A 7.333 gram sample of an organic compound containing C, H and O is analyzed by combustion analysis and 18.96 grams of CO2 and 3.882 grams of H2O are produced. In a separate experiment, the molar mass is found to be 136.2 g/mol

A 7.333 gram sample of an organic compound containing C, H and O is analyzed by combustion analysis and 18.96 grams of CO2 and 3.882 grams of H2O are produced. In a separate experiment, the molar mass is found to be 136.2 g/mol

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Related questions

Q: The combustion of 1.683 g of an organic compound containing only carbon, hydrogen and oxygen…

Q: 23. How many grams of Cr can be produced by the reaction of 44.1 g of Cr,O; with 35.0 g of Al…

A: 2 Al + Cr2O3 ......> Al2O3 + 2Cr Mass of Cr2O3 = 44.1g Molar mass of Cr2O3 = 152g/mol Moles of…

Q: Product X has a theoretical yield of 4.8 g. Isolated product X was placed in a plastic sample tray.…

A: Yield is the amount of product formed in a reaction. Theoretical yield is the amount of desired…

Q: The metals industry was a major source of air pollution years ago. One common process involved…

A: Given the reaction is, 2PbS+3O2---->2PbO+2SO2 Mole of PbS is 9.53mol. We have to calculate mole…

Q: The combustion of gasoline produces carbon dioxide and water. Assume gasoline to be pure octane…

A: Introduction: A combustion reaction is a reaction between fuel and oxidizing agents like air. It is…

Q: The first step in the reaction of Alka–Seltzer with stomach acid consists of one mole of sodium…

A: Given, one mole of sodium bicarbonate (NaHCO3) reacting with one mole of hydrochloric acid (HCl) to…

Q: A 0.3459 g tablet that contains bicarbonate generates 1.24 x 10−3 moles of CO2. What is the percent…

Q: Consider the reaction below used in the production of Lead (Pb). In a reaction utilizing 57.33g, PbO…

A: Given reaction: 2PbO + PbS —> 3Pb + SO2 amount of PbO given = 57.33 g Moles of PbO in…

Q: Consider the reaction to isolate titantium metal from titanium(IV) chloride: 2 Mg(s) + TiCl4(l)…

Q: Consider this reaction, which occurs in the atmosphere and contributes to photochemical smog: H2(g)…

A: Given, mass of H2 = 11.3 g we know, molar mass of H2 = 2.016 g/mol molar mass of HI = 127.911 g/mol…

Q: Morphine (C₁₇H₁₉NO₃) is a painkiller in the opiate family. A sample of morphine was discovered that…

Q: Sucrose (C₁₂H₂₂O₁₁) is combusted in air according to the following reaction: C₁₂H₂₂O₁₁(s) + O₂(g) →…

A: Given : Mass of sucrose = 35.4 gram Molar mass of sucrose = 342 gm/mole

Q: Sucrose (C₁₂H₂₂O₁₁) is combusted in air according to the following reaction: C₁₂H₂₂O₁₁(s) + O₂(g) →…

A: Given: Mass of sucrose = 82.9 g Molar mass of sucrose = 342.30 g/mol

Q: Consider the following reaction Ca(s) + 2HCI(aq) --> CaCl2(aq) + H2(g) If the theoretical yield of…

A: Theoretical yield = 0.736 g Actual yield = 0.710 g Percent yield = ?

Q: A 8.648 gram sample of an organic compound containing C, H and O is analyzed by combustion analysis…

A: 8.648 gram sample of an organic compound containing C, H and O 18.63 grams of CO2 Number of moles…

Q: The maximum amount of nickel(II) that could be plated out using 15 amps for an hour is

A: Given that - Nickel (II) - Ni2+ Current in Amperes = 15 ampere Time = 1 hour = 60 minutes = 60×60…

Q: In a reaction to make ethyl acetate, 25.5 g CH3COOH react with 11.5 g CH5OH to give a yield of 17.6…

Q: The combustion of gasoline produces carbon dioxide and water. Assume gasoline to be pure octane…

A: Gasoline: Gasoline is petroleum based flammable liquid. It is used as fuel for IC engines. Main…

Q: 18 g of CH4(g) are reacted with 5.2 g of O2(g) by the following reaction CH4(g) + 2O2(g) -->…

A: Given, mass of CH4 (g) = 18 g mass of O2 (g) = 5.2 g Now, the moles of CH4 (g) and O2…

Q: . Consider the reaction between NiS2 and O2:2 NiS2(s) + 5 O2( g) → 2 NiO(s) + 4 SO2( g)When 11.2 g…

