We’re being asked to **determine the temperature** at which benzene boil when the external pressure is 450 torr

For this problem, we can use the ** Clausius-Clapeyron Equation**:

$\overline{){\mathbf{ln}}\frac{{\mathbf{P}}_{\mathbf{2}}}{{\mathbf{P}}_{\mathbf{1}}}{\mathbf{}}{\mathbf{=}}{\mathbf{}}{\mathbf{-}}\frac{\mathbf{\u2206}{\mathbf{H}}_{\mathbf{vap}}}{\mathbf{R}}\mathbf{[}\frac{\mathbf{1}}{{\mathbf{T}}_{\mathbf{2}}}\mathbf{-}\frac{\mathbf{1}}{{\mathbf{T}}_{\mathbf{1}}}\mathbf{]}}$

where:

**P _{1}** = vapor pressure at T

**P _{2}** = vapor pressure at T

**ΔH _{vap}** = heat of vaporization (in J/mol)

**R** = gas constant (8.314 J/mol•K)

**T _{1} and T_{2}** = temperature (in K).

Benzene has a heat of vaporization of 30.72 kJ/mol and a normal boiling point of 80.1 ^{o}C. At what temperature does benzene boil when the external pressure is 450 torr?

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Clausius-Clapeyron Equation concept. You can view video lessons to learn Clausius-Clapeyron Equation. Or if you need more Clausius-Clapeyron Equation practice, you can also practice Clausius-Clapeyron Equation practice problems.

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