(Physical Chemistry Question) 4. The vapor pressures of benzene and toluene have the following values in the temperaturerange between their boiling points at 1 bar;T, °C79.488941001101.5261.801P*(C,H), barP*(C-Hs), bar1.001.2850.5080.6160.7421.00a) Calculate the composition of the vapor and liquid phases at each temperature and plotthe boiling point diagram.dreamstie

The law which states that the partial vapor pressure of solution is equal to the mole fraction…

4. The vapor pressures of benzene and toluene have the following values in the temperature between their boiling points at 1 bar; T, °C P*(CHs), bar | P*(C-Hs), bar range 79.4 88 94 100 110 1.00 1.285 1.526 1.801 0.508 0.616 0.742 1.00 a) Calculate the composition of the vapor and liquid phases at each temperature and plot the boiling point diagram.

4. The vapor pressures of benzene and toluene have the following values in the temperature between their boiling points at 1 bar; T, °C P(CHs), bar | P(C-Hs), bar range 79.4 88 94 100 110 1.00 1.285 1.526 1.801 0.508 0.616 0.742 1.00 a) Calculate the composition of the vapor and liquid phases at each temperature and plot the boiling point diagram.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter17: Spontaneity, Entropy, And Free Energy

Section: Chapter Questions

Problem 128IP: Some nonelectrolyte solute (molar mass = 142 g/mol) was dissolved in 150. mL of a solvent (density =...

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Some nonelectrolyte solute (molar mass = 142 g/mol) was dissolved in 150. mL of a solvent (density = 0.879 g/cm3). The elevated boiling point of the solution was 355.4 K. What mass of solute was dissolved in the solvent? For the solvent, the enthalpy of vaporization is 33.90 kJ/mol, the entropy of vaporization is 95.95 J/K mol, and the boiling-point elevation constant is 2.5 K kg/mol.
The table below shows temperature/composition data collected for a mixture of methylbenzene (M) and octane (O) at 1 atm. Recall that x stands for the mole fraction in the liquid and y stands for the mole fraction in the vapor in equilibrium. The boiling points for methylbenzene (M) and octane (O) are 110.60C and 125.60C, respectively. Construct the phase diagram with Temperature vs. xM. What is the composition of the vapor in equilibrium with the liquid of composition (a) xM = 0.250 and (b) xO = 0.250. T (0C) 110.9 112.0 114.0 115.8 117.3 119.0 121.1 123.0 xM 0.908 0.795 0.615 0.527 0.408 0.300 0.203 0.097 yM 0.923 0.836 0.698 0.624 0.527 0.410 0.297 0.164
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
Since the melting point of ice is 0⁰C and its melting enthalpy is 6.010 kJ/mol, calculate the freezing point depression of water at 95 bars and 450 bars. (Assume that the densities of water in liquid and solid state are 0.997 g/ and 0.917 g/cm3 and remain constant.)
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?
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.)
Consider a pure liquid in equilibrium with its vapor at constant temperature. a) write an expression relating the chemical potential of the liquid, u(l), and vapor, u(g). b) express u(g) in terms of the vapor pressure of the pure liquid, P.
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 mixture of phenol and water, under certain conditions of temperature and composition, forms two separate liquid phases, one rich in phenol and the other rich in water. At 30⁰ the compositions of the upper and lower layers are 70% and 9% by mass phenol, respectively. If 40kg of phenol and 60kg of water are mixed and the layers are allowed to separate at 30⁰C, what will be the weight of the two layers?
The vapour pressure of pyridine is 50.0 kPa at 365.7 Kand the normal boi ling point is 388.4 K. W hat is the enthalpyof vaporization of pyridine?
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.
Steam pressures for pure CCl4 and SiCl4 are given as 0.4226 bar and 0.7999 bar respectively, while the temperature is 50°C. For a mixture prepared with these two liquids and boiling at 50°C under a pressure of 0.5333 bar, find the composition of the phases as a mole fraction and a mass fraction. [M(CCl4):153,82 g/mol, M(SiCl4):169,9 g/mol]