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The vapor pressure of nitric acid varies with temperature as follows. T/oC 0 20 40 50...

The vapor pressure of nitric acid varies with temperature as follows.

T/oC 0 20 40 50 70 80 90 100
P/torr 14.4 47.9 133 208 467 670 937 1282

What is the normal boiling point and the enthalpy of vaporization?

Solutions

Expert Solution

from clasius-clepyron equation

ln(p2/p1) = DH0rxn/R[1/T1 - 1/T2]

P1 = 14.4 torr, T1 = 273.15+0 = 273.15 k

P2 = 47.9 torr,    T2 = 273.15 +20 = 293.15 k

DHvap = ? kj/mol

ln(47.9/14.4) = (x/8.314)((1/273.15)-(1/293.15))

enthalpy of vaporisation = DHvap = 40.006 kj/mol

at normal boiling point, Pressure = atmospheric pressure = 1 atm = 760 torr.

ln(p2/p1) = DH0rxn/R[1/T1 - 1/T2]

P1 = 14.4 torr, T1 = 273.15+0 = 273.15 k

P2 = 760 torr,    T2 = ? k

DHvap = 40.006*10^3 j/mol

ln(47.9/760) = (40.006*10^3/8.314)((1/273.15)-(1/x))

T2 = 236.1 k

normal boiling point = 273.15-236.1 = 37.05 c

queen_honey_blossom answered 2 years ago
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