As with any combustion reaction, the products. I combusting a hydrocarbon fuel (C, Hy) with oxygen (O₂) are carbon dioxide (CO₂) and water (H₂O). A mass of 12.43 g for an unknown fuel was combusted in a reaction vessel containing an unknown amount of oxygen. At the end of the reaction, there still remained 12.39 g of the fuel as well as 0.0654 g of water and 0.1198 g of carbon dioxide. The oxygen was completely consumed during the reaction. How many molecules of oxygen gas were initially present in the reaction vessel? Express the number of molecules to three significant digits. ▸View Available Hint(s) amount of O₂ = ΕΠΙ ΑΣΦ 1 C ? molecules

As with any combustion reaction, the products. I combusting a hydrocarbon fuel (C, Hy) with oxygen (O₂) are carbon dioxide (CO₂) and water (H₂O). A mass of 12.43 g for an unknown fuel was combusted in a reaction vessel containing an unknown amount of oxygen. At the end of the reaction, there still remained 12.39 g of the fuel as well as 0.0654 g of water and 0.1198 g of carbon dioxide. The oxygen was completely consumed during the reaction. How many molecules of oxygen gas were initially present in the reaction vessel? Express the number of molecules to three significant digits. ▸View Available Hint(s) amount of O₂ = ΕΠΙ ΑΣΦ 1 C ? molecules

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter3: Stoichiometry

Section: Chapter Questions

Problem 178CP: You take 1.00 g of an aspirin tablet (a compound consisting solely of carbon, hydrogen, and oxygen),...

See similar textbooks

Similar questions

You take 1.00 g of an aspirin tablet (a compound consisting solely of carbon, hydrogen, and oxygen), burn it in air, and collect 2.20 g CO2 and 0.400 g H2O. You know that the molar mass of aspirin is between 170 and 190 g/mol. Reacting 1 mole of salicylic acid with I mole of acetic anhydride (C4H6O3) gives you 1 mole of aspirin and 1 mole of acetic acid (C2H4O2). Use this information to determine the molecular formula of salicylic acid.
The reaction of equal molar amounts of benzene, C6H6, and chlorine, Cl2, carried out under special conditions completely consumes the reactants and yields a gas and a clear liquid. Analysis of the liquid shows that it contains 64.03% carbon, 4.48% hydrogen, and 31.49% chlorine, and has a molar mass of 112.5 g/mol. Write the balanced equation for this reaction.
Write the balanced chemical equation for the complete combustion of adipic acid, an organic acid containing 49.31% C, 6.90% H, and the remainder O, by mass.
(a) Butane gas, C4H10, can burn completely in air [use O2(g) as the other reactant] to give carbon dioxide gas and water vapor. Write a balanced equation for this combustion reaction. (b) Write a balanced chemical equation for the complete combustion of C3H7BO3, a gasoline additive. The products of combustion are CO2(g), H2O(g), and B2O3(s).
Calcium carbonate forms carbon dioxide and calcium oxide when it is heated above 900 °C in a limekiln. When heated to 1000 °C in a laboratory, 4.31 g calcium carbonate produces 2.40 g calcium oxide and 1.90 g carbon dioxide. Outline a method similar to combustion analysis by which you could determine the empirical formula for calcium carbonate from these data. Carry out the determination.
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.
Many cereals are made with high moisture content so that the cereal can be formed into various shapes before it is dried. A cereal product containing 58% H2O by mass is produced at the rate of 1000. kg/h. What mass of water must be evaporated per hour if the final product contains only 20.% water?
Disulfur dichloride, S2Cl2, is used to vulcanize rubber. It can be made by treating molten sulfur with gaseous chlorine. S8() + 4 Cl2(g) 4 S2Cl2(g) Complete this table of reaction quantities for the production of 103.5 g S2Cl2.
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.
4.106 An ore sample with a mass of 670 kg contains 27.7% magnesium carbonate, MgCO3. If all of the magnesium carbonate in this ore sample is decomposed to form carbon dioxide, describe how to determine what mass of CO2 is evolved during the process.