a) An unknown liquid has a heat of vaporization of 31.97 kJ/mole.  If the normal boiling point is 80, 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).

a) An unknown liquid has a heat of vaporization of 31.97 kJ/mole.  If the normal boiling point is 80, 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). 

b) Image: Graph, Energy on X axis, Temp on Y axis. There is a line sloping up and to the right labelled "A" beginning near bottom of Y-axis. At end of this line, there is a horizontal line labelled "B". At the end of this line there is another line sloping up and to the right labelled "C". End of Image.

NH₃ (MW = 17.034 g/mol)

Melting point = minus 77.73 degrees C

Boiling point = minus 33.34 degrees C

Heat capacity of liquid = 4.700 J/g/K

Heat capacity of gas = 2.060 J/g/K

Heat of vaporization = 23.40 kJ/mol

Find A, B and C (as far as 0 degrees C) and the total energy required (in that order) in Joules (express as 'J'). Assume 100.0 g of substance. A, B and C should have four significant figures.

When entering your values import your answer followed by a space then J

Example: 3450. J

Notice that in this particular example a decimal point was included after 3450 to indicate that the zero is significant. If the answer does not need a decimal do not include one.

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