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Unformatted text preview: 97-2 Physical Chemist ry 1st Exam
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) (10pt) : (5pt) 2. (a) Define Ideal Gas and Real Gas (b) Calculate the pressure exerted by 1.0 mol of C2H6 (g), under 273.15 K in 22.5 dm3, behaving as (i) a perfect gas, (ii) a van der Waals gas. (For C2H6 gas a=5.507 dm6 atm mol-2 and b= 0.0651 dm3 mol1 (10pt) ) (c) Calculate the compression factor base on these calculations. Which is the dominate interaction in this gas, repulsive of attractive force? (5pt) b, c) ¶ Ë (ˆ Ã 3. At 500 ℃ and 92.3 kPa, the mass density of sulfur vapor is 37.10 kg m-3, what is the molecular (10pt) formula of sulfur under this condition? (a ) 4. A vessel of volume 22.4 dm3 contains 2.0 mol H2 and 1.0 mol of N2 at 273.15 K. Calculate the mole (10pt) fractions and partial pressure of each gas. (a ) 5. (a) Define Boyle Temperature, TB, of a real gas. (5pt) (b) Prove that TB = a/Rb for van der Waals gases. (10pt) (c) Use van der Waals parameters for chlorine (a=6.260 dm6 atm mol-2, b=0.0542 dm3 mol-1) to estimate (i) Boyle Temperature, TB, (ii) the radius of chlorine molecule regarded as a sphere. (10pt) c) ¶ Ë (ˆ Ã 6. (a) Define critical point of a real gas. (5pt) (10pt) (b) Prove that Vc=3b and Zc=3/8 for a van der Waals gas. (c) The critical constants of methane are Vc=98.7 cm3 mol-1, Pc=45.6 atm , and Tc=190.6 K. Calculate (i) van der Waals parameters (ii) the radius and (iii) Boyle temperature of methane. c) (15pt)¶ Ë (Ã ˆ 97-2 Physical Chemist ry 1st Exam
: : : 7. Calculate the work done by isothermal expansion of 1.00 mol Ar at 0°C from 22.4 dm3 to 44.8 dm3 , (15pt) if the process is: (a) reversibly, (b) against a constant external pressure equal to the final pressure of the gas, (c) freely expansion. (a ) 8. ( (a) É qÀ ºÉ qÀ ) (10pt) (b) a, b. (a) 21 A ¢ (c) a A, B, C, D,?ªE,¹ Õ F x ñ ...
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