Boiling Enthalpy ofpoint vaporization(K) (kJ mol-1)Liquidbenzenetoluene353.130.72383.633.18octane398.734.41chloroform334.229.24n-propanol370.241.44ammonia239.623.35Predict which of the following compounds follow Trouton's rule.Check all that apply.• View Available Hint(s)tolueneammoniachloroformn-propanoloctanebenzene

Trouton's rule states that entropy of vaporisation is almost same value, which is about 85 - 88…

Boiling Enthalpy of point vaporization (К) Liquid (kJ mol 1) benzene toluene 353.1 30.72 383.6 33.18 octane 398.7 34.41 chloroform |п-propanol 334.2 29.24 370.2 41.44 ammonia 239.6 23.35 Predict which of the following compounds follow Trouton's rule. Check all that apply. • View Available Hint(s) toluene ammonia chloroform n-propanol octane benzene

Boiling Enthalpy of point vaporization (К) Liquid (kJ mol 1) benzene toluene 353.1 30.72 383.6 33.18 octane 398.7 34.41 chloroform |п-propanol 334.2 29.24 370.2 41.44 ammonia 239.6 23.35 Predict which of the following compounds follow Trouton's rule. Check all that apply. • View Available Hint(s) toluene ammonia chloroform n-propanol octane benzene

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 6.3E

See similar textbooks

Similar questions

Formula: C3H6OMelting Point: -94.0°CBoiling Point: 56.0°CDensity of liquid: 0.791 g/mLHeat of Fusion: 98.14 J/gHeat of vaporization: 538.9 J/gSpecific heat capacity (solid): 1.653 J/g°CSpecific heat capacity (liquid): 2.161 J/g°CSpecific heat capacity (gas): 1.291 J/g°C How much heat is involved in taking 165.2 g of acetone from 14.7°C to 52.1°C?
Name two characteristic physical properties that distinguish condensed from gas phases, and one which distinguishes solid from liquid phases. Discuss the differences for each property. Name one colligative property and by an equation (label all variables) and 1-2 sentences the physical meaning. Consider a balloon. What thermodynamic system does it represent? How does this system interact with the environment? Calculate the heat capacity at constant pressure of methane for all its contribution and the total value according to the equipartition theorem. What is a more realistic value at room temperature? Why?
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 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?
please answer all the following: How much energy per mole does it take to boil each of the following molecules from starting at standard state ambient temperature, 298 K. Boiling means increase temperature to the boiling point and then converting the liquid to a gas. Assume constant pressure conditions. Use Table 2C.1 to find Tboil and ΔHvap. Use Table 2C.7 to find Cpm values. a. Methanol (CH3OH) b. Ethanol (C2H5OH) c. Water (H2O) d. Which needs the largest amount of energy? What factor has the greater impact on this value?
Butane liquid and vapor coexist at 370.0 K and 14.35 bar. The densities of the liquid and vapor phases are 8.128 mol/ L and 0.6313 mol/L , respectively. Use the van Der Waals equation, the Redlich-Kwong equation and the Peng-Robinson equation to calculate these densities. Use α = 16.44 bar L2 mol-2 and β = 0.07245 L mol-1 for the Peng-Robinson equation. Please show each step and calculations explicitly, particularly how to arrive to the numerical result for the densities
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.
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?
What is w when 1.83 kg of H20(1), initially at 25.0 °C, is converted into water vapour at 185 °C against a constant external pressure of 1.00 atm? Assume that the vapour behaves ideally and that the density of liquid water is 1.00 g/ml (Remember to include a+or-sign as appropriate.) Enter your answer in acceptable SI units, accurate to 3. significant figures. Use an acceptable Sl symbol for units.
Using Soave-Redlich-Kwong Equation calculate the molar volume of saturated liquid and the molar volume of saturated vapor for one of the following and compare results with values found by suitable generalized correlations.(a) Propane at 40°C where put = 13.71 bar
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
Calculate the freezing point of water at 95 bar and 450 bar since the melting point of ice is 0⁰C and the melting enthalpy is 6.010 kJ/mol. (Accept that the densities of water in liquid and solid state are 0.997 G/ and 0.917 g/cm3 and remain constant.)