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sashaice [31]
3 years ago
5

What is the freezing point of a solution containing 4.78 grams naphthalene (molar mass = 128.2 g/mol) dissolved in 32.0 grams pa

radichlorobenzene?
Chemistry
1 answer:
tester [92]3 years ago
4 0
This is a freezing point depression problem, so it will use the equation:

ΔT = i Kf<span> m
</span>
i = 1 (naphthalene does not dissociate further when dissolved)
Kf = 7.10 C/m (a constant for paradichlorobenzene, which you'd be given)
m = moles of solute / kg of solvent; moles of solute = 4.78 / 128.2 = 0.0373; kg of solvent = 0.032; m = 0.0373 / 0.032 = <span>1.166m

</span>ΔT = 1 x 7.10 x 1.166 = 8.279 C

This means the normal freezing point of pure paradichlorobenzene is decreased by 8.279 C; the normal freezing point (again, something you'd be given) is 53.5 C, so the new freezing point would be 53.5 - 8.279 = 45.221 C.
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Explanation:

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d =

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DENSITY

Density is defined as mass per unit volume.

d =

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Example:

A brick of salt measuring 10.0 cm x 10.0 cm x 2.00 cm has a mass of 433 g. What is its density?

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d =

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If 500 mL of a liquid has a density of 1.11 g/mL, what is its mass?

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V =

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Example:

What is the volume of a bar of gold that has a mass of 14.83 kg. The density of gold is 19.32 g/cm³.

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14.83 kg ×

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A balloon has a volume of 6.2 liters at 23.2 C. The balloon is then heated to a temperature of 144.0 C. What is the volume of th
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Answer:

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