The apparatus shown here is used to measure the vapor pressure of ethylene diamine. The system is loaded with pure ethylene diamine and the bath is adjusted to each of several known temperatures. The following readings are taken on a day when the atmospheric pressure is 758.9 mm Hg:

(a) Calculate p for ethylene diamine at each temperature.

(b) Use a semi log plot of p* versus 1/T to estimate the normal boiling point and the heat of vaporization of ethylene diamine.

(c) Does the Clausius?Clapeyron equation appear to be justified for ethylene diamine in the temperature range covered by the data? Explain.

Transcribed Image Text:

42.7 58.9 68.3 Constant- temperature bath 77.9 88.6 98.3 105.8 Mercury Level T(°C) Right Arm (mm) Left Arm (mm): 138 160 182 213 Liquid 262 323 383 Vapor 862 840 818 787 738 677 617