Under 1.000 bar of atmospheric pressure, the boiling point of nitromethane is . The vapor pressure at is 15.48 kPa. Estimate to 3 significant figures the enthalpy of vaporization of nitromethane.
At , the vapor pressure of chloroform is 22.4 kPa and the enthalpy of vaporization is 31.40 kJ/mol. Estimate the boiling point of chloroform under 1 bar of atmospheric pressure.
The vapor pressure of ethanol is 5.95 kPa at and 75.0 kPa at . Estimate the enthalpy of vaporization of ethanol.
The normal boiling point of is 331.9 K, and its vapor pressure at 298 K is 0.287 bar. Within the approximations inherent to the Clausius-Clapeyron equation, what value of (the molar enthalpy of vaporization) for would be compatible with this data?
Under 1.00 bar of atmospheric pressure, the boiling point of furan is and the enthalpy of vaporization is 27.71 kJ/mol. Estimate to 3 significant figures the vapor pressure of furan at .
The vapor pressure of isooctane is 10.0 kPa at and 100.0 kPa at . Estimate the enthalpy of vaporization of isooctane.
For a compound X, which enthalpy change is associated with the process ?
When the temperature of a liquid is increased, the vapor pressure increases from to . How does the ratio vary with the enthalpy of vaporization?
Which of the following statements is incorrect?
Under 101.3 kPa of atmospheric pressure, the boiling point of acetone is and the enthalpy of vaporization is 31.3 kJ/mol. Estimate the vapor pressure of acetone at .