Question

Question 2 The vapour pressure, p, of nitric acid varies with temperature as follows: Temperature / °C Vapour pressure / Torr 0 14.4 20 47.9 40 133 50 208 70 467 80 90 670 937 1282 100 Determine the following graphically: (a) the enthalpy of vaporization of nitric acid (b) the normal boiling point of nitric acid

Answer 1

Vapor pressure (Torr) vs Temperature(C) 1400 1200 1000 y = 12.115x - 211.56 20 40 60 80 100 120 -400

Using clausius-clapeyron equation:-

If P1 and P2 are the vapor pressures at two temperatures T1 and T2, then a simple relationship can be found.

que les balla): - Alap ic in/ & A Mug ( 1 ) for any 2 values of partial pressure and o corresponding temperatures, we can find out enthalpy of vapouization. For P = 47.9 , T, = ☆ 20°c = 293k l=133 Tz = 50°c = 313k en ( 933 ) mayo titi s +1.02= Aluap 40.00022 ) 8.314 A Hvap = 1.02X 8.314 0.00022 . Hvap = 38.55 kJ/mol - bl Now, the boiling point is the temperaturen at which the vapor presure becomes equal to the atmospheric pressure. We need to find the temperature at a which vapour presive = 760 Tour (atm: pressure): Scanned, with P

The equation of the graph as shown on . the graph is a 12-1150-211.56 Here, y= vapor pressure and y=760 Towe, t we need to findn, le: Temperature (Boiling point) 760=12.1154 -211-56 CamScanner X = 80.2°C 7 Boiling point of nitric aitt Scarited-with-

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