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katen-ka-za [31]
3 years ago
15

A certain substance melts at a temperature of . But if a sample of is prepared with of urea dissolved in it, the sample is found

to have a melting point of instead. Calculate the molal freezing point depression constant of . Round your answer to significant digits.
Chemistry
1 answer:
pshichka [43]3 years ago
5 0

Answer:

2.2 °C/m

Explanation:

It seems the question is incomplete. However, this problem has been found in a web search, with values as follow:

" A certain substance X melts at a temperature of -9.9 °C. But if a 350 g sample of X is prepared with 31.8 g of urea (CH₄N₂O) dissolved in it, the sample is found to have a melting point of -13.2°C instead. Calculate the molal freezing point depression constant of X. Round your answer to 2 significant digits. "

So we use the formula for <em>freezing point depression</em>:

  • ΔTf = Kf * m

In this case, ΔTf = 13.2 - 9.9 = 3.3°C

m is the molality (moles solute/kg solvent)

  • 350 g X ⇒ 350/1000 = 0.35 kg X
  • 31.8 g Urea ÷ 60 g/mol = 0.53 mol Urea

Molality = 0.53 / 0.35 = 1.51 m

So now we have all the required data to <u>solve for Kf</u>:

  • ΔTf = Kf * m
  • 3.3 °C = Kf * 1.51 m
  • Kf = 2.2 °C/m
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3.- Write a coefficient of 45/2 to the O₂, and multiply all the equation by 2.

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Explanation:

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Now, the ice has melted.

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Q = 79.7 cal/g . 10 g → 797 cal

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Water is ready now, to become vapor so let's determine the heat.

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Q = 10 g . 0.470 cal/g°C . (120°C - 100°C) → 94 cal

Now, we have to sum all the heat that was added in all the process.

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