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- Certain amount of pure charcoal (carbon) has to be burnt with supplied natural air. Process engineer allowed exact amount of air required to burn the entire charcoal completely to carbon dioxide. Carbon has no reaction with nitrogen gas present in the air. In the reaction outlet if 50 kg of carbon dioxide gas was found, calculate the amount of charcoal and air used. (12C, 16O, 14N).Acetyl Salicylate, C9H8O4, reacts with Potassium hydroxide. 1.75g of acetyl salicylate were hydrolyzed with 50cm3 of 0.57mol/dm3 of potassium hydroxide and the mixture were made up of 250cm3 with distilled water in a volumetric flask. Calculate: The number of moles of acetyl salicylate in 1.75g The number of moles of potassium hydroxide of 0.575mol/dm3 solution. The molarity of excess potassium hydroxide in the 250cm3 solution. If 1.15g of salicylic acid, C7H8O3, were obtained. Determine the percentage yield of the reaction.(a) A commercial 737 jet transporting 143 passengers and 5 crew members from Kansas City (MCI) to Baltimore (BWI) burned 11,800 lb (about 1700 gallons) of Jet A fuel en route. Jet A fuel is kerosine based, consisting primarily of CnH2n+2 hydrocarbons, with n =6 to 16, so the carbon:hydrogen ratio is close to 1:2. During this flight, how much CO2 was released into the atmosphere? Assume the combustion of the fuel was complete, so all the fuel was burned to form CO2 and H2O. Give both the mass of CO2 produced (in kg and in lbs) and the volume it would occupy at 298 K, 1 atm.(b) How much CO2 would be released into the atmosphere if those passengers and crew made the trip instead, in pairs, in hybrid cars at 40 miles per gallon. Assume the density of the gasoline is 0.75 kg L-1 and that carbon and hydrogen dominate the composition in a ratio of 1:2. The road trip is 1082 miles.
- An ether solution of cyclohexane-1,2-dicarboxylic acid (CDA), a compound with two carboxyl (COOH) groups, was extracted with a 10.0% NAHCO3(aq) solution. Assume that reaction between cyclohexane- 1,2-dicarboxylic acid (CDA) and NaHCO:(aq) goes to completion:i.e., the limiting reagent (CDA) is used up and both carboxyl groups of the acid react. HO HO cyclohexane-1,2-dicarboxylic acid In the space below, provide the balanced chemical equation for the complete deprotonation of cyclohexane-1,2-dicarboxylic acid (CDA) by sodium bicarbonate, in which both carboxyl groups react. Provide chemical structures ( not molecular formulae) of all reactants/reagents & products:In an Orsat analysis the % CO2 of the product of the combustion is 20% . If percent excess air is 30% . find the maximum percentage of CO2 attainable.6.) Since all the products have the same molecular weight, you can closely approximate the density of the product mixture by averaging the densities of the products. Using the average product density, determine the theoretical yield in mL when 1.5 mL of 3,3-dimethyl-2-butanol and 7 drops of H2SO4 (conc) are heated together at 70°C.
- 3-28 A 1.8-m3 rigid tank contains steam at 220°C. One-third of the volume is in the liquid phase and the rest is in the vapor form. Determine (a) the pressure of the steam, (b) the quality of the saturated mixture, and (c) the density of the mixture. Value (5/30) Steam 1.8 m 220°Ccombustion equation. Q2 // For the reaction bellow, find the mole fractions of all spices. If KP-0.1 A + 2B + C 03//In a combustion operation, anthracite used showed 92.8% C and 1.3% ash. If this coal is burned in dry air at 28°C, 1 atm abs, combustion gases with the following Orsat analysis results: 14.15% CO2, 5.77% 02, 79.97% N2, 0.03% SO2, and 0.08% NO. The combustion gases leave at 600°C and 800 mmHg. a) What is the ultimate analysis of the anthracite coal? b) What is the calorific value of the solid fuel in MJ for every kg of anthracite coal? c) What is the Orsat analysis of the flue gas?
- A 600.0 mg sample consist only of CaC2O4 and MgC2O4 was heated at 500°C converting the two salts to CaCO3 and MgCO3. The resulting precipitate weighed 465.0 mg. If the sample had been heated at 900°C, the products would be CaO and MgO, what would the mixture of oxides weigh? (FW: CaC2O4=128.1; MgC2O4=112.3; CaCO3=100.1; MgCO3=84.31; CaO=56.08; MgO=40.31)C. DETERMINATION Mass of empty calorimeter cups Mass of calorimeter cups - H₂O Mass of water Mass of anhydrous MgSO (s) Moles of anhydrous MgSO (s) Calculations: Temperature Readings, 'C Initial (0) ½ minute 1 minute 1½ minutes 2 minutes 3 minutes 4 minutes 4½ minutes OF MOLAR HEAT OF SOLVATION 4.603 43.910 34.241 8 2.009 0.017 mol 5 minutes 5½ minutes 6 minutes 6½ minutes 7 minutes 7½ minutes 8 minutes 8½ minutes 9 minutes 20.60⁰°C 20.60°C 20.60°C 20.60°C 20.60°C Add MgSO, to water 25.50°C 25.90°C 26.00° C 26-10° C 26.20° C 26.30° C 26.30°C 26.30°C 26.30° C 26-30°C 26.30°CCalculate (a) the specific volume, (b) Enthalpy, and (c) the absolute humidity of the air at 40°C and the relative humidity of 49%, at a barometric pressure of 700 mm Hg. (a) specific volume = m3 / kg (b) Enthalpy = (kj / kg air) (c) absolute humidity = (kg water / kg air)