Concept explainers
Automobile exhaust is a major cause of air pollution. One pollutant is the gas nitrogen oxide, which forms from nitrogen and oxygen gases in the air at the high temperatures in an automobile engine. Once emitted into the air, nitrogen oxide reacts with oxygen to produce nitrogen dioxide, a reddish brown gas with a sharp, pungent odor that makes up smog. One component of gasoline is heptane, C7H16, a liquid with a density of 0.684 g/mL. In one year, a typical automobile uses 550 gal of gasoline and produces 41 lb of nitrogen oxide. (7.4, 7.8, 8.6)
a. Write balanced chemical equations for the production of nitrogen oxide and nitrogen dioxide.
b. If all the nitrogen oxide emitted by one automobile is converted to nitrogen dioxide in the atmosphere, how many kilograms of nitrogen dioxide are produced in one year by a single automobile?
c. Write a balanced chemical equation for the combustion of heptane.
d. How many moles of gaseous CO2 are produced from the gasoline used by the typical automobile in one year, assuming the gasoline is all heptane?
e. How many liters of carbon dioxide at STP are produced in one year from the gasoline used by the typical automobile?
Two gases found in automobile exhaust are carbon dioxide and nitrogen oxide.
Trending nowThis is a popular solution!
Chapter 9 Solutions
Chemistry: An Introduction to General, Organic, and Biological Chemistry, Books a la Carte Edition (12th Edition)
- A power plant is driven by the combustion of a complex fossil fuel having the formula C11H7S. Assume the air supply is composed of only N2 and O2 with a molar ratio of 3.76:1.00, and the N2 remains unreacted. In addition to the water produced, the fuels C is completely combusted to CO2 and its sulfur content is converted to SO2. In order to evaluate gases emitted at the exhaust stacks for environmental regulation purposes, the nitrogen supplied with the air must also be included in the balanced reactions. a Including the N2 supplied m the air, write a balanced combustion equation for the complex fuel assuming 100% stoichiometric combustion (i.e., when there is no excess oxygen in the products and the only C-containing product is CO2). Except in the case of N2, use only integer coefficients. b Including N2 supplied in the air, write a balanced combustion equation for the complex fuel assuming 120% stoichiometric combustion (i.e., when excess oxygen is present in the products and the only C-containing product is CO2). Except in the case of use only integer coefficients c Calculate the minimum mass (in kg) of air required to completely combust 1700 kg of C11H7S. d Calculate the air/fuel mass ratio, assuming 100% stoichiometric combustion. e Calculate the air/fuel mass ratio, assuming 120% stoichiometric combustion.arrow_forward89 A number of compounds containing the heavier noble gases, and especially xenon, have been prepared. One of these is xenon hexafluoride (XeF6), which can be prepared by heating a mixture of xenon and fluoride gases. XeF6 is a white crystalline solid at room temperature and melts at about 325 K. A mixture of 0.0600 g of Xe and 0.0304 g of F2 is sealed into a 100.0-mL bulb. (The bulb is heated, and the reaction goes to completion. Then the sealed bulb is cooled back to 20.0°C. What will be the final pressure in the bulb, expressed in torr?arrow_forwardWrite a balanced equation for the reaction between (a) dihydrogen sulfide and sulfur dioxide gases to form sulfur solid and steam. (b) methane, ammonia, and oxygen gases to form hydrogen cyanide gas and steam. (c) iron(lll) oxide and hydrogen gas to form molten iron and steam. (d) uranium(IV) oxide and hydrogen fluoride gas to form uranium(IV) fluoride and steam. (e) the combustion of ethyl alcohol (C2H5OH) to give carbon dioxide and water.arrow_forward
- 4.61 What is actually measured by the octane ratings of different grades of gasoline?arrow_forwardA Boron and hydrogen form an extensive family of compounds, and the diagram below shows how they are related by reaction. The following table gives the weight percent of boron in each of the compounds. Derive the empirical and molecular formulas of compounds A-E.arrow_forwardThe heat of neutralization, Hneut, can be defined as the amount of heat released (or absorbed), q, per mole of acid (or base) neutralized. Hneut for nitric acid is -52 kJ/mol HNO3. At 27.3C, 50.00 mL of 0.743M HNO3 is neutralized by 1.00 M Sr(OH)2 in a coffee-cup calorimeter. (a) How many mL of Sr(OH)2 were used in the neutralization? (b) What is the final temperature of the resulting solution? (Use the assumptions in Question 11.)arrow_forward
- The carbon dioxide exhaled in the breath of astronauts is often removed from the spacecraft by reaction with lithium hydroxide 2LiOH(s)+CO2(g)Li2CO3(s)+H2O(l) Estimate the grams of lithium hydroxide required per astronaut per day. Assume that each astronaut requires 2.50 103 kcal of energy per day. Further assume that this energy can be equated to the heat of combustion of a quantity of glucose, C6H12O6, to CO2(g) and H2O(l). From the amount of glucose required to give 2.50 103 kcal of heat, calculate the amount of CO2 produced and hence the amount of LiOH required. The H for glucose(s) is 1273 kJ/mol.arrow_forwardHydrogen peroxide is used as a cleansing agent in the treatment of cuts and abrasions for several reasons. It is an oxidizing agent that can directly kill many microorganisms; it decomposes on contact with blood, releasing elemental oxygen gas (which inhibits the growth of anaerobic microorganisms); and it foams on contact with blood, which provides a cleansing action. In the laboratory, small quantities of hydrogen peroxide can be prepared by the action of an acid on an alkaline earth metal peroxide, such as barium peroxide: BaO2(s)+2HCl(aq)H2O2(aq)+BaCl2(aq) What mass of hydrogen peroxide should result when 1.50 g barium peroxide is treated with 25.0 mL hydrochloric acid solution containing 0.0272 g HCI per mL? What mass of which reagent is left unreacted?arrow_forwardCinnabar, (or Cinnabarite) HgSHgS is the common ore of mercury. Because of its mercury content, cinnabar can be tpxoc to human beings; however, because of its red color, it has also been used since ancient times as a pigment. Alchemists produced elemental mercury by roasting cinnabar ore in air: HgS(s)+O2(g) → Hg(l) + SO2(g) The votality and toxicity of mercury make this a hazardous procedure, which likely shortened the life span of many alchemists. Given 100g of cinnabar, a. How much elemtal mercury can be produced from this reaction? b. How much oxygen is required to completely react with the given amount of cinnabar?arrow_forward
- The combustion of gasoline produces carbon dioxide and water. Assume gasoline to be pure octane (C8H18) and calculate how many kilograms of carbon dioxide are added to the atmosphere per 7.8kg of octane burned.arrow_forwardThe 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?arrow_forwardThe manufacture of aluminum includes the production of cryolite (Na3AlF6) from the following reaction: 6〖HF〗_((g))+3〖NaAlO〗_(2(s))→ 〖Na〗_3 〖AlF〗_(6(s))+3H_2 O_((l))+ 〖Al〗_2 O_(3(s)) How much HF (hydrogen sulfide) is required to produce 2.50kg of Na3AlF6? How many cm3 of HF(g) are needed to produce 26.0g of Na3AlF6? The density of HF (g) at 25is 1.15g/L.arrow_forward
- Chemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage LearningChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
- General Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage LearningChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningChemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning