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sweet-ann [11.9K]
3 years ago
5

PLEASE HELP ME ASAPPPP

Chemistry
1 answer:
steposvetlana [31]3 years ago
7 0
Answer: 100.95°C


Explanation:

1) The increase of the boiling point of a solution is a colligative property and its value is:

ΔTb = m × Kb × i 

2) i is the Van't Hoof constant ans for non ionic solute is 1.

3) m is the molality

m = moles of solute / Kg of solvent


moles of solute = mass in grams / molar mass

molar mass of <span>C₂H₅OH = 2 × 12.0 g/mol + 2 × 1.0 g/mol + 16.0 g/mol + 1.0 g/mol = 43.0 g/mol
</span><span>
</span><span>
</span><span>moles of solute = 20.0 g / 43.0 g/mol = 0.465 mol
</span><span>
</span><span>
</span>m = 0.465 mol / 0.250 kg = 1.86 m


3) Kb is the molal boiling constant of the solvent.

For water Kb = 0.512 °C / mol 

4) ΔTb = 1.86m × 1 × 0.512 °C / mol = 0.95°C.

5) Boiling temperature

Tb = 100°C + 0.95°C = 100.95°C
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Aspirin sun thesis Green Chemistry and Assime the aspirin is prepared by the following reaction and that 10.09. of salicylic aci
klemol [59]

<u>Answer:</u> The percentage yield of aspirin is 38.02 %.

<u>Explanation:</u>

To calculate the number of moles, we use the equation:

\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}      .....(1)

  • <u>For salicylic acid:</u>

Given mass of salicylic acid (C_7H_6O_3) = 10.09 g

Molar mass of salicylic acid (C_7H_6O_3) = 138.12 g/mol

Putting values in equation 1, we get:

\text{Moles of salicylic acid}=\frac{10.09g}{138.12g/mol}=0.0730mol

The chemical equation for the formation of aspirin follows:

C_7H_6O_3+C_4H_6O_3\rightarrow C_9H_8O_4+CH_3COOH

As, acetic anhydride is present in excess. So, it is considered as an excess reagent.

Thus, salicylic acid is a limiting reagent because it limits the formation of products.

By Stoichiometry of the reaction:

1 mole of salicylic acid produces 1 mole of aspirin.

So, 0.0730 moles of salicylic acid will produce = \frac{1}{1}\times 0.0730=0.0730mol of aspirin

Now, calculating the mass of aspirin from equation 1, we get:

Molar mass of aspirin = 180.16 g/mol

Moles of aspirin = 0.073 moles

Putting values in equation 1, we get:

0.073mol=\frac{\text{Mass of aspirin}}{180.16g/mol}\\\\\text{Mass of aspirin}=13.15g

To calculate the percentage yield of aspirin, we use the equation:

\%\text{ yield}=\frac{\text{Experimental yield}}{\text{Theoretical yield}}\times 100

Experimental yield of aspirin = 5.0 g

Theoretical yield of aspirin = 13.15 g

Putting values in above equation, we get:

\%\text{ yield of aspirin}=\frac{5.0g}{13.15g}\times 100\\\\\% \text{yield of aspirin}=38.02\%

Hence, the percent yield of aspirin is 38.01 %.

6 0
4 years ago
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