A: Given data Reaction : 2 NiS2(s) + 5 O2( g) → 2 NiO(s) + 4 SO2( g) mass of NiS2 reacts = 11.2 g mass…

Q: Example: A reaction mixture for the combustion of octane contains 5.0 moles of octane and 50. moles…

Q: "A liquid fuel mixture contains 30.25% hexane (C6H14), 17.10% heptane (C7H16), and the rest octane…

A: Mass of fuel mixture = 15 kgHexane = 30.25%Heptane = 17.10%Octane = 100 - (30.25+17.10)…

Q: A compound containing only C, H, and O, was extracted from the bark of the sassafras tree. The…

A: Given:Mass of CO2 = 167 mg.Mass of H2O = 34.2 mg.Molar mass of CO2 = 44 g/mol.Molar mass of H2O = 18…

Q: The combustion of gasoline produces carbon dioxide and water. Assume gasoline to be pure octane…

A: Combustion reaction of octane 2C8H18 + 25O2 → 16CO2 + 18H2O From this Balanced chemical equation we…

Q: When 3.232 grams of a hydrocarbon, C,Hy, were burned in a combustion analysis apparatus, 11.10 grams…

A: Data given: Mass of sample = 3.232 g Mass of CO2 = 11.10 g Mass of H2O = 1.818 g Molar mass of the…

Q: Give the chemical formula for 3-ethyl-4,4-dimethyl heptane. Make sure you can draw the structure.

A: Here we have to write the chemical formula of 3-ethyl-4,4-dimethyl heptane-

Q: Under appropriate reaction conditions Ag and S produce Ag2S according to the equation 2Ag + S → Ag2s…

A: Balanced reaction: 2Ag + S ....> Ag2S Mass of Ag = 28.6 g Molar mass of Ag = 107.9g/mol Moles of…

Q: When 4.673 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 16.05 grams…

A: Given: Mass of compound burned = 4.673 g. Mass of CO2 produced = 16.05 g. Mass of H2O produced =…

Q: Consider the combustion of methane. CH4(g)+2O2(g)→CO2(g)+2H2O(g) Suppose 2.5 mol of methane are…

A: Given:Moles of CH4 = 2.5 mol.Moles of O2 = 3.5 mol.

Q: Dimethylhydrazine is a carbon–hydrogen–nitrogen compound used in rocket fuels. When burned in an…

A: Answer:

Q: 1. The organic solvent thiophene is a carbon-hydrogen-sulfur compound that yields CO2, H2O, and SO2…

A: Given: Mass of compound burned = 1.3020 g. Mass of CO2 produced = 2.7224 g. Mass of H2O produced =…

Q: A 1.000 g sample of an unknown compound containing only carbon, hydrogen, and oxygen was analyzed…

A: Given: Mass of sample = 1.000 g Mass of CO2 formed = 2.579 g Mass of H₂O formed = 0.6536 g Molar…

Q: If 13.2 g of NH3 is collected following the reaction of 2.88 mol NO with,7.00 mol H2, calculate the…

A: Given: Mass of NH3 formed experimentally = 13.2 g. Moles of NO taken = 2.88 mol. Moles of H2 taken =…

Q: Methanol has tremendous potential to be used as an alternate fuel. Carbon monoxide gas reacted with…

Q: The combustion of ammonia in the presence of excess oxygen yields NO2 and H2O according to the…

A: We have 52.4 g of ammonia, we have to calculate the mass of nitrogen dioxide produced.

Q: A 1.000 g sample of an unknown compound containing only carbon, hydrogen, and oxygen was analyzed…

Q: consider the following balanced equation. N2O4(l) + 2 N2H4(l) → 3 N2(g) + 4 H2O(g) Determine the…

A: Given, N2O4(l) + 2 N2H4(l) → 3 N2(g) + 4 H2O(g) Given, mass of N2O4 react = 60.0 g mass of N2H4…

Q: Sodium

A: 2. Given chemical reaction is- Fe(ClO3)2 + Na2S -> FeS + 2NaClO3 Given that Fe(ClO3)2 is in…

Q: In a particular reaction 8.60g of dinitrogen trioxide gas (N2O3) was actually produced by reacting…

Q: Morphine (C₁₇H₁₉NO₃) is a painkiller in the opiate family. A sample of morphine was discovered that…

A: Given: When morphine undergoes combustion, carbon dioxide is produced. Mass of mixture =…

Q: Complete combustion of 7.30 g of a hydrocarbon produced 22.4 g of CO2 and 10.7 g of H2O. What is…

Q: Molar Mass NaHCO3 84.01 g/mol. Molar Mass Na2CO3 105.99 g/ moo. A 1.375- gram sample of baking soda…

Question

A 7.333 gram sample of an
organic compound containing C,
H and O is analyzed by
combustion analysis and 18.96
grams of CO2 and 3.882 grams
of H2O are produced. In a
separate experiment, the molar
mass is found to be 136.2 g/mol
Determine the empirical
formula and the molecular
formula of the organic
compound.

