Question

The normal molar vaporization enthalpy (∆H_Vap ^ °) of methanol is worth 37.4 kJmol ^ (- 1), and its normal molar vaporization entropy (∆S_Vap ^ °) 110.9 JK ^ (- 1) mol ^ (- 1). Calculate:
The vapor pressure of methanol, at 298 K (R = 8.3144 J K -1 mol -1).
The approximate normal boiling point.
The boiling point for an external pressure of 0.1 atm. Applying the Clausius-Clapeyron equation, estimate the cooking temperature in a pressure cooker whose valve is set to open when the internal pressure exceeds 1 atm outside. ∆H_Vap ^ ° (H2O, 298 k) = 44.2 kJ mol ^ (- 1)
∆S_Vap ^ ° (H2O, 298 k) = 118.8 JK ^ (- 1)
R = 8.3144 J K ^ (- 1)
Toluene C6H5CH3, has a normal boiling point of 111 * C and its normal molar enthalpy of evaporation is 35.9 kJmol ^ (- 1). Calculate the toluene vapor pressure at 55 * C (R = 8.3144 J K ^ (- 1)).

Answer 1