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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 mixture
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- The combustion gases from an industrial furnace using a hydrocarbon fuel and dry air enter the stack gas at normal barometric pressure and 3750F and have the following Orsat analysis: 12.2% CO2, 3.1% O2, 1.2% CO, and 83.5% N2. Determine the following: (a) The percent excess air (b) The volume of gases entering the stack, expressed as cubic feet per pound of carbon burnt in the furnace (c) The dew point of the stack gas (d) The atomic ratio of hydrogen to carbon in the fuel (e) The mol of stack gas per atom of carbon burntThe liquefied petrolieum gas(LPG) is composed of 80% C;Hg and 20% C4H10 in mass basis. (1). Determine the molar fraction of C3H8 and C4H10 in LPG. (2). Determine the stoichiometric air fuel ratio of the LPG. (3). Determine the lower heating value of LPG in kJ/m³ at 25°C and 100 kPa. (4). LPG is mixed with excess air to burn in a boiler at 100 kPa. The CO2 in burned gas is 7% on dry basis. Determine the equivalence ratio of the mixture.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. Answer the following: 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 mixture
- 1. A rigid tank containing 1.36 kg gas mixture of nitrogen and carbon dioxide (each 50% by volume) at 272 kPa and 65°C. Determine (a) molar analysis (or % by mol (b) molecular weight and gas constant of mixture (c) volume of mixture (d ) partial volumes of gases (e ) partial pressures of gases (f) gravimetric analysis (or % by mass) (g ) masses of gases (h) mols of gases (i) specific heats Cp and Cv of mixture (j) specific heat ratio of mixture (k) internal energy of mixture (1) enthalpy of mixture Use subscripts: 1 = nitrogen (N,) 2 = carbon dioxide (CO,) no subscript = gas mixture From Table A-1 Specific Heats in kJ/kg K Cp, = 1.0414 Carbon dioxide Cp; = 0.8452 Nitrogen %3D %3DAn experiment on the growth rate of certain organisms requires an environment of humid air enriched in oxygen. Three input streams are fed into an evaporation chamber to produce an output stream with the following composition. (A) Liquid water, fed at a rate of 20.0 cm³/min (B) Air (21% mole % 02, the balance N2) (C) Pure oxygen, with a molar flow rate one-fifth of the molar flow rate of stream B The output gas is analyzed and is found to contain 1.5 mole % water. Calculate the molar flowrate of all unknown stream variables.1. A wet gas from a field in Iran is processed through two stages of separation; first stage separator operates at 220 psia and 71°F, while the stock tank operates at atmospheric pressure and 69°F. The separator gas condensate ratio is 41,000 scf/STB and the stock tank gas condensate ratio is 450 scf/STB. The molecular weights of the separator gas and stock tank gas are 25.0 and 35.0 lb/lb-mol, respectively. The stock tank condensate gravity is 0.85 and its molecular weight is 125 lb/lb-mol. Let us calculate the specific gravity of the reservoir gas in a step-wise manner, by considering quantities for one STB of condensate. Note that 1.0 bbl is 5.614 ft. Separator gas MWsg = 25 lb/lb-mol 41,000 scf/STB Reservoir gas 1st stage separator 220 psia and 71°F Stock tank gas MWsg = 35 lb/lb-mol 450 scf/STB 2nd stage separator (Stock tank) 14.7 psia and 69°F MW=125 lb/lb-mol SGstc = 0.85 Stock tank condensate a. to one STB. Calculate the mole number [lb-mole] of the stock tank condensate that…
- 20. A mixture consisting of 6 kg of O, and 9 kg of N, has a pressure of 3 bar and temperature of 20°C. For the mixture determine the following : (i) The mole fraction of each component ; (iii) The specific gas constant; (v) The partial pressures and partial volumes. (ii) The average molecular weight ; (iv) The volume and density; [Ans. (i) 0.3684, 0.6315 ; (iüi) 29.475 ; (iii) 0.282 kJ/kg K ; (iv) 4.13 m?, 3.629 kg/m² ; (v) 1.1 bar, 1.894 bar ; 1.52 m², 2.61 m²)P1A.6 The molar mass of a newly synthesized fluorocarbon was measured in a gas microbalance. is device consists of a glass bulb forming one end of a beam, the whole surrounded by a closed container. e beam is pivoted, and the balance point is attained by raising the pressure of gas in the container, so increasing the buoyancy of the enclosed bulb. In one experiment, the balance point was reached when the fluorocarbon pressure was 327.10Torr; for the same setting of the pivot, a balance was reached when CHF3 (M = 70.014 g mol−1) was introduced at 423.22 Torr. A repeat of the experiment with a di erent setting of the pivot required a pressure of 293.22 Torr of the uorocarbon and 427.22 Torr of the CHF3. What is the molar mass of the fluorocarbon? Suggest a molecular formula.To evaluate the use of renewable resources, an experiment was carried out with rice hulls. After pyrolysis, the product gas analyzed 6.4% CO2, 0.1% O2, 39% CO, 51.8% H2, 0.6% CH4, and 2.1% N2. It entered a combustion chamber at 90 °F and a pressure of 35.0 in. Hg and was burned with 40% excess air (dry) at 70 °F and an atmospheric pressure of 29.4 in. Hg; 10% of the CO remains. a. How many cubic feet of air were supplied per cubic foot of entering gas? b. How many cubic feet of product gas were produced per cubic foot of entering gas if the exit gas was at 29.4 in. Hg and 400 °F?
- 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 %.Alnu tme rest Hitroģen (N2). Calculate: (i) Composition of the gas by mass. (ii) Average molecular weight. (iii) Density of the gas at 30°C and 200 kN/m². 3.60 A mixture of gas has the following composition by volume: Methane = 80% Ethane = 12% and Nitrogen = 8%. Calculate: (i) The composition of gas by weight%. (ii) Average molecular weight. (iii) Density of the gas mixture at 30°C and 750 mmHg. (iv) Specific gravity. 3.61 A by-product of coke oven produces 30,000 m3 of gas per hour having the following analysis: C6H6 = 5% CHs = 5% CH4 = 40% CO = 7% H2 = 35% CO2 = 5% N2 = 3% The gas leaves the oven at 1.4 atm and 390 °C. After cooling to 40°C, the benzene and toluene are completely removed by absorption. Calculate: (i) Average molecular weight of the gas entering the absorber. (ii) Weight of gas leaving the oven per hour. (iii) Volumetric composition of the gas leaving the absorber. (iv) Weight of benzene and toluene absorbed.P1A.6 The molar mass of a newly synthesized fluorocarbon was measured in a gas microbalance. is device consists of a glass bulb forming one end of a beam, the whole surrounded by a closed container. The beam is pivoted, and the balance point is attained by raising the pressure of gas in the container, so increasing the buoyancy of the enclosed bulb. In one experiment, the balance point was reached when the fluorocarbon pressure was 327.10Torr; for the same setting of the pivot, a balance was reached when CHF3 (M = 70.014 g mol−1) was introduced at 423.22 Torr. A repeat of the experiment with a di erent setting of the pivot required a pressure of 293.22 Torr of the uorocarbon and 427.22 Torr of the CHF3. What is the molar mass of the fluorocarbon? Suggest a molecular formula.