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- a) Calculate the volume in ft of one Ib-mole of air (MW = 29 lbm/lb-mole) at a temperature of 492 R at a pressure of 1 atm (absolute). b) Repeat the calculation of a) but now considering 1 Ib-mole of CO2 (MW= 44 lbmlb-mole). c) Calculate the molar volume (V) of this mole of air in ft'/lb-mole. d) Calculate the density (P) of air in Ibm/ft under these conditions e) Calculate the density (p) of CO, in Ib.m/ft under these conditionsThe ideal gas law relates the pressure P, volume V, and temperature T of an ideal gas: PV = nRT where n is the number of moles and R = 8.3145 J/(K mol). Plots of pressure versus volume at constant temperature are called isotherms. Plot the isotherms for one mole of an ideal gas for volume ranging from 1 to 10 m', at tempera- tures of T = 100, 200, 300, and 400 K (four curves in one plot). Label the axes and display a legend. The units for pressure are Pa. n=1What is the volume of a container that holds exactly 1 mole of anideal gas at standard temperature and pressure (STP), defined asT = 0°C = 273.15 K and p = 1 atm = 1.013 * 105 Pa?
- Problem 3. The viral coefficients of a gas at 20 °C and 11.5 bar are B = -138 cm³ mol¹ and C=7222 cmº mol². Calculate the V (molar volume) Z (compressibility factor) of the gas. Use the equation below (R = 83.14 cm³ bar mol-¹ K-¹). PV 2 = ² = (1 + = + =) Z RTA given gas is heated from 273 K to 546K, while its volume is doubled. If initially the gas pressure is 4 x 105 Pascal, the final pressure is: A-P = 4 × 105 Pascal B- P = 2 x 105 Pascal C- P = 1 × 105 Pascal D- P = 0.5 x 105 Pascal E- P = 0.25 x 105 Pascal O A Ос D ОЕQ/ Calculate the Vanderval temperature of a gas with a value of a = 1.35 dmemol 7atm b = 0.0322 dm * mol1 if 2 moles %3D of gas occupy 51.5 liters at one atmosphere
- mol K 1) The Ideal Gas Law, PV = RT, relates the pressure (P, in pascals), temperature (T, in Kelvin), and volume (V, in cubic meters) of 1 mole of a gas (with R = 8.314 as the universal gas constant), and describes the behavior of gases that do not liquefy easily, such as oxygen and hydrogen. We can solve the ideal gas law for volume and hence treat the volume as a function of the pressure and temperature: V(P,T) = 8.314T P 1000 tells us about a key relationship between a) Explain in detail what the trace of V with P two quantities. b) Explain in detail what the trace of V with T = 5 tells us. c) Explain in detail what the level curve V = 0.5 tells us. d) Use 2 or 3 additional traces in each direction to make a rough sketch of the surface over the domain of V where P and T are non-negative. Write at least one sentence that describes the way the surface looks. e) Based on all your work above, write a couple of sentences that describe the effect that temperature and pressure have on…A gas consists of NO₂ molecules at temperature T. What is the r.m.s. speed of the molecules, in m/s? The mass of an NO₂ molecule is 1.53x10-26 kg. T = 10 °C; (in m/s) OA: 639.3 OB: 747.9 OC: 875.1 OD: 1023.8 OE: 1197.9 OF: 1401.5 OG: 1639.8 OH: 1918.6The average speed of a gas molecule in meters per second is ????=8????⎯⎯⎯⎯⎯⎯⎯√,vavg=8RTπM, where the temperature ?T is given in kelvins, the molar mass ?M is given in kilogram–moles, and ?=8.31.R=8.31. Calculate ???????dvavgdT at ?=300 KT=300 K for oxygen, which has a molar mass of 0.032 kg/mol.
- XEx. 27: Find the density of nitrogen at N.T.P. (Given : M.W. of nitrogen = 28) P= 1.013 x 105 /m² R = 8.314 J/mole KWhen air expands adiabatically (without gaining or losing heat), its pressure P and volume V arerelated by the equation:P V 1:4 = C, where C is a constant.Suppose that the pressure is decreasing at a rate of 10 kPa/min. Determine the rate of change in volume (incm3/min) at the point when pressure is 80 kPa, given that C = 235 000. SEE IMAGEFor steam at a pressure of 45 atm, some values of tempera- ture and specific volume are as follows, T, °F 600 600 500 700 800 900 у, RлЬт Find an average value of the predicted gas constant R in m/(s . K). Does this data reasonably approximate an ideal zas? If not, explain. 0.7014 0.9653 0.8464 1.074 1.177