Liquid nitrogen has a measured enthalpy of vaporization ( ΔH^o vap) = 2.79 kJ/mol and entropy of vaporization ( Δ S^ovap) = 36.1 J/K mol. Calculate the boiling point of liquid nitrogen, in oC using this information. (Use 273.15 K = 0 oC for the temperature conversion. Report your answer with three significant figures.)
Tvap = ????? °C
I got 196^oC but it is incorrect.
Liquid nitrogen has a measured enthalpy of vaporization ( ΔH^o vap) = 2.79 kJ/mol and entropy...
36.1 J/K mol. Calculate the boiling point of liquid Liquid nitrogen has a measured enthalpy of vaporization (AH vap -2.79 kJ/mol and entropy of vaporization (AS nitrogen, in °C using this information. (Use 273.15 K 0°C for the temperature conversion. Report your answer with three significant figures.) Tp C
3. A liquid compound has an enthalpy of vaporization equal to 65.0 kJ and an entropy of equal to 98 J/K at its boiling point. Calculate the boiling point of the compound. AH = 65 kJ AS - 987
A liquid has a ΔH o vap of 31.1 kJ/mol and a boiling point of 135°C at 1 atm. What is its vapor pressure at 106°C?
A liquid has a ΔH o vap of 34.2 kJ/mol and a boiling point of 124°C at 1 atm. What is its vapor pressure at 111°C? _____atm
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 standard enthalpy of vaporization (H°vap) of methylacrylate (CH2CHCO2CH3) is 36.0 kJ/mol. The normal boiling point of methylacrylate is 80.5°C. Calculate the vapour pressure of methylacrylate at 43.0°C.
The standard enthalpy of vaporization (DeltaH°vap) of acetic anhydride ((CH3CO)2O) is 45.7 kJ/mol. The normal boiling point of acetic anhydride is 139.6°C. Calculate the vapour pressure of acetic anhydride at 116.1°C.
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 enthalpy of vaporization of mercury is 58.5 kj/mol and the normal boiling point is 630K, You want to calculate the entropy of vaporization for mercury. Which of the following statements concerning this problem is incorrect? Why is this statement incorrect? A) We wxpect DS to be positive for the vaporization of mercury B) Once we know that DS is for this process we will know if it is spontaneous C) We can calculate the entropy of mercury because we...
A liquid has a vapor pressure of 8.36 torr at 319 K. Its enthalpy of vaporization is 33.4 kJ/mol. What is its normal boiling point, in K? Give your answer to the nearest 0.1 K. Store intermediate results in your calculator or write them down with at least four significant figures!