Chloroform has a normal boiling point of 61°C and a Hvap of 29.6 kJ/mol. Determine the...

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Question

Answer 1

Answer #1

We need to use the Clausius clapeyron equation, which describes the variation of boiling point with respect to temperature.

$ln\frac{p_{2}}{p_{1}} = \frac{-\Delta H_{vap}}{R}(\frac{1}{T_{2}}-\frac{1}{T_{1}})$

T₁ = 61 ^oC = 61 +273 = 334 K

T₂ = 35 ^oC = 35 +273 = 308 K

P₁ = 1 atm

R = 8.314 J/(mol.K)

delta H_vap = 29.6 kJ/mol = 29600 J/mol

Putting the values in the equation,

ln(P₂) = (-29600/8.314) * ((1/308)-(1/334))

Solving for gives P2 = 0.407 atm

Answer 2

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