The following data were obtained in a test on coal fired steam generator. The ultimate analysis of coal: C, 80.5%; H, 4.6%; O, 5.0%; N, 1.1%; ash, 8.8%. No carbon is lost in the refuse. The orsat analysis of flue gas: CO2, 16.4%; 02, 2.3%; CO, 0.4%; N2, 80.9%. Calculate (a) The weight of dry gaseous products formed per 100 kg of coal fired (b) The percent excess air supplied for combustion
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- Two-hundred fifty pounds per hour of iron pyrites containing 90% FeS2 and 10% gangue are burned with 20% excess air based on conversion to SO3. The cinder discharged from the burner contains no sulfur. No conversion to SO3 occurs in the burner. The burner gas is passed through a converter which effects a 98% conversion of SO2 to SO3. The converter gas is passed to an absorber where all the SO3 is absorbed by 80% H2SO4 solution, which becomes 100% H2SO4 solution in the process. Establish a basis of one hundred pounds of iron pyrites Calculate: (a) the burner gas analysis, (b) the converter gas analysis, (c) pounds of 100% H2SO4 produced per 24-h day, if waste gas analyzes 0.19% SO2, 4.14% O2 and 95.67% N2Jansen Gas creates three types of aviation gasoline(avgas), labeled A, B, and C. It does this by blendingfour feedstocks: Alkylate; Catalytic CrackedGasoline; Straight Run Gasoline; and Isopentane.Jansen’s production manager, Dave Wagner, hascompiled the data on feedstocks and gas types inTables 4.6 and 4.7. Table 4.6 lists the availabilitiesand values of the feedstocks, as well as their keychemical properties, Reid vapor pressure, and octanerating. Table 4.7 lists the gallons required, theprices, and chemical requirements of the three gastypes. Table 4.6 Data on Feedstocks Feedstock Alkylate CCG SRG Isopentane Gallons available (1000s) 140 130 140 110 Value per gallon $4.50 $2.50 $2.25 $2.35 Reid vapor pressure 5 8 4 20 Octane (low TEL) 98 87 83 101 Octane (high TEL) 107 93 89 108 Table 4.7 Data on Gasoline Gasoline A B C Gallons required (1000s) 120 130 120 Price per gallon $3.00 $3.50 $4.00 Max Reid pressure 7 7 7 Min octane 90 97 100 TEL level Low High High Note that each feedstock…ethylene oxide is produced by oxidation of ethylene 100 kmol of ethylene and 100 kmol of o2 are charged to a reactor.the % conversion of ethylene is 85 and%yield of ethylene oxide is 94.12 .calculate the composition of product stream leaving the reactor .the reactions takes place are
- In the industrial synthesis of aspirin, 200 kg of salicyclic acid, C7H6O3 and 150 kg of acetic anhydride (CH3CO)2O, form acetylsalicylic acid, C9H8O4, (aspirin) and acetic acid, C2H4O2. In a manufacturing process, 200 kg of aspirin are produced from 200 kg of impure salicyclic acid and 150 kg of acetic anhydride. The salicylic acid is the limiting reagent. Calculate the purity of the salicyclic acid. How many kg of excess reagent are left over, assuming there are no side reactions between the impurities in the limiting reagent and the excess reagent?A 0.2500-g of dry CaCO3 was completely dissolved into a solution of 5-mL conc. HCl and 50-mL distilled water in an erlemeyer flask. The resulting solution was boiled for 5 minutes to expel CO2 from the reaction, and then it was cooled to room temperature and the solution was transferred in a 500-mL volumetric flask filled to volume by rinsing the erlenmeyer flask and combining all the washings to fill the mark. A 5.0-mL aliquot of the CaCl2 solution was taken from the orignal solution and was transferred into an erlenmeyer flask with 10-mL NH3 buffer, 20-mL distilled water, and 5 gtts of EBT. The solution consumed 4.96 mL of an EDTA solution. MW: CaCO3 = 100.1 Compute for the N EDTA solution. 0.0053 N 0.0531 N 0.5313 N None of the choices7. Consider a1Msolution ofNa3AsO4. Write the charge and mass balance equations for this system. (please type answer not write by hend)
- So a Flame Test Investigation was conducted. In that activity, short wooden splints (sticks)were soaked in eight different chemical solutions. The splints were then held over a lit Bunsen burner oneat a time, at which time each one gave off a distinctive color of light Each splint produced a dominant, vibrant color, and the color was different for each one. Forexample, the splint soaked in copper chloride produced a green flame and the splint soaked in lithiumchloride produced a brilliant red flame. Please explain the following for me: 1. Why do chemicals give off light when heated by a Bunsen burner? 2. None of the chemicals produced “white light” similar to a common light fixture. In otherwords, none of the chemicals gave off the entire spectrum of visible colors. Why not? 3. Why does each chemical give off its own unique color that is different from every otherchemical? Give thorough explanations. Also, when explaining, correctly use each of the following terms at least…consider the balance to reaction 6 A + 9 B -> 3C + 5D If 6.448 moles of A (MW = 39.34) are consumed, how many moles of B (MW = 42.66) are also consumed?Use your balanced chemical reaction from the above problem. How many kilograms of the barium product can be produced at 100% yield from the double replacement reaction, made in industry at a larger scale of 675.00 pounds of barium nitrate that is then dissolved in water and mixed with an excess of the potassium sulfate solution. The product is collected by gravimetric filtration and dried. Use 453.592 g = 1 lb. Ba(NO3)2 + K2SO4 ---> BaSO4 + 2KNO3
- The analysis of a product of combustion on dry basis, when C6H18 was burned with atmospheric air, is as follows: CO2=12%, CO=1.75%, O2=3.01%, N2=83.24%. Compute the actual air-fuel ratio.A sample containing chlorophenol, C6H4ClOH, was analysed by gravimetric analysis. A 0.783-g of this sample goes through a chemical process allowing the chlorine in the chlorophenol to precipitate as silver chloride, weighing 0.271 g. Calculate the % (wt/wt) of the chlorophenol in the sample, assuming that chlorophenol is the only source of chlorine in the sample. Provide your answer to two decimal places and without units. Avoid using scientific notation.Gravimetric analysis of Fe3O4 (MW = 232 g/mole) may be undertaken with the following reactions: Fe3O4 → Fe2O3 → Fe (OH)3. Weight of sample containing 8.00% Fe3O4 that must be taken to obtain a precipitate of Fe(OH)3 (MW = 107 g/mole) that weighs 150 mg is . a. 0.108 g b. 0.325 g c. 1.355 g d. 4.065 g Amount of Fe2O3 (MW = 160 g/mole) from which 150 mg of Fe(OH)3 (MW = 107 g/mole) may be obtained is . a. 0.112 g b. 0.224 g c. 0.448 g d. none of the other choices