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The vapor pressure of nitrogen at several different temperatures is shown below. Temperature (K) Pressure (torr) 65 130.5 85 1718 Part A: Use the data to determine the heat of vaporization, ΔHvap, of nitrogen using the two-point form of the van't Hoff equation. This equation is known as the Clausius-Clapeyron equation when applied to the vaporization "reaction" of liquid phases. For this problem, the vaporization reaction is: N2(l) ⇌ N2(g). Express your answer in kilojoules per mole. Part B: Determine the normal boiling point of nitrogen. Remember that boiling points are temperatures, so you're finding the temperature at which the vapor pressure is equal to the atmospheric pressure, which is the condition that must be met for boiling to occur. The normal boiling point defines atmospheric pressure to be 760 torr. So, you're finding the temperature at which the vapor pressure is equal to 760 torr. Express your answer in kelvins.

          The vapor pressure of nitrogen at several different temperatures is shown below.

Temperature (K)   Pressure (torr)
65                130.5
85                1718

Part A: Use the data to determine the heat of vaporization, ΔHvap, of nitrogen using the two-point form of the van't Hoff equation. This equation is known as the Clausius-Clapeyron equation when applied to the vaporization "reaction" of liquid phases. For this problem, the vaporization reaction is: N2(l) ⇌ N2(g). Express your answer in kilojoules per mole.

Part B: Determine the normal boiling point of nitrogen. Remember that boiling points are temperatures, so you're finding the temperature at which the vapor pressure is equal to the atmospheric pressure, which is the condition that must be met for boiling to occur. The normal boiling point defines atmospheric pressure to be 760 torr. So, you're finding the temperature at which the vapor pressure is equal to 760 torr. Express your answer in kelvins.

Added by Johnny P.

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