look for critical parameters and calculate its molar volume using the real gas equation of states at 2 atm pressure and temperatures a.) T>Tc b.) T = Tc c.) T< TC of Carbon Dioxide. Describe the volume obtained.
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look for critical parameters and calculate its molar volume using the real gas equation of states at 2 atm pressure and temperatures a.) T>Tc b.) T = Tc c.) T< TC of Carbon Dioxide. Describe the volume obtained.
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- stack gas analysis: 83.08% N2, 7.5% CO2, 2.3% CO, 1.12% H2, 6% O2 with a saturation temperature of 54°C at 400°C and 760mmHg. a) %excess of air (1000 m^3 of air is supplied, produced 3100 m^3 of stack gas) b) chemical formula of the fuel burned c) analysis of the fuel mixtureCalculate the partial pressure (Pa) of CO2 in a mixture that contains 45% wt CO2, 35% wt CO and 20% wt O2 at 100 deg C and 1.5 atm.The gas A(g) (1 mole) undergoes a two-step process one after another as described below :i) The gas is expanded at 25°C and from 1 bar pressure against a constant pressure of 0.2 bar and the final volume of the gas is the twice the initial volume.ii) The gas is cooled down to -25°C at constant volume.Cv,m = 3/2 RCalculate ΔU, ΔH, q and w for the each step and for the entire process
- The total pressure of a mixture of oxygen and hydrogen is 1.00 atm. The mixture is ignited, and water is removed. The remaining gas is pure hydrogen and has pressure at P = 0.400 atm when measured at the same T and V as the original mixture. What is the composition of the original mixture in mole percent?What is the final pressure, in atmospheres, when the fire extinguisher is used at a temperature of 71 ∘C∘C, if VV and nn are constant? Express your answer using two significant figures.Producer gas is a fuel that is manufactured from the reaction of coal, steam and air. A producer gas has the following composition by volume (dry basis): 20.35% CO, 11.03%, CO2, 15% H2, 51.43% N2, 1.98%O2 and 0.21 % CH4. The gas is flowing at 6000 cfm. It has a temperature of 200℃ , a pressure of 21 cm Hg and a partial pressure of 50 mm Hg for H2O. The atmospheric pressure is 758 mm Hg. The gas is delivered from the source to the furnace by means of a pipe. It cools down to 50 ℃ and is compressed to 2 atm pressure. At this condition, calculate:1. the volumetric flow ate2. the mass flow rate3. the partial pressure of each component/including water)4. complete analysis of the mixture
- 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.Gypsum (plaster of Paris : CaSO,. 2H,0) is produced by the reaction of calcium carbonate and sulfuric acid. A certain lime stone analyzes: CaCO, 96.89 %; MgCO, 1.41 %; inerts 1.70 %. For 5 metric tons of limestone reacted completely, determine: a. kg of anhydrous gypsum (CaSO,) produced. b. kg of sulfuric acid solution (98 wt%) required.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 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.Calculate the density of combustion gases with the following composition: 75% N2, 5.5% O2 ,11% CO2, 84% H2O, and 0,1% CO. The temperature is 350 oF and the pressure is 755 mm Hg,If 15.1 g of the mixture with a volumetric composition of 45% N2, 35% O2 and 20% X gas is applying 3 atm pressure to a 5 dm3 volume vessel at 25 ° C, in which option is the molecular weight of X gas given correctly? (MN2: 28 gmol-1, MO2: 32 gmol-1)