 years ago
4 0

Answer:

a. 2. The reagents were added to a round bottom flask prior to the reaction being heated under reflux.

b. 3. The solution of benzoic acid and methanol was heated in a steam bath

c. 4. The reaction mix was washed with sodium carbonate solution.

d. 1. Magnesium sulfate is added to the dichloromethane layer before the solvent is distilled off.

Explanation:

Fisher esterification is an equilibrium process. There are unreacted carboxylic acids in the reaction mix which are weak acids and they neutralize into aqueous solution. Magnesium sulfate is drying agent there water should be removed from dichloromethane solution before the solvent is distilled off.

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Vapor obtained by evaporating 0.495 grams of an unknown liquid is collected in a 127 mL flask. At 371 K, the pressure of the vap
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The molar mass in g/mol is 121.4 g/m

Explanation:

Let's apply the Ideal Gases Law to solve this:

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3 years ago
The most common source of copper (cu) is the mineral chalcopyrite (cufes2). how many kilograms of chalcopyrite must be mined to
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Answer : 0.8663 Kg of chalcopyrite must be mined to obtained 300 g of pure Cu.

Solution : Given,

Mass of Cu = 300 g

Molar mass of Cu = 63.546 g/mole

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  • First we have to calculate the moles of Cu.

\text{ Moles of Cu}=\frac{\text{ Given mass of Cu}}{\text{ Molar mass of Cu}}= \frac{300g}{63.546g/mole}=4.7209moles

The moles of Cu = 4.7209 moles

From the given chemical formula, CuFeS_2 we conclude that the each mole of compound contain one mole of Cu.

So, The moles of Cu = Moles of CuFeS_2 = 4.4209 moles

  • Now we have to calculate the mass of CuFeS_2.

Mass of CuFeS_2 = Moles of CuFeS_2 × Molar mass of CuFeS_2 = 4.4209 moles × 183.511 g/mole = 866.337 g

Mass of CuFeS_2 = 866.337 g = 0.8663 Kg         (1 Kg = 1000 g)

Therefore, 0.8663 Kg of chalcopyrite must be mined to obtained 300 g of pure Cu.


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