*4decimals final answers The vapor pressure of a single component, 2-phase system (vapor is assumed to be idealgas) was measured using a sealed-end manometer at different temperatures. The datacollected are as follows:T (K)251.2286321.5345Manometric363048151021pressure (mmHg)With these data. determine the following:Enthalpy change of vaporization in kJ/mola.b.| Normal boiling point using data at T = 321.5 K as referenceс.· Is the chemical species of interest vapor, liquid, or both at roomtemperature? Explain why.

We are given 4 different data sets for temperature and vapor pressure values. In order to find the…

Answered: The vapor pressure of a single…

Physical Chemistry

2nd Edition

ISBN:9781133958437

Author:Ball, David W. (david Warren), BAER, Tomas

Publisher:Ball, David W. (david Warren), BAER, Tomas

Chapter6: Equilibria In Single-component Systems

Section: Chapter Questions

Problem 6.50E

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It is well known that the temperature at which water freezes to ice or boils at a pressure of 1 atm, are 0°C and 100°C. In the next two tasks, we will now investigate what the temperatures would be at the top of Mount Everest, where the pressure is only 0.337 bar. The standard molar enthalpy of fusion of water at 0°C is ΔfusHmo = 6.008 kJ mol-1 and the standard molar enthalpy of vaporization of water at 100°C is ΔvapHmo = 40.656 kJ mol-1. The density of liquid water at 0°C is ρ(l) = 999.9 kg m-3, while the density of ice at 0°C is only ρ(s) = 916.2 kg m-3. The densities and enthalpies are assumed to be independent of temperature. 1) Calculate the temperature at which ice melts on top of Mount Everest. 2) Calculate the temperature at which water boils on top of Mount Everest.
The Clausius- Clapeyron equation on the assumption that the enthalpy of vaporization is independent of temperature in the range of interest. (a) Theenthalpy of vaporization of water is 40.656 kJ mol-1 at its normal boiling temperature, 373 K. Assuming that the enthalpy of vaporization does not vary with temperature, calculate the vapour pressure of water at 308 K. (b) Derive an improved version of the equation on the basis that the enthalpy of vaporization has the form ΔvapH =a+ bT. (c) For water in the range298- 373 K, a= 57.373 kJ mol-1 and b = -44.801 J K-1 mol- 1. Use your improved version of the Clausius-Clapeyron equation to calculate a more reliable value for the vapour pressure of water at 308 K.
A rigid vessel contains 0.014 m3 of saturated-vapor steam in equilibrium with 0.021 m3 of saturated-liquid water at 373.15 K (100°C). Heat is transferred to the vessel until one phase just disappears, and a single-phase remains. Which phase (liquid or vapor) remains, and what are its temperature and pressure? How much heat is transferred in the process?
Melting enthalpy of ice at 1 bar 9.134 kJ /mol; At 0 ° C, the density of water is 999.9 kg m-3, and the density of ice is 812.0 kg m-3. Assuming that the molar volume and enthalpy change in fusion are constant, find the freezing point of water at 85 bar using the information given?
The latent heat of fusion (∆H fus) of water at 0 °C is 6.025 KJ/mole and the molar heat capacities (Cp,m) of water are 75.3 for the liquid state and 37.7 for the solid state (or ice) - both in J/(K–mole). The Cp values can be taken to be independent of temperature. Considering these information and a kilogram of pure, liquid water at 25 °C, answer the questions that follow. (A). Calculate the ΔH (in KiloJoules) required to cool 1.0-Kg liquid water at 25°C to 0°C (in KJ). (B). Calculate the ΔH (in KiloJoules) required to freeze 1.0-Kg liquid water at 0°C to ice (in KJ) (C). Calculate the ΔH (in KiloJoules) required to supercool 1.0-Kg ice at 0°C to -10.0°C (D). Calculate the total ΔH (in KiloJoules) for the freezing of 1.0-Kg of liquid water initially at 25°C supercooled to –10.0 °C (in KJ)
The pressure of the saturated vapor of benzene (vapor in equilibrium with liquid) is 101.32 kPa at 80°C and 4.81 kPa at 5.5°C, respectively. The latter pressure and temperature correspond to the triple point of benzene. Calculate the approximate molar heat of vaporization ∆Hmv of benzene (Clausius - Clapeyron equation).
A certain ideal heat engine uses water at the triple point as the hot source and an organicliquid as the cold sink. It withdraws 2.71 kJ of energy as heat from the hot source andgenerates 0.71 kJ of work. What is the temperature of the organic liquid?
Calculate the standard enthalpy of vaporization of methylbenzene (see question 1) at the standard boiling point (383.6 K), given that the molar volumes of the liquid and vapour at the standard boiling point are 0.12 dm3/mol and 30.3 dm3/mol, respectively
The latent heat of fusion (∆H fus) of water at 0 °C is 6.025 KJ/mole and the molar heat capacities (Cp,m) of water are 75.3 for the liquid state and 37.7 for the solid state (or ice) - both in J/(K–mole). The Cp values can be taken to be independent of temperature. Considering these information and a kilogram of pure, liquid water at 25 °C, answer the questions that follow. Calculate the total ΔH (in KiloJoules) for the freezing of 1.0-Kg of liquid water initially at 25°C supercooled to –10.0 °C
A solution containing 1.470 g of dichlorobenzene in 50.00 g of benzene boils at 80.60 degree C and a pressureof 1.00 bar. The boiling point of pure benzene is 80.09 degree C, and the molar enthalpy of vaporization of purebenzene is 32.0 kJ/mol. Determine the molecular mass of dichlorobenzene
The solid–liquid equilibrium line in the phase diagram of water has a negative slope, equal to −0.0076 °C bar−1. Calculate the freezing point of water beneath a glacier that is 3 km high and has a density of 917 kg/m3.
Carbon tetrachloride melts at 250 K. The vapor pressure of the liquid is 10539 Pa at 290 K and 74518 Pa at 340 K. The vapor pressure of the solid is 270 Pa at 232 K and 1092 Pa at 250 K. Calculate the normal boiling point and ∆Svaporization at the boiling point and calculate the triple point pressure and temperature.

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