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- Combustible vapor-air mixtures are flammable over a limitedrange of concentrations. The minimum volume % of vapor thatgives a combustible mixture is called the lower flammable limit(LFL). Generally, the LFL is about half the stoichiometric mix-ture, the concentration required for complete combustion of thevapor in air. (a) If oxygen is 20.9 vol % of air, estimate the LFL forn-hexane, C₆H₁₄. (b) What volume (in mL) of n-hexane (d=0.660 g/cm³) is required to produce a flammable mixture of hexane in 1.000 m³of air at STP?When limestone (solid CaCO3) is heated, it decomposes into lime (solid CaO) and carbon dioxide gas. This is an extremely useful industrial process of great antiquity, because powdered lime mixed with water is the basis for mortar and concrete — the lime absorbs CO2 from the air and turns back into hard, durable limestone. Suppose some calcium carbonate is sealed into a limekiln of volume 550.L and heated to 700.0°C. When the amount of CaCO3 has stopped changing, it is found that 4.14kg have disappeared. Calculate the pressure equilibrium constant Kp this experiment suggests for the equilibrium between CaCO3 and CaO at 700.0°C. Round your answer to 2 significant digits. Note for advanced students: it's possible there was some error in this experiment, and the value it suggests for Kp does not match the accepted value.The ideal gas law relates the amount of gas present to its pressure, volume, and temperature. The ideal gas law is typically written as ??=???PV=nRT where ?P is the pressure, ?V is the volume, ?n is the number of moles of gas, ?R is the ideal gas constant, and ?T is the temperature. Rearrange the equation to solve for ?. then.... At 256 K,256 K, 1.435 mol1.435 mol of an ideal gas occupy a volume of 10.83 L10.83 L and have a pressure of 2.785 atm.2.785 atm. What is the value of the ideal gas constant? R=
- (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.During photosynthesis, plants convert carbon dioxide and water to glucose (C6H12O6) and oxygen gas. a. Is photosynthesis a source or a sink of a GHG? Explain. b. Write and balance the chemical equation for the photosynthesis c. It is estimated that the amount of CO2 sequestered (removed from the air) by an urban tree is 60.0 kg.4 How much glucose can be produced from 60.0 kg CO2 during photosynthesis?Assume that a single cylinder of an automobile engine hasa volume of 524 cm3. (a) If the cylinder is full of air at 74 °Cand 0.980 atm, how many moles of O2 are present? (Themole fraction of O2 in dry air is 0.2095.) (b) How manygrams of C8H18 could be combusted by this quantity ofO2, assuming complete combustion with formation ofCO2 and H2O?
- A sample of potassium permaganate (KMnO4) reacts to completion with sodium oxalate (Na2C2O4) in the folowing redox reaction: 2MnO4- (aq) + 5C2O4-2 (aq) + 16H+ (aq) --> 10CO2 g) + 2Mn+2 (aq) + 8H2O (l) The volume of carbon dixoide released by the reaction at 297 K and 1.00 atm was 138 L. How many moles of potassium permanganate reacted? The Universal Gas Constant is 0.082057 L x atm/ mol x K. (answer in sig figs)Assume that a single cylinder of an automobile engine hasa volume of 524 cm3. (a) If the cylinder is full of air at 74 °C and 0.980 atm, how many moles of O2 are present? (Themole fraction of O2 in dry air is 0.2095.) (b) How manygrams of C8H18 could be combusted by this quantity ofO2, assuming complete combustion with formation ofCO2 and H2O?4a Assume that worldwide combustion of fossil fuel accounts for an energy use of 500 x 1015 kJ/year. Also, assume that all fossil fuels can be represented by the formula C3H5 with energy content of 32,500 kJ/kg.Finally, assume that air is 79% N2 and 21% O2 , and has a molecular weight of 29 kg/kmol. i. Estimate the annual release of CO2 to the atmosphere by burning fossil fuels, in kg/yr ii. If all that CO2 entered the atmosphere (and none was removed), estimate the increase in atmospheric concentration, in ppm by volume. Assume the atmosphere contains 6.7 x 1018 kg of air.
- The reaction is balanced: citric acid: 3NaHCO3 + C6H10O8 -> Na3 C6H7O8 + 3H2O + 3 CO2 Show the calculations required to determine quantities of sodium hydrogen carbonate and citric acid: (3NaHCO3 + C6H10O8) . Pressure is 100.800kPa, Temperature is 23 C and Volume is 784ml.Freon-12 (CF₂Cl₂), widely used as a refrigerant and aerosolpropellant, is a dangerous air pollutant. In the troposphere, ittraps heat 25 times as effectively as CO₂, and in the stratosphere,it participates in the breakdown of ozone. Freon-12 is preparedindustrially by reaction of gaseous carbon tetrachloride with hy-drogen fluoride. Hydrogen chloride gas also forms. How manygrams of carbon tetrachloride are required for the production of16.0 dm₃ of Freon-12 at 27°C and 1.20 atm?At 25°C and 1 atm, 0.500 mol/kg solution of NaCl is water has VNaCI = 18.63 cm³/mol and VH2O = 18.062 cm³/mol. Find the volume of a solution prepared by dissolving 0.5000 mol of NaCl in 1000.0 g of water.