Calculate w, q, DU, and DH for 1.0 mol of liquid water at 373 K changing to vapor at constant pressure of 1 bar. The molar volume of liquid water at 373 K is 1.89 x 10-5 m3 mol-1.
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- 7A A mass m of a perfect gas [C=0.815 KJ/Kg K , cp=1.42 KJ/Kg K] is compressed from 0.85 m' and 105 N/m2 to volume 0. 034 m and pressure 3.0x10 N/m2 the temperature is reduced by AT = 100 K. the gas constant r in kJ/kgK. isThe literalized Boltzmann-Poisson equation considering ionic atmosphere theory of Debye Huckel, for dilute ionic solution is, d do 74) - ² dr dr ɛk BT Σn,(0)z, e²o(r): (symbols have their usual meanings). Find expression of o(r).8. Consider a gas with the equation of state P - RT(1/V+ a/V + b/V). Usually one finds the critical pressure P, critical temperature T, and critical molar volume Vm, in terms of a, b, and R. Here solve for a and b in terms of critical constant(s) and then evaluate the critical pressure. Why can you not determine the critical temperature from the criteria of an inflection point? [a --Vcl
- The diagram below shows some isotherms of water. (a) S Estimate values for the critical constants and the van der Waals constants a and b for this gas. (b) Using the information from part (a), estimate the radius of a water molecule. Compare to the value of 1.37 A obtained from interpolation of ionic radii (Y. Zhang and Z. Xu, American Mineralogist 80 (1995) 670-675). PIMPa C 8 15- 10- M 50 400°C 374°C 350°C 300°C 425°C 450°C 275°C 100 150 200 250 300 350 Vicm mole 400 5001. If C,H3FY vapour diffuses 1.196 times faster than C,H10F2 vapour under the same conditions, show how you determine the values of x & y and the molecular formula of C,H3Fy.For ethane at 298.15 K, B = -186 cm³mol-¹ and C= 1.06x104 cm'mol². Use the formula B PVm = RT [1 1+ + Vm V2 m to calculate the pressure of 28.8 g of ethane in a 999 cm³ container at 298.15 K and the amount of atm in which it is far from the ideal value.
- What mass of H2 gas can be collected over water from a 250-mL flask at a temperature of 25ºC and a pressure of 105.325 kPa? (The vapour pressure of H2O at these conditions is 3.169 kPa.)13. (a) ] Determine the reduced temperature, reduced pressure and reduced molar volume of a sample of argon with a molar volume of 4.518 L at 10.0°C and 3.00 bar pressure. For Ar, T=150.86 K, Vc = 74.57 x 10-³ L, P = 48.98 bar (b) [ Calculate the P and I values for which NH3 is in a corresponding state with Ar. For NH3, Tc=405.40 K, Pc = 113.53 bar1. A vessel of volume 24.4 dm3 contains 1.0 mol H2 and 2.5 mol N2 at 298.15 K. Calculate(a) the mole fractions of each component, (b) their partial pressures, and (c) their totalpressure. 2. The critical constants of carbon dioxide are Pc = 72.85 atm, Vc = 94.0 cm3 mol–1, and Tc =304.2 K. Calculate the van der Waals parameters of the gas. Please provide complete solutions.
- A water Stonge tank contatns liquid and vapour in eguilibruim at ilo2. The distance from bottom of the tank to the liquld level is 8 m. What is the absolute pressure at the bottom of the tank. [218 kpa]A 500.0 mL sealed canister only containing exactly 0.1376 mol of n-pentane (CH3CH2CH2CH2CH3) is heated to 350.0 °C.All of the n-pentane will have vapourized.Use Van der Waal's equation to calculate the pressure.(Pobs+[(n2a)/(V2)])(V−nb)=nRTFor n-pentane: a=19.01 L2 atm/mol2; b=0.146 L/mol. P(obs)=What pressure would exert by 20 g of argon gas (MM-39.95 g mol) in a vessel of volume 2 dm at 40°C if it behaved as a van der Waals gas (R-0.0831 dm bar Kmol).(a-1.354 dm° bar mol and b= 3.20 x 102 dm mol) bar 10.53 bar 8.99 bar 7.75 bar 6.55 O O