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Anit [1.1K]
3 years ago
8

A chemistry student needs 60.0 g of 2-ethyltoluene for an experiment. He has available 1.5 kg of a 15.3% w/w solution of 2 ethyl

toluene in carbon tetrachloride Calculate the mass of solution the student should use. If there's not enough solution, press the "No solution" button. Round your answer to 3 significant digits.
Chemistry
1 answer:
Mila [183]3 years ago
8 0

Answer:

392 g

Explanation:

The given concentration tells us that<em> in 100 g of solution, there would be 15.3 g of 2-ethyltoluene</em>.

With that in mind we can<u> calculate how many grams of solution would contain 60.0 g of 2-ethyltoluene</u>:

  • Mass of solution * 15.3 / 100 = 60.0 g 2-ethyltoluene
  • Mass of solution = 392 g
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What is the theoretical yield of fluorenone if you oxidize 175 mg of fluorene?
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Answer:

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Explanation:

The<em> yield</em> is measured by the amount of each product produced by the reaction.

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The <em>oxidation</em>, also know as combustion, of this hydrocarbon is represented by the following balanced chemical equation:

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<u />

<u>2. Convert 175mg of fluorene to number of moles</u>

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  • Number of moles = mass in grams / molar mass

  • \text{number of moles}=0.175g/166.223g/mol=0.0010528mol

<u>3. Set a proportion for each product of the reaction</u>

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i) number of moles

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ii) mass in grams

The molar mass of H₂O is 18.015g/mol

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  • mass = 0.00526 moles × 18.015 g/mol = 0.0948mg = 94.8 mg
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