i)
enthalpy for vaporization is calculated by using Clausius clapeyrons equation , and unit for Enathalpy will be = unit of gas constant X unit of temperature that is joules per Mole.
ii).
we know for any liquid the the vapour pressure at boiling point is always 1 atm. On conversion of atm into kilo pascal we know the relation
1 atm = 101.325 k Pa
hence T =? , P1 = 101.325 kPa and we take T2 and P2 feom any of given set. now again using Clausius clapeyrons equation we get the boiling point.
iii)
entropy of vaporization is related to enthalpy of vaporization at boiling point is H(vap)/T
E4B.13(a) Naphthalene, C, H, melts at 80.2°C. If the vapour pressure of liquid is 1.3 kPa...
Naphthalene, C10H8, melts at 80.0 ˚C; the vapor pressure of the solid is 1.00 torr at 52.6 ˚C, and that of the liquid is 10.0 torr at 85.8 ˚C and 40.0 torr at 119.3 ˚C. Calculate: (a) the enthalpy of vaporization, the normal boiling point, and the entropy of vaporization at the boiling point; (b) the vapor pressure at the melting point (Hint: liquid and solid are in equilibrium there)
A. The normal melting point of naphthalene is 80.0 °C. At 85.8 Celsius, the liquid has a vapor pressure of 10.0 Torr which increases to 40.0 Torr at 119.3°c. Use this information to calculate the heat of vaporization, the normal boiling point, and the entropy of vaporiza of naphthalene. How similar is your calculated entropy change to the prediction of Trouton's rule? B. Assume that the triple point temperature of naphthalene is also 80.0 Celsius and that the sublimation pressure...
1) The enthalpy of vaporization for a liquid is found to be 14.4 kJ mol- at 180 K, its normal boiling point. The molar volumes of the liquid and the vapour at the boiling point are are 115 mL mol-1, and 14.5 L mol-1, respectively. a) Use the Clapeyron equation to estimage the temperature dependence of the vapour pressure (dp/dT) at the normal boiling point. b) Use the Clausius-Clapeyron equation to estimate dp/dT. c) Does the Clausius-Clapeyron equation overestimate or...
benzene melts at 5.5 degrees c if the vapor pressure of liquid benzene is 19.2 kOa at 15.8 degrees c and 15.3 kLa at 2 degrees c cakc normal boiling point and entropy if vap at normal boiling
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P4B.9 The vapour pressure, p, of nitric acid varies with temperature as follows: 0/°C 0 20 40 50 70 80 90 100 p/kPa 1.92 6.38 17.7 27.7 62.3 89.3 124.9 170.9 Determine (a) the normal boiling point and (b) the enthalpy of vaporization of nitric acid.
Estimate the saturation pressure, in kPa, of a substance at 100 °C, given that the normal boiling point is 70 °C and the enthalpy of vaporization is 30 kJ/mol.
The standard enthalpy of vaporization (H°vap) of carbon tetrachloride (CCl4) is 34.6 kJ/mol. The normal boiling point of carbon tetrachloride is 76.5°C. Calculate the vapour pressure of carbon tetrachloride at 62.5°C. after solving I got 0.4994 when using Clausius - Clapeyron equation. How do I get P2?
11.115 The following figure is a plot of vapour pressure versus temperature for dichlorodifluoromethane (CC1,F2). The enthalpy change of vaporization of the liquid is 165 kJ g'. and the specific heat capacity of the liquid is about 10 JK- Vapour pressure (kPa) воб 700 600 500 400 300 200 100 30 -40 -30 -20 -10 0 10 20 Temperature (°C) (a) What is the normal boiling point of CC1,F22 (b) A steel cylinder containing 25 kg of CC1,F2 in the...
The vapor pressure of a liquid is 300 torr at 51.0 °C, and its enthalpy of vaporization is 37.66 kJ/mol. Calculate the normal boiling point of this liquid in °C?