**Chemical Analysis of a Compound**A sample of 8.50 grams of a certain compound, known to consist of carbon, hydrogen, and possibly oxygen, is completely burned in excess oxygen. The molecular molar mass of the compound is 70 g/mol. Upon combustion, the mass of the resulting products is meticulously measured, yielding 26.72 grams of carbon dioxide (CO₂) and 10.94 grams of water (H₂O). Use this information to determine the molecular formula of compound X.

(1)The amount of carbon and hydrogen is calculated from the grams of CO2 and H2O

8.50 of a certain Compound, known to be made of carbon, hydrogen and perhaps oxygen, and to have a molecular molar mass of 70. g/mol, is burned completely in excess oxygen, and the mass of the products carefully measured: Carbon Dioxide: 26.72 g Water: 10.94 g Use this info to find the molecular formula of X

8.50 of a certain Compound, known to be made of carbon, hydrogen and perhaps oxygen, and to have a molecular molar mass of 70. g/mol, is burned completely in excess oxygen, and the mass of the products carefully measured: Carbon Dioxide: 26.72 g Water: 10.94 g Use this info to find the molecular formula of X

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: 7.50 g of a certain Compound X, known to be made of carbon, hydrogen and perhaps oxygen, and to have…

A: Given carbon dioxide = 19.42 g water=3.97 g

Q: A 7.73 g sample of an organic compound containing carbon, hydrogen, and oxygen was burned in excess…

A: Given: Compound contains only C, H and O. Mass of compound combusted = 7.73 g. Mass of CO2 produced…

Q: Nitric oxide (NO) is made from the oxidation of ammonia (NH3) based on the BALANCED equation: 4…

A: The given balanced equation is- 4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g) As per this equation, 4…

Q: 4.00 g of a certain Compound X, known to be made of carbon, hydrogen and perhaps oxygen, and to have…

A: Given that, 4.0 g of a compound X is made of carbon, hydrogen and perhaps oxygen. The molecular…

Q: A 2.500g sample of an unknown hydrocarbon (CxHyOz) is put in a combustion chamber. From the…

A: We have to calculate the mass of O .

Q: completely in excess oxygen, and the mass of the products carefully measured: product mass carbon…

A: Explanation given as follows

Q: 4.00 g of a certain Compound X, known to be made of carbon, hydrogen and perhaps oxygen, and to have…

Q: 2.50 g of a certain Compound X, known to be made of carbon, hydrogen and perhaps oxygen, and to have…

Q: 6.50 g of a certain Compound X, known to be made of carbon, hydrogen and perhaps oxygen, and to have…

Q: A 2.86 g sample of a compound consisting of carbon, hydrogen, oxygen, nitrogen, and sulfur was…

A: Given, mass of 2.86 g sample of a compound produced 1.61 g CO2 and 0.989 g H2O.Moles of CO2 and H2O…

Q: Hydrogen fluoride is one of the few substances that react with glass (which is made of silicon…

A: we have to calculate moles of HF mass of water produced

Q: 3.00 g of a certain Compound X, known to be made of carbon, hydrogen and perhaps oxygen, and to have…

A: Given that,Mass of compound, which is made up of carbon, hydrogen and oxygen = Molecular mass of…

Q: 8.50 g of a certain Compound X, known to be made of carbon, hydrogen and perhaps oxygen, and to have…

Q: Consider the following unbalanced reaction: D4(s) + X2(g) --> DX3(g) Determine the amount of…

A: The % yield is equal to the ratio of actual yield to the theoretical yield multiplied by 100. The…

Q: 8.15g of phosphorus reacts with bromine to form 71.22g of phosphorus tribromide. Calculate the…

Q: 1.50 g of a certain Compound X, known to be made of carbon, hydrogen and perhaps oxygen, and to have…

A: Step 1: Step 2: Step 3: Step 4:

Q: For the combustion of butanol (C4H10O), what mass (in g) of butanol must we react to produce 60.7 g…

A: Step 1:- First, a balanced chemical equation for the combustion of butanol is written. Step 2: Then…

Q: 8.50 g of a certain Compound X, known to be made of carbon, hydrogen and perhaps oxygen, and to have…

A: Given : Mass of Compound X = 8.50 g Molar mass of Compound = 128 g/mol Mass of CO2 = 29.22 g Mass…

Q: A student performs an experiment like the one you saw in Experiment 8. The student determines that…

A: Using the concept of weight percentage by mass we can calculate the total mass.

