The anserw is D. I need help understanding and what formula to use 11:55 Oa0 aoPhotoRel AbundanceIIA sample of air is analyzedby GC/MS, followed byelemental analysis.Among the varioussubstances in the sample,this major pollutants isfound.10050.0% O0850.0% S6040200.0+10702030405060mizFind the empirical (EF) and molecular (MF) formulas ofthis substanceMF = S,02A. EF = S,0C. EF SOB. EF = SOO EF = SO,MF = S,02MF = SO2%3D%3D%3DMF = SO%3D%3D

Answer - The correct option is (d) Solution - According to the question - Given - Molecular mass of…

Answered: air is analyzed 5, followed by cal…

air is analyzed 5, followed by cal analysis. the various s in the sample, - pollutants is pund. pirical (EF) and m this subs MF = S,02 MF = SO

Introduction to General, Organic and Biochemistry

11th Edition

ISBN:9781285869759

Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Publisher:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Chapter5: Gases, Liquids, And Solids

Section: Chapter Questions

Problem 5.47P

See similar textbooks

Similar questions

5-56 The three main components of dry air and the percentage of each are nitrogen (78.08%), oxygen (20.95%), and argon (0.93%). (a) Calculate the partial pressure of each gas in a sample of dry air at 760 mm Hg. (b) Calculate the total pressure exerted by these three gases combined.
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.
5-118 Isooctane, which has a chemical formula C8H18 is the component of gasoline from which the term octane rating derives. (a) Write the balanced chemical equation for the combustion of isooctane. (b) The density of isooctane is 0.792 g/mL. How many kg of C02 are produced each year by the annual U.S. gasoline consumption of L? (c) What is the volume in liters of this CO2 at STP? (d) The chemical formula for isooctane can be represented by (CH3)3CCH2CH(CH3)2. Draw a Lewis structure of isooctane. (e) Another molecule with the same molecular formula is octane, which can be represented by: When comparing isooctane and octane, one structure is observed to have a boiling point of 99°C, while another is known to have a boiling point Of 125°C. Which substance, isooctane or octane, is expected to have the higher boiling point? (f) Determine whether isooctane or octane is expected to have the greater vapor pressure.
A sample of a smoke stack emission was collected into a 1.25-L tank at 752 mm Hg and analyzed. The analysis showed 92% CO2, 3.6% NO, 1.2% SO2, and 4.1% H2O by mass. What is the partial pressure exerted by each gas?
93 The complete combustion of octane can be used as a model for the burning of gasoline: 2C8H18+25O216CO2+18H2O Assuming that this equation provides a reasonable model of the actual combustion process, what volume of air at 1.0 atm and 25°C must be taken into an engine to burn 1 gallon of gasoline? (The partial pressure of oxygen in air is 0.21 atm and the density of liquid octane is 0.70 g/mL.)
The Mount Pinatubo volcano eruption in 1991 released an estimated 1.82 x 1013g of SO2 into the atmosphere. If the gas had an average temperature of -17.0 C and filled the troposphere, whose approximate volume is 8 x 1021L, what is the approximate partial pressure of SO2 caused by the eruption?
5-115 Ammonium nitrite decomposes upon heating to form nitrogen gas and water vapor according to the following unbalanced chemical reaction: When a sample is decomposed in a test tube, 511 mL Of wet N2(g) is collected over water at 26°C and 745 torr total pressure. How many grams of dry NH4NO2(s) were initially decomposed? The vapor pressure of water at 26°C is 25.2 torr.
5-54 Automobile air bags are inflated by nitrogen gas. When a significant collision occurs, an electronic sensor triggers the decomposition of sodium azide to form nitrogen gas and sodium metal. The nitrogen gas then inflates nylon bags, which protect the driver and front-seat passenger from impact with the dashboard and windshield. What volume of nitrogen gas measured at 1 atm and 27°C is formed by the decomposition of 100. g of sodium azide?
sodium azide (Na3N) decomposes on heating to form sodium and nitrogen gas. 2Na3N--> 6Na+N2 1.35g of sodium nitride were heated. a) calculate the mass of sodium formed on complete decomposition of the sodium nitride. give your answer to 3 significant figures.(AO2) b)calculate the volume of nitrogen gas (in cm^3)produced on complete decomposition of 1.35g of sodium nitride at 320K and 110kpa. the gas constant R= 8.31JK^-1 mol^-1. give your answer to 3 significant figures. (AO2)
A gas sample is collected in a special gas sampling bag that does not react with the pollutantscollected but is free to expand and contract. When the sample was collected, the atmosphericpressure was 103.0 kPa. At the time the sample was analyzed, the atmospheric pressure was100.0 kPa. The bag was found to contain 0.020 ppm of SO2. Would the original concentrationof SO2 be more, less, or the same? Explain.
Nitrogen is maintained at 152 kPa in a 2.00-dm3 vessel at 298.15K. If its molar mass is 28.0134 g mol-1 calculate: (a) The amount of N2 present (ans: 0.123) (b) The number of molecules present (ans: 7.41 x 1022) (c) The root-mean-square speed of the molecules (ans: 515.2) (d) The average translational kinetic energy of each molecule (ans: 6.174 x 10-21) (e) The total translational kinetic energy in the system (ans: 457)
Given, Mass of lighter initially: 13.948 g Final mass of lighter: 13.668 g Mass of fuel used: 0.28 g Temperature in C: 22.2 C Temperature in K: 295.35 K Volume of gas collected in mL: 93.5 mL Volume of gas collected in L: 0.0935 L Total pressure: 0.99956 atm Using a graph of ln P in mmHg versus 1/T where T is the temperature in Kelvin. The equation is y = -5206.4 x + 20.621 (With an R^2 = 0.9999) Using y = -5206.4x + 20.621 (With an R^2 = 0.9999) Find the; 1. Vapor pressure of water: 2. Pressure of fuel: 3. Pressure of fuel in atm: 4. Molar mass of fuel :