olo 6 A major component of gasoline is octane (C,H,). When liquid octane is burned in air it reacts with oxygen (0,) gas to produce carbon dioxide gas and water vapor. Calculate the moles of water produced by the reaction of 1.1 mol of octane. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits. OLX

olo 6 A major component of gasoline is octane (C,H,). When liquid octane is burned in air it reacts with oxygen (0,) gas to produce carbon dioxide gas and water vapor. Calculate the moles of water produced by the reaction of 1.1 mol of octane. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits. OLX

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter4: Stoichiometry

Section: Chapter Questions

Problem 4.69PAE: 4.69 The pictures below show a molecular-scale view of a chemical reaction between H2 and CO to...

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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.
3.83 For the reaction of nitrogen, N2, and hydrogen, H2, to form ammonia, NH3, a student is attempting to draw a particulate diagram, as shown below. Did the student draw a correct representation of the reaction? If not, what was the error the student made?
4.69 The pictures below show a molecular-scale view of a chemical reaction between H2 and CO to produce methanol, CH3OH. The box on the left represents the reactants at the instant of mixing, and the box on the right shows what is left once the reaction has gone to completion. Was there a limiting reactant in this reaction? If so, what was it? Write a balanced chemical equation for this reaction. As usual, your equation should use the smallest possible whole number coefficients for all substances.
The production of ammonia nia * (N*H_{3}) from nitrogen and hydrogen, shown below, was an important breakthrough resulting in Nobel prizes in chemistry to Fritz Haber (1918) and Carl Bosch (1931). This compound is widely used in manufacturing fertilizers. 3H 2 (g)+N 2 (g) 2NH 3 (g) Calculate the mass of nitrogen (in kg ) needed to manufacture 1000 kg of ammonia . Assume four significant figures .
Imagine that you are given 0.2500 g of a sample of copper(II) sulfate pentahydrate (CuSO4 • 5 H2O). You very carefully heat the compound for an extended period of time to drive off water, after which you determine the mass of the remaining solid to be 0.1598 g. Determine whether the data given confirm the formula of the hydrate. You must show any relevant calculation
The great French chemist Antoine Lavoisier discovered the law of conservation of mass in part by doing a famous experiment in 1775. In this experiment they found that mercury(II) oxide, when heated, decompose into liquid mercury and an invisible and previously unknown substance: oxygen gas. A. Write a balanced chemical equation, including physical state symbols, for the decomposition of solid mercury (II) oxide (HgO) into liquid mercury and gaseous dioxygen. B. Suppose 72 mL of dioxygen gas are produced by this reaction, at a temperature of 120°C and pressure of exactly 1 atm. Calculate the mass of mercury (II) oxide that must have reacted in grams. Round your answer to three significant digits.
Ammonium perchlorate NH4ClO4 is a powerful solid rocket fuel, used in the Space Shuttle boosters. It decomposes into nitrogen N2 gas, chlorine Cl2 gas, oxygen O2 gas and water vapor, releasing a great deal of energy. Calculate the moles of oxygen produced by the reaction of 0.075mol of ammonium perchlorate. Be sure your answer has a unit symbol, if necessary, and round it to the correct number of significant digits.
320.4 grams of isomaltitol, C12H24O11, was combusted in a furnace completely in an excess oxygen. The products of this reaction are liquid water and gaseous carbon dioxide. How much water (in kg) do you expect from this reaction assuming that all of the isomaltitol reacts? Enter your numeric answer in the units of kg. Do not enter the unit. Use enough significant digits to prevent rounding errors. Hint: balance the reaction first. Recall that 1 kg = 1000 g.
Napeleon doesn’t think the water is clean enough at the water park “Waterloo”. In an effort to sanitize the water, Napeleon (he has OCD) knows that bromine can be used to purify the water at the water park. If 7.82 x 1021 formula units of sodium bromide are reacted with excess chlorine gas, how many milliliters of liquid bromine (density = 3.12 g/mL) are formed? 2 NaBr (s) + Cl2 (g) à 2 NaCl (s) + Br2 (l) (BALANCED)
The equation for the complete combustion of butane gas (C4H10) is : 2C4H10+ 13O2 8CO2+ 10H2O Measured under the same conditons, how many liters of carbon dioxide are produced when 0.250 liters of butane gas is burned?
Liquid hexane CH3CH24CH3 reacts with gaseous oxygen gas O2 to produce gaseous carbon dioxide CO2 and gaseous water H2O . What is the theoretical yield of water formed from the reaction of 79.3g of hexane and 213. g of oxygen gas? Be sure your answer has the correct number of significant digits in it.
You take 4 tablets of aspirin (a compound that contains carbon, hydrogen, and oxygen) and perform a combustion reaction by burning the 4 tablets in the presence of air, which produces 2.20 g CO2 and 0.400 g H2O. If each tablet weighs 5.51 x 10-4 lbs, and the molar mass is 180.1 g/mol, what is the molecular formula of aspirin?

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