Q: An air conditioner compressor contains pure CClF3, also known as the refrigerant R-13. CClF3 has a…

A: We know that, density can be expressed as the mass per unit volume, i.e.…

Q: Ammonium perchlorate NH4ClO4 is the solid rocket fuel that was used by the U.S. Space Shuttle and is…

A: The objective of this question is to determine the mass of water produced by the reaction of 6.89g…

Q: 5.00 g of a certain Compound X, known to be made of carbon, hydrogen and perhaps oxygen, and to have…

Q: An unknown compound contains only C, H, and O. Combustion of 7.00 g of this compound produced 15.9 g…

Q: For the combustion of butanol (C4H10O), what mass (in g) of butanol must we react to produce 60.7 g…

A: The combustion of butanol (C4H10O) in the presence of oxygen (O2) produces water (H2O) and carbon…

Q: 1.50 g of a certain Compound X, known to be made of carbon, hydrogen and perhaps oxygen, and to have…

Q: 2.00 g of a certain Compound X, known to be made of carbon, hydrogen and perhaps oxygen, and to have…

A: Empirical formula :- The formula which gives the simplest whole number ratio of atoms of various…

Q: 1.00 g of a certain Compound X, known to be made of carbon, hydrogen and perhaps oxygen, and to have…

Q: Consider the following balanced chemical reaction: CaSO3 + 2HCl → SO2 + H2O + CaCl2 If 750.0 grams…

A: Calcium sulfide reacts with hydrochloric acid to form sulfur dioxide, water, and calcium chloride.…

Q: A classic SUV features a 194 L gas tank. Assuming a molecular formula of C8H18 for gasoline and…

A: Consider the balanced reaction for the complete combustion of gasoline to give CO2 and H2O is as…

Q: 5. Lead metal can be extracted from a mineral called galena, which contains 83.2% lead by mass. A…

A: Given,mass of ore = 6.75 kgmass percent of lead in the galena = 83.2 %mass percent of galena in the…

Q: A mixture of 132.1 g of P and 136.5 g of O, reacts completely to form P¸O, and PO,0. Find the masses…

A: We have to calculate the mass of product formed.

Q: Morphine sulfate used for severe pain relief is an opiate alkaloid isolated from the plant Papaver…

A: While writing the chemical formula, the number that represents the number of atoms is written as…

Q: 8.50 g of a certaln Compound X, known to be made of carbon, hydrogen and perhaps oxygen, and to have…

Concept explainers

Stoichiometry

Stoichiometry is a chemical division that evaluates the quantitative content of the chemical process with the help of the reacting molecules or products taking part in the reaction. The term “stoicheion” in “Stoichiometry”, is an old Greek term for "element" whereas “metron” means "measure".

Question

**Chemical Analysis of a Compound**

A sample of 8.50 grams of a certain compound, known to consist of carbon, hydrogen, and possibly oxygen, is completely burned in excess oxygen. The molecular molar mass of the compound is 70 g/mol. Upon combustion, the mass of the resulting products is meticulously measured, yielding 26.72 grams of carbon dioxide (CO₂) and 10.94 grams of water (H₂O).

Use this information to determine the molecular formula of compound X.

Expert Solution

This question has been solved!

