The vapor pressure of dichloromethane, CH2Cl2, at 0°C is 134 mmHg. The normal boiling point of dichloromethane is 40°C. Calculate its molar heat of vaporization using the Clausius-Clapeyron equation.

Understand the Clausius-Clapeyron equation, which relates the vapor pressure and temperature to the molar heat of vaporization. The equation is: $P^1=P^2-\frac{\mathrm{\Delta H_vap}}{R\times (\frac{1}{\mathrm{T₁}}}$, where $P$ is the vapor pressure, $T$ is the temperature in Kelvin, $\mathrm{\Delta H_vap}$ is the molar heat of vaporization, and $R$ is the universal gas constant.