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

SEE SOLUTION Check out a sample Q&A here

Step 1: No. of mass of each element

VIEW

Step 2: Determine empirical formula and molecular formula

VIEW

Solution

VIEW

Step by step

Solved in 3 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

Sucrose (C₁₂H₂₂O₁₁) is combusted in air according to the following reaction: C₁₂H₂₂O₁₁(s) + O₂(g) → CO₂(g) + H₂O(l) How many grams of carbon dioxide would be produced by the complete combustion of 0.755 moles of sucrose in the presence of excess oxygen?
An organic compound X was found to contain only C, H, and Cl. The following experiments were carried out with compound X: 1) When a 1.50-g sample of the compound was completely combusted in air, 3.52 g CO2 was formed. 2) When a 1.00-g sample of the compound was allowed to react with an excess of Ag, 1.27 g of AgCl was obtained. Determine the empirical formula of compound X. C9H4Cl C6H4Cl2 C9H6Cl C3H2Cl2 C6H5Cl
if u add 400.0 mL of water to 50.0 mL of 6.0 M HCl what is new concentration ?
A mixture contains KClO3 and KCl. When the mixture is heated, only the KClO3 decomposes via the following reaction: 2KClO3 (s) → 3O2 (g) + 2KCl (s)In an experiment to determine the percent KClO3 in a KClO3/KCl mixture, the mixture was heated in a crucible several times in order to bring it to constant mass. The following experimental data was obtained.Before Heating Mass empty crucible + lid = 20.61 g Mass crucible + lid+ KClO3/KCl mixture = 26.11 gAfter Heating Mass crucible + lid+ contents (after final heating ) = 24.68 g a) Mass KClO3 in mixture (stoichiometric calculation from the mass of oxygen evolved) b) %KClO3 in mixture (g KClO3/g mixture then multiply by 100)
Complete combustion of 4.50 g of a hydrocarbon produced 14.4 g of CO2 and 5.15 g of H2O. What is the empirical formula for the hydrocarbon?
A student performs the reduction of vanillin (152.15 g/mol) with sodium borohydride (37.83 g/mol) in the presence of 1 M NaOH. The student mixes 4.08 g of vanillin with 0.700 g of sodium borohydride and obtains 1.87 g of vanillyl alcohol (154.17 g/mol). What is the percent yield of this reaction? the answer to 3 significant figures.
For the following reaction: Co(OH)2 + CO2 → CoCO3 + H2O If 2.44g of Co(OH)2 is added to 1.99g of CO2, how many grams of CoCO3 can be made?
An unknown compound contains only C, H, and O. Combustion of 7.00 g of this compound produced 15.9 g CO2 and 6.51 g H2O. Convert the masses of C, H, and O in the unknown compound to moles.
Consider the following balanced chemical equation: 4KO2(s) + 2H2O(l) → 4KOH(s) + 3O2(g) Determine the mass (in g) of KOH formed if 47.1 g of KO2 reacts with 47.1 g of H2O.
Aspirin (C9H8O4) may be synthesized by mixing salicylic acid (C7H6O3) with excess acetic anhydride (C4H6O3). When 2.0 g of salicylic acid is mixed with excess acetic anhydride, 1.7 g of aspirin is collected. What is the percent yield of this reaction? The balanced equation is C7H6O3 + C4H6O3  C9H8O4 + C2H4O2 A.98 % B.85 % C.77 % D.65 % E.55 %
Ethanol (C₂H₆O) is combusted in air according to the following reaction: C₂H₆O(l) + O₂(g) → CO₂(g) + H₂O(l) How many grams of water would be produced by the complete combustion of 12.10 moles of ethanol in the presence of excess oxygen?
Consider the following balanced equation. Mg3N2(s) + 6H2O(l) → 3Mg(OH)2(s) + 2NH3(g) When 36.0 g of H2O reacts with excess of Mg3N2, how many grams of NH3 are produced? The molar masses are as follows: H2O = 18.02 g/mol, NH3 = 17.03 g/mol.