An unknown liquid has a heat of vaporization of 37.62 kJ/mole. If the normal boiling point is 81, what is vapor pressure (in torr) of this liquid at room temperature of 25 degrees C? HINT: Normal boiling point occurs when the vapor pressure of the liquid is the same as atmospheric pressure (1 atm or 760 mm Hg). Your Answer:

The normal boiling point of a liquid is 282.0 °C. What is the vapor pressure of this liquid at 136.0 °C in atm? (∆Hvap = 28.5 kJ/mol)

An unknown liquid has a heat of vaporization of 6.41 kJ/mole. If the vapor pressure of this liquid at -200 degrees C is 120 torr, what is the normal boiling point of this liquid in degrees C? HINT: Normal boiling point occurs when the vapor pressure of the liquid is the same as atmospheric pressure (1 atm or 760 mm Hg).

The following information is given for mercury, Hg, at latm: boiling point = 357 °C AHvap(3 p(357 °C) = 59.3 kJ/mol specific heat liquid = 0.139 J/g°C At a pressure of 1 atm, kJ of heat are needed to vaporize a 27.2 g sample of liquid mercury at its normal boiling point of 357 °C.

An unknown liquid has a heat of vaporization of 32.78 kJ/mole. If the normal boiling point is 89, what is vapor pressure (in torr) of this liquid at room temperature of 25 degrees C? HINT: Normal boiling point occurs when the vapor pressure of the liquid is the same as atmospheric pressure (1 atm or 760 mm Hg). Your Answer:

The fluorocarbon compound C2Cl3F3 has a normal boiling point of 47.6 °C. The specific heat of this compound in the liquid state is 0.91 J/g-K and in the gas state is 0.67 J/g-K. The heat of vaporization is 27.5 kJ/mol. What is the amount of heat required to convert 5.6 g of the compound from a liquid at 30.0 °C to a gas at 60.5 °C?   I have been getting multiple answers, please help..

An unknown liquid has a heat of vaporization of 31.32 kJ/mole. If the normal boiling point is 88, what is vapor pressure (in torr) of this liquid at room temperature of 25 degrees C? HINT: Normal boiling point occurs when the vapor pressure of the liquid is the same as atmospheric pressure (1 atm or 760 mm Hg).

An unknown liquid has a heat of vaporization of 31.17 kJ/mole.  If the normal boiling point is 81, what is vapor pressure (in torr) of this liquid at room temperature of 25 degrees C? HINT: Normal boiling point occurs when the vapor pressure of the liquid is the same as atmospheric pressure (1 atm or 760 mm Hg).

8) The normal boiling point of acetic acid, HC₂H3O2, is 117.9°C, and its heat of vaporization is 39,690 J/mol. What is its vapor pressure at 100.0°C? A) 479.7 torr B) 616.2 torr C) 586.6 torr D) 694.4 torr E) 423.2 torr

The normal boiling point of a liquid is 282 °C. At what temperature (in °C) would the vapor pressure be 0.740 atm? (∆Hvap = 28.5 kJ/mol)