The U.S. Environmental Protection Agency (U.S. EPA) monitorsair quality in the United States. Lead is among the pollutantsregularly monitored and regulated. Lead is released into the at-mosphere primarily by the processing of metals ores containinglead and by lead-based battery manufacturing. The effects of toomuch exposure to lead include neurological damage and cardio-vascular disease. Because of the Clean Air Act and its amend-ments, the amounts of lead in air have been decreasing for manyyears. The chart below shows the lead concentration in air in theUnited States from 2000 to 2014. Examine the data and answerthe questions below.Lead Concentration in Air in U.S.0.350.300.250.200.150.10£ 0.031998 2000 2002 2004 2006 2008 2010 2012 2014 2016Year100%50%-204 206 207 208Mass (amu)How many lead atoms were in one cubic centimeter of air in2011?Pb Concentration ug/mIntensity %

Here in question lead concentration is given in µg/m3. In 2011 the lead concentration is 0.10µg/m3.…

Answered: The U.S. Environmental Protection…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter8: Properties Of Gases

Section: Chapter Questions

Problem 122QRT

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perform stoichiometric ca1cu1uions for reactions involving gases as reactants or products.
Methane (CH4) gas flows into a combustion chamber at a rate of 200. L/min at 1.50 atm and ambient temperature. Air is added to the chamber at 1.00 atm and the same temperature, and the gases are ignited. a. To ensure complete combustion of CH4 to CO2(g) and H2O(g), three times as much oxygen as is necessary is reacted. Assuming air is 21 mole percent O2 and 79 mole percent N2, calculate the flow rate of air necessary to deliver the required amount of oxygen. b. Under the conditions in part a, combustion of methane was not complete as a mixture of CO2(g) and CO(g) was produced. It was determined that 95.0% of the carbon in the exhaust gas was present in CO2. The remainder was present as carbon in CO. Calculate the composition of the exhaust gas in terms of mole fraction of CO, CO2, O2, N2, and H2O. Assume CH4 is completely reacted and N2 is unreacted.
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?
Environmentally conscious Susan has been toldthat a new electric car will only generate 6 ounces of green-house gases (GHG) per mile, but that a standard internalcombustion car is double that at 12 ounces per mile. However,the nature of electric cars is such that the new technology andelectric batteries generate 30,000 lbs. of GHG to manufactureand another 10,000 lbs. to recycle. A standard car generatesonly 14,000 lbs. of GHG to manufacture, and recycling withestablished technology is only 1,000 lbs. Susan is interested intaking a systems approach that considers the life-cycle impactof her decision. How many miles must she drive the electriccar for it to be the preferable decision in terms of reducinggreenhouse gases?
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?
Carbon dioxide, which is recognized as the major contributorto global warming as a “greenhouse gas,” is formedwhen fossil fuels are combusted, as in electrical powerplants fueled by coal, oil, or natural gas. One potential wayto reduce the amount of CO2 added to the atmosphere isto store it as a compressed gas in underground formations.Consider a 1000-megawatt coal-fired power plant that producesabout 6 * 106 tons of CO2 per year. (a) Assumingideal-gas behavior, 1.00 atm, and 27 °C, calculate the volumeof CO2 produced by this power plant. (b) If the CO2 isstored underground as a liquid at 10 °C and 120 atm and adensity of 1.2 g>cm3, what volume does it possess? (c) If itis stored underground as a gas at 30 °C and 70 atm, whatvolume does it occupy?
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 a limekiln of volume 800.L is pressurized with carbon dioxide gas to 26.6atm, and heated to 600.0°C. When the amount of CO2 has stopped changing, it is found that 10.1kg of CaCO3 have appeared. Calculate the pressure equilibrium constant Kp this experiment suggests for the equilibrium between CaCO3 and CaO at 600°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 ??=???P⁢V=n⁢R⁢T 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=
Global warming’s drastic effect were attributed to the rapid accumulation of “greenhouse gases”in the atmosphere. Naming carbon dioxide as its major contributor, is formed when fossil fuels arecombusted in different power plants (e.g. fuel powered, namely by coal, oil, or natural gas). Some of thepotential way to reduce the amount of carbon dioxide that is added to atmosphere is to compress the gasin underground formations. We can consider this with a 1000-MW coal-fired power plant that produces an amount of 6.0 × 10^6tons of CO2 per year. (a) In an ideal gas – or perfect gas behavior, 1.00 atm, 27°C, calculate the volume of the carbon dioxide produced by the power plant mentioned. (b) What volumecan we obtain if CO2 (liquid form) stored in underground has an equation of state as 10 °C, 120 atm, anddensity of 1.2 g/cm^3? (c) Storing this underground as gas [on another note] at 36 °C and 90 atm, whatvolume can it occupy? Is the volume is larger or smaller than in liquid form? Explain.
Soil vapor extraction (SVE) is used to remove volatile or-ganic pollutants, such as chlorinated solvents, from soil at haz-ardous waste sites. Vent wells are drilled, and a vacuum pump is applied to the subsurface. (a) How does this remove pollutants?(b) Why does heating combined with SVE speed the process?
If 8g of ammonium hydroxide is completely decomposed by the reaction below in a closed container with a total volume of 5.00L and at 25°C, what will be the partial pressure of the ammonia gas liberated, in atmospheres? Assume the volume of the liquid is negligible. NH4OH(aq) --> H2O(l)+NH3(g)
The sudden appearance of hot gaseous products in a small initial volumeleads to rapid increases in pressure and temperature, which give the rocketits thrust. What total pressure of gas would be produced at 800°C by igniting 7.00 × 105 kg NH4ClO4 (a typical charge of the booster rockets in the space shuttle) and allowing it to expand to fill a volume of 6400 m3 (6.40 × 106L)? Use the ideal gas law

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