Combustion of hydrocarbons such as octane (C,H,g) produces carbon dioxide, a "greenhouse gas." Greenhouse gases in the Earth's atmosphere can trap the 18 Sun's heat, raising the average temperature of the Earth. For this reason there has been a great deal of international discussion about whether to regulate the production of carbon dioxide. 1. Write a balanced chemical equation, including physical state symbols, for the combustion of liquid octane into gaseous carbon dioxide and gaseous water. 2. Suppose 0.280 kg of octane are burned in air at a pressure of exactly 1 atm and a temperature of 20.0 °C. Calculate the volume of carbon dioxide gas that is produced. Round your answer to 3 significant digits.

Combustion of hydrocarbons such as octane (C,H,g) produces carbon dioxide, a "greenhouse gas." Greenhouse gases in the Earth's atmosphere can trap the 18 Sun's heat, raising the average temperature of the Earth. For this reason there has been a great deal of international discussion about whether to regulate the production of carbon dioxide. 1. Write a balanced chemical equation, including physical state symbols, for the combustion of liquid octane into gaseous carbon dioxide and gaseous water. 2. Suppose 0.280 kg of octane are burned in air at a pressure of exactly 1 atm and a temperature of 20.0 °C. Calculate the volume of carbon dioxide gas that is produced. Round your answer to 3 significant digits.

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter9: Chemical Quantities

Section: Chapter Questions

Problem 100CP: he production capacity for acrylonitrile (C3H3N)in the United States is over 2 billion pounds per...

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he production capacity for acrylonitrile (C3H3N)in the United States is over 2 billion pounds per year. Acrylonitrile, the building block tor acrylonitrile fibers and a variety of plastics, is produced from gaseous propylene, ammonia, and oxygen: :math>2C3H6(g)+2NH3(g)+3O22C3H3N(g)+6H2O(g) l type='a'> Assuming 100% yield, determine the mass of acrylonitrile which can be produced from the mixture below: l> Mass Reactant msp;5.23102g propylene td> msp;5.00102g ammonia td> msp;1.00103g oxygen td> i>What mass of water is formed from your mixture? Calculate the mass (in grams) of each reactant after the reaction is complete.
The element carbon undergoes many inorganic reactions, as well as being the basis for the field of organic chemistry. Write balanced chemical equations for the reactions of carbon described below. l type='a'> Carbon burns in an excess of oxygen (for example. in the air) to produce carbon dioxide. If the supply of oxygen is limited, carbon will still burn but will produce carbon monoxide rather than carbon dioxide. molten lithium metal is treated with carbon, lithium car bide, Li2C2 , is produced. i>Iron(II) oxide reacts with carbon above temperatures of about 700 °C to produce carbon monoxide gas and molten elemental iron. i>Carbon reacts with fluorine gas at high temperatures to make carbon tetrafluoride.
On Easter Sunday, April 3, 1983, nitric acid spilled from a tank car near downtown Denver, Colorado. The spill was neutralized with sodium carbonate: 2HNO3(aq)+Na2CO3(aq)2NaNO3(aq)+H2O(l)+CO2(g) a. Calculate H for this reaction. Approximately 2.0 104 gal nitric acid was spilled. Assume that the acid was an aqueous solution containing 70.0% HNO3 by mass with a density of 1.42 glcm3. What mass of sodium carbonate was required for complete neutralization of the spill, and what quantity of heat was evolved? (Hf for NaNO3(aq) = 467 kJ/mol) b. According to The Denver Post for April 4, 1983, authorities feared that dangerous air pollution might occur during the neutralization. Considering the magnitude of H, what was their major concern?
Oxygen is not normally found in positive oxidation states, but when it is combined with fluorine in the compound oxygen difluoride, oxygen is in a +2 oxidation state. Oxygen difluoride is a strong oxidizing agent that oxidizes water to produce O2 and HF. OF2(g) + H2O(g) → 2 HF(g) + O2(g) The standard formation enthalpy of oxygen difluoride is 24.5 kJ/mol. Using this information and data from Appendix J, calculate the standard reaction enthalpy for the reaction of oxygen difluoride with water. Table 4.2 Selected Standard Formation Enthalpies, ΔfH°, at 25°C
Many over-the-counter antacid tablets are now formulated using calcium carbonate as the active ingredient, which enables such tablets to also be used as dietary calcium supplements. As an antacid for gastric hyperacidity, calcium carbonate reacts by combining with hydrochloric acid found in the stomach, producing a solution of calcium chloride, converting the stomach acid to water, and releasing carbon dioxide gas (which the person suffering from stomach problems may feel as a “burp”). Write the unbalanced chemical equation for this process.
The percent nitrogen (N) in a protein sample can be determined by reacting the protein with sulfuric acid to produce ammonium sulfate. The ammonium sulfate is reacted with concentrated sodium hydroxide to form ammonia gas. The ammonia gas is collected by bubbling it through a known volume of standardized hydrochloric acid solution (all of the ammonia reacts in this step, is consumed). The unreacted hydrochloric acid is then back-titrated with standardized sodium hydroxide solution. The reactions involved are shown below: Protein-N + H2SO4 (aq) ⟶⟶ (NH4)2SO4 (aq) 2 NH4+(aq) + 2 NaOH (aq) 2 NH3 (g) + 2 H2O NH3 (g) + HCl (excess) NH4Cl (aq) + HCl (unreacted) HCl (unreacted) + NaOH (aq) NaCl (aq) + H2OA 1.85 g sample of the protein required 25.00 mL of 0.1535 M HCl and 21.55 mL of 0.0986 M NaOH. How many moles of NH3 were consumed by the standardized HCl? A. 8.55 x 10-4 B. 1.71 x 10-3 C. 2.13 x 10-3 D. 3.84 x 10-3 E. 5.97 x 10-3 What is the mass percent nitrogen in…
When exposed to oxygen and heat, copper metal oxidizes and copper (II) oxide appears onthe surface. Write the complete balanced chemical equation for this reaction. Identify the typeof reaction taking place and explain why it is NOT combustion.
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What mass of carbon dioxide is produced upon the complete combustion of 23.7 L of propane (the approximate contents of one 5-gallon tank)? Assume that the density of the liquid propane in the tank is 0.621 g/mL . (Hint: Begin by writing a balanced equation for the combustion reaction.)
22. A recipe for 1 cup of hollandaise sauce calls for ½ cup of butter, ¼ cup of hot water, 4 egg yolks, and the juice of a medium-sized lemon. How many cups of this sauce can be made from a pound (2 cups) of butter, a dozen eggs, 4 medium lemons, and an unlimited supply of hot water? Write an equation for making sauce, then use dimensional analysis and the process used in class for dealing with limiting reagents. How much of each ingredient are in excess?
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Chlorine is prepared industrially by heating hydrogen chloride gas with oxygen gas. Assuming the only products are water and chlorine gas, write a balanced chemical equation for the manufacture of chlorine.