At 300K and 1 bar the volumetric data for a liquid mixture of benzene and cyclohexane are represented by V = 109.4 x 106 - (16.8 x 10 6) x – (2.64 x 10 6) x² where x is the mole fraction of the benzene and V has the units of mmol. Find the partial molar volumes of benzene and cyclohexane for x-02 O a. 50x10-6 m³/mol; 78.9x10-6 m³/mol Ob. 91.6x10-6 m³/mol; 109.5x10-6 m³/mol O c. 75.6x10-6 m³/mol; 98x10-6 m³/mol O d. 100x10-6 m/mol; 108x10-6 m³/mol

A liquid mixture is made of 15 kg Benzene (MW= 78), 30 kg Toluene (MW=92) and 15 kg Xylene (MW=106) the average molecular weight of this mixture is: Answer:

Oxygen is contained in a cylinder at a pressure of 95 bar and a temperature of 185.52 K. Estimate the molar volume in units ?^3/??? and the specific volume in units ?^3/?? using : (a) The ideal gas equation of state (b) Van der Waals equation of state (c) Redlich-Kwong equation of state (d) Lee Kesler correlation Argue why oxygen is a real gas under these conditions. Evaluate the accuracy of each correlation.

QUESTION 1 Calculate the pressure exerted by Ar for a molar volume 0.39L at 265K using the van der Waals equation of state. The van der Waals parameters a and b for Ar are 1.355 bar dm6 mol-2 and 0.0320 dm³mol-1, respectively. Please write your answer (unit: bar) round to 1 decimal places, as 12.2. Please do not add unit to your answer.

(a)Using the compressibility chart, determine the compression factor (Z). Express your final answers in 3 significant figures (b)What would be the corresponding state of carbon dioxide? (Pc = 72.9 atm, Tc = 304.2 K) T (K) 200 P (atm) Tс (К) Pc (atm) Gas Argon 23.0 150.7 48.0 1.1 1.0 T- 2.00 0.9 I=1.50 0.8 Tx =1.30 0.7 to 0.6 T=1.20 0.5 T-1.10 0.4 Legend: X Methane O Ethylene A Ethane O Propane O n-Butane Iso-pentane • n-Heptane A Nitrogen T =1.00 0.3 Carbon dioxide Water 0.2 Average curve based on data on hydrocarbons 0.1 0.5 1.0 1.5 2.0 2.5 3.0 3.5 4.0 4.5 5.0 5.5 6.0 6.5 7.0 Reduced pressure P x of x

PHYSICAL CHEMISTRY:Calculate the pressure exerted by 1.0 mol C2H6 at 1000 K in 100 cm3 using (a) the ideal gas equation and (b) the van der Waals equation. The van der Waals constant for C2H6 are: a = 5.562 bar dm6 mol-2 ; b = 0.06380 dm3 mol-1 answer:[831; 1.72 x 10-3]

Consider cyclohexane at 175ºC. Determine Z and V (cm^3/mol) when P = 8.74 bar (saturated liquid)

6) Calculate the absolute entropy for 1 mole of Ar gas (monatomic) with 22.4 liter volume at 273 K using Boltzmann's formula. What is the change in entropy if the temperature doubles while V is constant? What is the change in entropy if the volume doubles while T is constant? What is the change in entropy if both T and V double? (Note: To evaluate In(N!) use Stirling's asymptotic formula In(N!) ~ N In N – N ) S-k log W LVDWIG BOLTZMANN 18W-1906 DE FHILPAULA BOLTZMANN GER CAR