The vapor pressure of the liquid CaH10 is measured at different temperatures. The following vapor pressure data are obtained. Temperature, K P, mmHg 251.1 325.5 626.0 267.4 Calculate the enthalpy of vaporization (AH) in ka/mol for this liquid. k/mol

The enthalpy of vaporization for methanol is 35.2 kJ/mol. Methanol has a vapor pressure of 101.3 kPa at 64.7 °C. Using the Clausius-Clapeyron equation, what is the vapor pressure for methanol at 44.9 °C? Give your answer in kPa, to the first decimal point.

The enthalpy of vaporization of Substance X is 7.00 kJ/mol and its normal boiling point is −33.°C. Calculate the vapor pressure of X at −57.°C. Round to two sig figs. Answer in atm. .

Ethanol, with AHvap = 40.5 kJ mol, has a higher AHvap than methanol, which is 35.2 kJ mol, due to its larger size and greater intermolecular forces. Because the AH for ethanol is larger, we would expect that for the two liquids to reach the same vapor pressure, the temperature for ethanol would have to be higher. If the vapor pressure is 0.0992 atm at 27.3 °C, what would the temperature be when the vapor pressure is 4.87 atm? The temperature will be K. e Textbook and Media

Ethanol, with ΔHvap = 40.5 kJ mol-1, has a higher ΔHvap than methanol, which is 35.2 kJ mol-1, due to its larger size and greater intermolecular forces. Because the ΔHvap for ethanol is larger, we would expect that for the two liquids to reach the same vapor pressure, the temperature for ethanol would have to be higher. If the vapor pressure is 0.0992 atm at 27.3 °C, what would the temperature be when the vapor pressure is 4.52 atm?

The enthalpy of vaporization for methanol is 35.2 kJ/mol. Methanol has a vapor pressure of 101.3 kPa at 64.7 °C. Using the Clausius-Clapeyron equation, what is the vapor pressure for methanol at 37.7 °C? Give your answer in kPa, to the first decimal point.

Measurements of the saturated vapor pressure of liquid SiCl4 give 0.1396 atm at 280 K and 0.4880 atm at 310 K. Calculate the normal boiling temperature of SiC14.

.  The vapor pressure and enthalpy of vaporization of an unknown substance are measured to be 479.6 torr and 35.3 kJ/mol, respectively at room temperature (298.15 K). Estimate the normal boiling point of the substance at an atmospheric pressure of 760 torr.

What is Δq for the vaporization of 50.0 g of Compound A (76.03 g/mol;  ΔHvap is 31.6 kJ/mol)?