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Luda [366]
3 years ago
15

Ethanol is used widely as a solvent in laboratories for various chemical reactions. A laboratory technician takes 50.0 mL of eth

anol and dilutes it to 100.0 mL with distilled water. What is the percentage concentration by volume of the resulting solution?
Chemistry
2 answers:
puteri [66]3 years ago
8 0
This question is quite vague, as the initial concentration of ethanol is not provided. However, from experience I can tell you that most laboratory work is done with 98% ethanol, and not absolute ethanol (100%). So in order to calculate the final concentration, we need to take the given values, which includes the initial concentration (98%), the initial volume (50.0mL) and the final volume (100.0mL). We apply the following equation to calculate the final concentration:

C1V1 = C2V2
C1 = Initial concentration
C2 = Final concentration
V1 = Initial volume
V2 = Final volume

(98%)(50.0mL) = (C2)(100.0mL)
Therefore, the final concentration (C2) = 49%
borishaifa [10]3 years ago
8 0
The answer is B 50% just finished the test
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Answer:

92.87 g.

Explanation:

∵ The percentage yield = (actual yield/theoretical yield)*100.

  • We need to calculate the theoretical yield:

From the balanced reaction:

<em>PCl₃ + Cl₂ → PCl₅,</em>

It is clear that 1 mol of PCl₃ reacts with 1 mol of Cl₂ to produce 1 mol of PCl₅.

  • We need to calculate the no. of moles of 73.7 g PCl₃:

n = mass/molar mass = (73.7 g)/(137.33 g/mol) = 0.536 mol.

<u><em>Using cross multiplication:</em></u>

1 mol of PCl₃ produce  → 1 mol of PCl₅, from stichiometry.

∴ 0.536 mol of PCl₃ produce  → 0.536 mol of PCl₅.

∴ The mass of PCl₅ (theoretical yield) = (no. of moles) * (molar mass) = (0.536 mol)*(208.24 g/mol) = 111.62 g.

<em>∵ The percentage yield = (actual yield/theoretical yield)*100.</em>

The percentage yield = 83.2%, theoretical yield = 111.62 g.

∴ The actual yield of PCl₅ = (The percentage yield)(theoretical yield)/100 = (83.2%)(111.62 g)/100 = 92.87 g.

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