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- P1C.4 Calculate the volume occupied by 1.00 mol N2 using the van der Waals equation expanded into the form of a virial expansion at (a) its critical temperature, (b) its Boyle temperature. Assume that the pressure is 10 atm throughout. At what temperature is the behaviour of the gas closest to that of a perfect gas? Use the following data: Tc = 126.3 K, TB = 327.2 K,a = 1.390 dm6 atm mol−2, b = 0.0391 dm3 mol−1.To prevent tank rupture during deep-space travel, an engineering team is studying the effect of temperature on gases confined to small volumes. What is the pressure of 2.00 molmol of gas DD measured at 251 ∘C∘C in a 1.75-LL container assuming ideal behavior?Use the virial equation of state to calculate the pressureexerted by 1.00 mol CH4, at 273 K confined to a volumeof 1.00 cm3, given the value of the second virial coefficient.B = -53.6 cm3 mol·'. at this temperature. You may assumethat the expansion may be truncated after the second term.
- (a) Using the Lennard-Jones parameters, determine the van der Waals radius for xenon. (ɛ and o for xenon are 1.77 kJ•mol-1 and 4.10 Å, respectively.) 4.0 (b) Use this radius to determine the fraction of the volume occupied by 1.22 mol of xenon at 25°C and 1.00 atm. 4.0 Supporting MaterialsThe energy of the van der Waals bond, which is responsible for a number of the characteristics of water, is about 0.50 eV. (a) At what temperature would the average translational kinetic energy of water molecules be equal to this energy? (b) At that temperature, would water be liquid or gas? Under ordinary everyday conditions, do van der Waals forces play a role in the behavior of water?To prevent tank rupture during deep-space travel, an engineering team is studying the effect of temperature on gases confined to small volumes. What is the pressure of 2.00 molmol of gas DD measured at 251 ∘C∘C in a 1.75-LL container assuming real behavior?
- Given the constant for H 2 (g)+l 2 (g) 2Hl(g) at 427 degrees C . At same temperature, complete the Table below.Calculate the amount of energy in the form of heat that is produced when a volume of 4.37 L of SO2(g) is converted to 4.37 L of SO3(g) according to this process at constant pressure and temperature of 1.00 bar and 25.0 ° C. Assume ideal gas behavior.Calculate the pressure exerted by 1.0 mol C2H6 behaving as (a) a perfect gas, (b) a van der Waals gas when it is confined under the fol lowing conditions: (i) at 273.15 K in 22.414 dm3 , (ii) at 1000 K in 100 cm3. Use the data given.
- Cylinders of compressed gas are typically filled to a pressure of 200 bar. For oxygen, what would be the molar volume at this pressure and 25 °C based on (i) the perfect gas equation, (ii) the van der Waals equation? For oxygen, a = 1.364 dm6 atm mol−2, b = 3.19 × 10–2 dm3 mol−1.2. A sample of vapor weighing 0.368 g filled a Florence flask when heated in a water bath at 95.0°C. The actual volume of the flask was 128.4 mL and the barometric pressure was 747 torr. Calculate (a) the volume of the vapor at STP and (b) the molar mass of the volatile liquid. (Use the approach applied in the Introduction and on the data sheet.)Calculate the mean free path of carbon dioxide molecules using σ = 0.52 nm2 at 25°C and (a) 15 atm, (b) 1.0 bar, (c) 1.0 Torr.