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

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1: Calculate mass of each element

VIEW

Step 2: Calculate percent composition of each element

VIEW

Step 3: Calculate moles of each element

VIEW

Step 4: Calculate empirical formula

VIEW

Step 5: Calculate molecular formula

VIEW

Step 6: Final answer

VIEW

Solution

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 7 steps with 7 images

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

4.33 g sample of a compound consisting of carbon, hydrogen, oxygen, nitrogen, and sulfur was combusted in excess oxygen. This produced 6.38 g CO2 and 2.88 g H2O. A second sample of this compound with a mass of 5.05 g produced 2.70 g SO3. The third sample of this compound with a mass of 6.95 g produced 2.94 g of HNO3. What is the empirical formula of the compound?
An acid, HEI, is formed from a hypothetical element, El, and a subsequent aqueous solution is created with the acid and water. The solution is meaured to be 28.55% HEI by weight. Calculate the mol% of the acid in the solution. Atomic mass: H: 1.00784 g/mol O: 15.999 g/mol EI: 158.67986 g/mol
8.50 g of a certain compound X, known to be made of carbon, hydrogen and perhaps oxygen, and to have a molecular molar mass of 176. g/mol, is burned completely in excess oxygen, and the mass of products carefully measured: product mass carbon dioxide 12.75 g water 3.48 g Use this information to find the molecular formula of X.
DDT, an insecticide harmful to fish, birds, and humans, is produced by the following reaction: 2C6H5 Cl + C₂2 HOC13 → C14H9 Cl5 + H₂O chlorobenzene chloral DDT In a government lab, 1167 g of chlorobenzene is reacted with 470 g of chloral. a. What mass of DDT is formed, assuming 100% yield? g b. Which reactant is limiting? Which is in excess? is limiting. Mass= is in excess. c. What mass of the excess reactant is left over? g in excess d. If the actual yield of DDT is 285.0 g, what is the percent yield? Percent yield = % Mass=
6.00 g of a certain Compound X , known to be made of carbon, hydrogen and perhaps oxygen, and to have a molecular molar mass of 46. g/mol , is burned completely in excess oxygen, and the mass of the products carefully measured: product mass carbon dioxide 11.48g water 7.05g Use this information to find the molecular formula of X .
Ammonium perchlorate (NH, CIO) is the solid rocket fuel that was used by the U.S. Space Shuttle and is used in the Space Launch System (SLS) of Artemis rocket. It reacts with itself to produce nitrogen gas (N₂), chlorine gas (C1₂), oxygen gas (O₂), water (H₂O), and a great deal of energy. What mass of oxygen gas is produced by the reaction of 3.73 g of ammonium perchlorate? Be sure your answer has the correct number of significant digits. 0 X
9. Isobutylene is a hydrocarbon used in the manufacture of synthetic rubber. When 0.847 g of isobutylene was subjected to combustion analysis, 2.657 g CO₂ and 1.089 g H₂O were produced. a. What is the empirical formula of isobutylene? b. What is the molecular formula of isobutylene if the molar mass is 60.077 g/mol?
Vitamin C, an antioxidant present in citrus fruits, contains only C, H, and O. Combustion of 10.0 g of vitamin C produces 14.99 g of CO₂ and 4.092 g of H₂O. Determine the molar mass of the compound if it is between 150.0 and 220.0 g/mol.
When mixed, these compounds react as follows. This is balanced as written: Na2CO3(s) + 2 CH3CO2H(aq) --> CO2(g) + H₂O() +2 NaCH3CO2(aq) One of the products is the gas carbon dioxide (CO₂). Based on this reaction, for every ONE molecule of sodium carbonate (Na₂CO3) that reacts, how many molecules of GAS will form? 01 3 O N
2.50 g of a certain Compound X, known to be made of carbon, hydrogen and perhaps oxygen, and to have a molecular molar mass of 138. g/mol, is burned completely in excess oxygen, and the mass of the products carefully measured: product 4 carbon dioxide 0 water Use this information to find the molecular formula of X. mass 5.58 g 0.98 g S A
9. Vanillin, the dominant flavoring in vanilla, contains C, H, and O. When 1.05 g of this substance is completely combusted, 2.43 g of CO2 and 0.50 g of H2O are produced. What is the empirical formula of vanillin?