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klio [65]
3 years ago
9

Determine the boiling point of a solution that contains 70.6 g of naphthalene (C10H8, molar mass = 128.16 g/mol) dissolved in 72

2 mL of benzene (d = 0.877 g/mL). Pure benzene has a boiling point of 80.1°C and a boiling point elevation constant of 2.53°C/m.
Chemistry
1 answer:
MissTica3 years ago
3 0

Answer:

Boiling point of the solution is 82.3°C

Explanation:

Boiling point elevation is defined as the increasing of a boiling point of a substance by the addition of a solute. The formula is:

ΔT = K×m×i

<em>Where ΔT is change in temperature (Final T - 80.1°C), K is boiling point elevation constant (2.53°C/m), m is molality of the solution (moles of naphthalene / kg of benzene) and i is Van't Hoff factor (1 for Naphthalene)</em>

Moles of 70.6g of naphthalene are:

70.6g × (1mol / 128.16g) = 0.5509 moles

Kg of 722mL of benzene are:

722mL × (0.877g / mL) × (1kg / 1000g) = 0.633kg of benzene

Replacing in boiling point elevation formula:

(T - 80.1°C) = 2.53°C/m×(0.5509mol / 0.633kg)×1

T - 80.1°C = 2.2°C

T = 80.1°C + 2.2°C

T = 82.3°C

<h3>Boiling point of the solution is 82.3°C</h3>
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