The enthalpy of an unknown liquid is 28.96 kJ/mol. and its normal boiling point is 65.0oC. Use the Clausius-Clapeyron equation to calculate the vapor pressure of the unknown liquid at 21.0oC. Enter your answer in units of torr.
The enthalpy of an unknown liquid is 28.96 kJ/mol. and its normal boiling point is 65.0oC....
The enthalpy of an unknown liquid is 29.86 kJ/mol. and its normal boiling point is 77.0oC. Use the Clausius-Clapeyron equation to calculate the vapor pressure of the unknown liquid at 24.0oC. Enter your answer in units of torr.
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...
The ΔHvap of hexane is 28.16 kJ/mol and its boiling point is 65.2 °C. Using the Clausius-Clapeyron equation, calculate the vapor pressure (mm Hg) of hexane at 25.0 °C.
A liquid with an enthalpy of vaporization, DHv, of 32.80 KJ/mole has a normal boiling point at 39.20°C. Its vapor pressure at 57.35°C is: (a) 1728 Torr (b) 2644 Torr (c) 2185 Torr (d) 1521 Torr
The molar enthalpy of vaporization of carbon disulfide is 26.74 kJ/mol, and its normal boiling point is 46°C. What is the vapor pressure of CS2 at 0°C? a)447 torr b)4160 torr c)313 torr d)139 torr e)5.47 torr
The molar enthalpy of vaporization of hexane (C6H14) is 28.9 kJ/mol, and its normal boiling point is 68.73°C. What is the vapor pressure of hexane at 25°C? (R-8.314 J/K • mol) O 4.44 torr O 117 torr O 171 torr O 759 torr 0 3370 torr
The molar enthalpy of vaporization of liquid nh4 is 23.5 kJ/mol, and it’s normal boiling point is -33.4 C. What is the vapor pressure of ammonia at-21.5C
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?
The normal boiling point of ammonia is -33.3°C, and its enthalpy of vaporization is 23.35 kJ/mol. Calculate the temperature in °C required to double the vapor pressure of ammonia.
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?