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- Using the ideal gas law, PV = nRT, determine the volume 200 lbs of hydrogen would occupy at 180 degrees F and a pressure of 100 psig? Assume the constant “R” is 10.731 Ft3PSIA/0R lb mole and the molecular weight of H2 is 2 lbs./mole.A vessel contains an ideal gas with temperature of -15°C, a density of 0.16 kg/m3, and a molecular weight of 4 g/mol. A) What is the pressure of this gas in kPa? B) Its gage pressure? C) If the vessel were punctured which way would gas flow - gas exiting the hole or atmosphere entering the hole? (Ri = 8.314 kg-m2/K-mol-s?)(a) If the partial pressure of water vapor is 8.05 torr, what is the dew point? (760 torr = I atm 101, 325 Pa) (b) On a warn day when the air temperature is 35 and the dew point is 25 , what are the partial of the water in the air and the relative humidity?
- (a) Find the density in SI units of air at a pressure of 1.00 atm and a temperature of 20 , assuming that air is 78% N2, 21% O2, and 1% Ar, (b) Find the density of the atmosphere on Venus, assuming that it's 96% CO2 and 4% N2, with a temperature of 737 K and a pressure of 92.0 atm.A volume of 58.0 L of hydrogen is heated from 33°C to 68°C. If its originald ensity is 4.85 kg/m3 and its original absolute pressure is 120 kPa, what is the resulting density?The density of mercury is 13 600 kg/m3 at 0 oC. What would be its density at 151 oC?
- The 1.8kg gas nitrogen has temperature of 0°C, filled inside 25liter. Calculate the pressure of gas nitrogen. Take gas molecular weight = 28 Please answer in SI unit (even temperature) with no decimals.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 conditions3. A 6m3 tank contains helium at 127 C and in evacuated from atmospheric pressure to a pressure of 740 mm Hg vacuum. Determine (a) mass of helium remaining in the tank (b) mass of helium pumped out (c) the temp of the remaining helium falls to 10 C, what is the pressure in Kpa? R of helium is 2077.67 J/kg-K.
- Ex. 7 hydrogen molecule at 127°C. The density of hydrogen at N.T.P. is 0.09 kg/m³. : Calculate the R.M.S. velocity ofCalculate RM.S. velocity of helium at temperature 0° C. (Density of helium = 0.1785 kg/m³, atmospheric pressure = 1.013 × 105 N/m²).At the bottom of a lake where the temperature is 7.35 oC and the pressure is 3.07 bars the radius of a bubble is 2.11 cm. The bubble ascends to the surface where the pressure is 1.01325 bars and the temperature is 21.60 oC. What is the percent change (with respect to the volume at the bottom) in the volume of the bubble?