(a)
Interpretation:
Prove that the relative volatilities of species A and B is equal to the vapor ratio of vapor pressure at the system temperature.
Concept introduction:
The Raoult’s law can be written as,
Where, x and y represent mole fractions of component in liquid and vapor, P is total pressure and P* is the vapor pressure.
(b)
Interpretation:
Determine the relative volatility of styrene to ethylbenzene and relative volatility of benzene to ethylbenzene. Which pair is difficult to separate by distillation.
Concept introduction:
The Raoult’s law can be written as,
Where, x and y represent mole fractions of component in liquid and vapor, P is total pressure and P* is the vapor pressure.
(c)
Interpretation:
Prove the given expression is valid.
Concept introduction:
The Raoult’s law can be written as,
Where, x and y represent mole fractions of component in liquid and vapor, P is total pressure and P* is the vapor pressure.
(d)
Interpretation:
Estimate the mole fraction of benzene in the vapor phase in equilibrium with liquids having given benzene mole fractions. Calculate the total system pressure.
Concept introduction:
The Raoult’s law can be written as,
Where, x and y represent mole fractions of component in liquid and vapor, P is total pressure and P* is the vapor pressure.
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EBK ELEMENTARY PRINCIPLES OF CHEMICAL P
- 2. A polynomial fit to measurements of the molar volume of a binary mixture of A and B is: y = -6.6864x² + 60.067x + 22.764 where y = V (cm³ mol·1), x = xXA, and xẠ is the mole fraction of A. What are the partial molar volumes of A and B at xA = 0.5? 3. The partial molar volumes of propanone (acetone) and trichloromethane (chloroform) in a mixture in which the mole fraction of CHCI3 is 0.4693 are 74.166 cm³ mol-i and 80.235 cm³ mol-1, respectively. What is the volume of a solution of mass 1.000 kg?arrow_forwardThe following temperature/composition data were obtained for a mixture of two liquids A and B at 1.00 atm, where x is the mole fraction in the liquid and y the mole fraction in the vapor at equilibrium 140 125 130 135 145 150 ТРС 0.91 0.65 0.45 0.30 0.18 0.098 ХА 0.99 0.91 0.77 0.61 0.45 0.25 The boiling points are 124 °C for A and 155 °C for B a) Plot the temperature composition diagram for the mixture. b) What is the composition of the vapor in equilibrium with the liquid of composition (i) 0.50, and (ii) x = 0.33? ХАarrow_forwardIn the gas phase reaction 2 A(g) + B(g) 3 C (g) + 2 D (g), it was found that when 1.00 mol A, 2.00 mol B and 1.00 mol D were mixed and allowed to come to equilibrium at 25°C, the resulting mixture contained 0.9 mol C at a total pressure of 1.00 bar. Calculate the mole fractions of each species , Kx is , Kp is and A GO isarrow_forward
- 7. Assume that the data in the table below stems from a liquid mixture that obeys Raoult's law. mole fraction p(MBenzene)/Torr p(Benzene)/Torr Total x(Methylbenzene pressure/Torr 0 0.30 0.45 0.61 0.84 1 0 7.19 (ii) 14.90 (iv) 25.02 80.00 (i) 43.57 (iii) 11.90 a) Estimate the missing values. b) Estimate the total pressure for each composition. c) Determine which component is more volatilearrow_forwardIn the gas phase reaction 2 A(g) + B(g) ⇋ 3 C (g) + 2 D (g), it was found that when 1.00 mol A, 2.00 mol B and 1.00 mol D were mixed and allowed to come to equilibrium at 25oC, the resulting mixture contained 0.9 mol C at a total pressure of 1.00 bar. Calculate the mole fractions of each species , Kx is , Kp is and isarrow_forwardWhen ethanol is added to water at 25 °C and 1 bar, the total volume of the solution changes according to the empirical function cm x - 0.36394 cm (mol EtOH) = ** V = 1002.93 cm + 56.6664 mol EtOH cm (mol EtOH) + 0.028256- where x is the number of moles of ethanol in the solution. As ethanol is added to the solution, the partial molar volume of ethanol decreases, reaches a minimum, and then increases. This behavior is shown in the figure below. Find the function for (ma) find the value x = ng 56 Ong TP How many moles of ethanol are present when the partial molar volume of ethanol in the solution is minimum? How many moles of water are present if the mole fraction of ethanol with this amount of ethanol present is 0.0952? 53 5. *- nmol 10 Is the partial molar volume of water increasing, decreasing with increasing x, at a maximum or at a minimum? Explain based on an equation based on an equation from the lecture slides. Partial melar volume, VAcm motarrow_forward
- 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 0.164arrow_forwardWhat is AG for the decomposition of CaCO3 at 298 K and a partial pressure of CO2 of 4.00x10-4 bar? CaCO3(s) → CaO(s) + CO2(g) AGrxn (298 K, Pco2 = 0.400 mbar) = ??? CO2(g) Compound AG°; (kJ mol·1) CACO3(s) СаО(s) -1129 -604 -394arrow_forward3. A 12.0 cm3 sample of liquid H2O (density 1.00 g.cm-3) is heated to 328 oC under an external pressure of 0.8 atm, conditions under which it vapourises: (i) Calculate the volume of the gas. (ii) Calculate the mass of the same volume (as in part i) of CO2 gas under the same conditions. (iii) Calculate temperature of that sample of CO2 (as in part ii) at 8.0 atm pressure in a 20.0 L container.arrow_forward
- Underwater, the pressure increases by 1 bar for every 10 m of depth. When a scuba diver breathes pressurized air in which the partial pressure of N2(g) exceeds 4 bar, the result is nitrogen narcosis, which is similar to alcohol intoxication. What is the maximum mole percent of N2 in an air mixture that could be used by divers at depths up to 85 m below sea level without undue risk of nitrogen narcosis?arrow_forwardC6H5Cl e C6H5Br form nearly ideal mixtures. At 136.7◦ C the vapor pressure of C6H5Cl is 1.137 bar, while that of C6H5Br is 0.604 bar. Which is the composition of the mixture for which the total vapor pressure is 1 bar ?arrow_forwardAnswer Q48, 49, 50arrow_forward
- Introductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage Learning