Calculate the number of pounds of CO, released into the atmosphere when a 25.0 gallon tank of gasoline is burned in anautomobile engine. Assume that gasoline is primarily octane, CgH,8, and that the density of gasoline is 0.692 g mL. Thisassumption ignores additives. Also, assume complete combustion.CO, released:IbTOOLSx10

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Answered: Calculate the number of pounds of CO,…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter4: Energy And Chemical Reactions

Section: Chapter Questions

Problem 123QRT

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62 Ammonium dinitramide (ADN), NH4N(NO2)2, was considered as a possible replacement for aluminium chloride as the oxidizer in the solid fuel booster rockets used to launch the space shuttle. When detonated by a spark, AND rapidly decomposes to produce a gaseous mixture of N2,O2, and H2O. (This is not a combustion reaction. The ADN is the only reactant.) The reaction releases a lot of heat, so the gases are initially formed at high temperature and pressure. The thrust of the rocket results mainly from the expansion of this gas mixture. Suppose a 2.3-kg sample of ADN is denoted and decomposes completely to give N2,O2, and H2O. If the resulting gas mixture expands until it reaches a temperature of 100°C and a pressure of 1.00 atm, what volume will it occupy? Is your answer consistent with the proposed use of ADN as a rocket fuel?
Calculate the number of pounds of CO2 released into the atmosphere when a 10.0 gallon tank of gasoline is burned in an automobile engine. Assume that gasoline is primarily octane, C8H18,C8H18, and that the density of gasoline is 0.692 g⋅mL−1. This assumption ignores additives. Also, assume complete combustion.
How many moles of O2 are needed to burn 1.45 mol of C8H18? Express the amount in moles to three significant digits. The complete combustion of octane, C8H18, a component of gasoline, proceeds as follows: 2C8H18(l)+25O2(g)→16CO2(g)+18H2O(g) Relevant volumetric equivalencies 1 gal = 3.785 L 1 L = 1000 mL
From the discussion question from Module 5, recall the chemical equation for the combustion of gasoline (iso-octane, C8H18) is: 2C8H18 + 25O2 ---> 16CO2 + 18H2O This means that 2 moles of iso-octane combine with 25 moles of CO2 to produce 16 moles of CO2 and 18 moles of water. This is important for understanding the impact of fossil fuel use on the atmosphere because burning one mole of fuel adds a lot of CO2. Thinking about this in terms of the stoichiometry, and change in concentration, suppose we had 1.0 mole of iso-octane dissolved in 1.0 m3 of atmosphere. That means the concentration of carbon-containing molecules would be 1 mole per cubic meter. However, ff we burned all that iso-octane and convert the C8H18 into CO2 the concentration of carbon-containing molecules increases. How much does the concentration of carbon-containing molecules increase if 1.0 mole of C8H18 in 1.0 m3 of air is converted into CO2 as shown in the chemical equation above?
The citizens of the world burn the fossil fuel equivalent of 7 * 1012 kg of petroleum per year. Assume that all of this petroleum is in the form of octane (C8H18) and calculate how much CO2 (in kg) the world produces from fossil fuel combustion per year. (Hint: Begin by writing a balanced equation for the combustion of octane.) If the atmosphere currently contains approximately3 * 1015 kg of CO2, how long will it take for the world’s fossil fuel combustion to double the amount of atmospheric carbon dioxide?
How many grams of CO2 are produced from burning one gallon of biodiesel(3,311 g of biodiesel)?C19H36O2 + 27O2 ---> 19 CO2 + 18 H2O
Using car miles per gallon and the miles you drive in 1 week calculate the liters of carbon dioxide you produce when using your car. Compare your miles in February (pre-covid) versus June (post-covid). Assume that your engine combusts at 1.00 atm and 25.0 celsius. Assume that your gasoline is 100% octane (C8H18). You will also need to balance the combustion reaction that occurs in your car engine. You will need to use PV=nRT
Using your cars miles per gallon and the miles you drive in 1 week calculate the liters of carbon dioxide you produce when using your car. Compare your miles in February (pre-covid) versus June (post-covid). Assume that your engine combusts at 1.00 atm and 25.0 celsius. Assume that your gasoline is 100% octane (C8H18). You will also need to balance the combustion reaction that occurs in your car engine. You will need to use PV=nRT I think calculations are not correct specially for June. please help 2C8H18+ 25O2→16CO2+18H2O Feb, (pre covid), Miles covered per week=15×7=105 miles So fuel consumed per week=105 miles/30 miles ga =3.5 ga Density of octane=3.18 kg/ga Mass=volume × density Mass of Octane used per week = 3.5 ga x 3.18 kg/ga =11.13 kg Moles of octane in 11.13 kg 11.13 kg/114 kg/k mol =0.097 kmol 2 kmol octan≡16 kmol CO2 0.097 kmol octane =16/2 × 0.097 kmol CO2 0.097 kmol octane = 0.781 kmol CO2 n= 0.781 kmol=781 moles CO2 V=781 mol x 8.314j/k. mol x (25+273)K/1atm x…
The U.S. proven natural gas reserves in 2013 were 323 trillion ft3 . How long will these reserves last if there are no imports or exports and if the U.S. annual rate of use of 24.5 trillion ft3 continues?
Calculate the volume of air required for complete combustion of 1m3 of a gaseous fuel having the composition: CO = 46%; CH4 = 10%; H2 = 40%; C2H2 = 2%; N2 = 1% and the remaining being CO2.
Whenever organic matter is decomposed under oxygen-free(anaerobic) conditions, methane is one of the products. Thus,enormous deposits of natural gas, which is almost entirely methane, serve as a major source of fuel for home and industry.(a) Known sources of natural gas can produce 5600 EJ of energy(1 EJ 10^18J). Current total global energy usage is 4.0X10^2 EJper year. Find the mass (in kg) of known sources of natural gas(Hrxnfor the combustion of CH₄=802 kJ/mol).(b) For how many years could these sources supply the world’stotal energy needs?(c) What volume (in ft³) of natural gas, measured at STP, isrequired to heat 1.00 qt of water from 25.0C to 100.0C (d of H₂O= 1.00 g/mL; d of CH₄ at STP =0.72 g/L)?(d) The fission of 1 mol of uranium (about 4X10^4 ft³) in a nu-clear reactor produces 2X10^13 J. What volume (in ft3) of naturalgas would produce the same amount of energy?
GUIDE QUESTIONS: Differentiate the types of flame produced by the Bunsen burner. ________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________ a. Which type of flame: undergoes complete combustion of fuel (propane) used? Why? Write the reaction involved by predicting the product/s of the reaction. ____________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________ Reaction: C3H8(g) + O2(g)→ b. undergoes incomplete combustion of fuel used? Why? Write the reaction involved.…

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