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- A 20-cu ft tank at 100 degrees F is pressured to 200 psia with a pure paraffin gas. Ten pounds of ethane are added, and the specific gravity of the gas mixture is measured to be 1.68. Assume that the gases act as ideal gases. What was the gas originally in the tank?a cylinder was connected to an open ended U-tube (1 atm) containing some mercury, Hg (density=13.6gcm^-3), and the Hg was displaced 100mm towards the container. What is the pressure of the gas inside the container?Calculate the number density (amg) for an ideal gas at 20 kPa and 300.15 K.
- Argon is confined in a 2.4-gallon vessel, determine this mass of Argon at normal room temperature condition and 33.8 in Hg. Calculate the molar composition and partial pressures of a gas mixture that is 28%wt CO2, 12%wt CO, 5%wt water vapor, 30%wt N2 and the rest O2 at 28°C and112 kPa.A chimney gas has the following composition by volume: 9.5% C02, 0.2% CO, 9.6% O2 and 80.7% N2. Using the ideal gas law, calculate a. its composition by weightb. Volume occupied by 1 kg of the gas at 270C and 750 torrsc. density of the gas mixture (kg/m3) at conditions of b)d. specific gravity of the mixture.At low pressures, the compressibility factor of a van der Waals gas is given by the equation: Z = 1+ (b-a/RT) P/RT Calculate ΔG (in units J/mol) associated with the isothermal compression of nitrogen gas at 298 K from 10 bar to 25 bar. The van der Waals constants of nitrogen gas are a = 1.408 L^2-bar-mol and b = 0.03913 L-mol^-1
- Determine the specific weight, specific gravity, and mass of the natural gas (80% methane, 15% ethane and 5% propane) in a 2-m diameter cylindrical tank that is 5.4-ft long at 1.35 bar and 113°F.A gas mixture at 300K and 200kPa consists of 1kg of CO2 and 3kg of CH4. Determine the partial pressure of each gas1. A perfect gas undergoes compression at constant temperature, which reduces its volumeby 3.08 dm3. The final pressure and volume of the gas are 6.42 bar and 5.38 dm3, respectively. Calculate the original pressure of the gas in (a) bar, (b) atm. 2. Consider an isothermal column of an ideal gas at 25oC. What must be the molar mass ofthis gas be if the pressure is 0.80 of its ground level value at (a) 10km and (b) 1km ? Please show complete solutions
- Treat CO2 as an ideal gas and compute q, w, DH, and DU for its inhalation at a constant 1 bar pressure. The temperature outside the body is 15 °C and body temperature is 37 °C. Assume that the volume of air after inhalation (in the lungs) is 500 cm3 and that the concentration of CO2 in the atmosphere is 383 ppm (parts per million).A gas mixture at 300K and 1 bar analyzing by volume 20% N2 and 80% CH4 is subjected to liquefaction at the rate of 1500 kg/hr. It is found that only 30% (weight) of the entering gas is liquefied and the concentration of N2 in the liquid is 60% by weight. The unliquefied gas leaves the unit at 273K and 1 bar. Determine (a) the volume of the unliquefied gas, m3/hr (b) the composition of the gas leaving expressed as volume %.7. Two vessels A and B of different sizes are connected by a pipe which valve. A pipe with a valve. Vessel A contains 142 L of air at 2,767.92 kPa, 93.33 OC. Vessel B, of unknown volume, contains air at 68.95 kPa, 4.44 OC. The valve is opened and, when the properties have been determined, it is found that the pressure and temperature of the mixture of gasses is 1378.96 kPa, and 43.33 OC. What is the volume of vessel B. Use R = 287.08 Joules/Kg-KO for Air