A compound containing only carbon, hydrogen, and oxygen is subjected to elemental analysis. Upon complete combustion, a 0.2350-g sample of the compound produced 0.304 g of CO2 and 0.1244 g of H2O. What is the empirical formula of the compound? O CH2O3 O C4H&O5 O C3H6O3 O C2H2O O C3H3O

A compound containing only carbon, hydrogen, and oxygen is subjected to elemental analysis. Upon complete combustion, a 0.2350-g sample of the compound produced 0.304 g of CO2 and 0.1244 g of H2O. What is the empirical formula of the compound? O CH2O3 O C4H&O5 O C3H6O3 O C2H2O O C3H3O

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: An organic compound containing only C, H, and possibly O was subjected to combustion analysis. A…

Q: The compound known as butylated hydroxytoluene, abbreviated as BHT, contains carbon, hydrogen, and…

A: Consider the given information is as follows; Mass of sample = 3.751 g Mass of CO2 = 11.24 g Mass of…

Q: What is the theoretical yield of MgO from the combustion of 5.25 x 10^23 atoms of Mg and 4.69 x…

Q: Part 1: Calculate the mass percentage of N in N2O4. Report your answer to 3 significant figures.…

Q: Consider the chemical formula for one molecule of methane, CH4. If instead of one molecule we had 10…

A: According to chemical formula of methane ( CH4 ) , it's very clear each molecule of methane has one…

Q: An unknown compound containing only carbon, hydrogen, and oxygen undergoes combustion analysis. The…

Q: Combustion of a hydrocarbon in a limited supply of air produces COCO in addition to CO2CO2 and…

A: You don't provide the amount of water. But based on my experience put this value. If this value is…

Q: When 5.942 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 19.34 grams…

A: When organic compounds undergo combustion, they produce carbon dioxide and water. Chemical reactions…

Q: Two chemists determined the weight of X obtainable from several samples of an organic compound,…

A: Given: Mass of X(C6H5)3 = 5.341 gm Mass of X2O3 = = 2.829 gm

Q: Tartaric acid contains only C, H and O. While it's often found in sour candies, tartaric acid is…

Q: 7.) Considering the equation 2H₂O(g) → 2 H₂ (g) + O₂(g) Calculate how many grams of 0₂ (9) Can be…

A: We will use the balanced reaction to calculate the grams of O2 produced. We can see from the…

Q: Determine the mass percent of anhydrous sodiumcarbonate (N a 2 C O 3 ) and water in sodium…

A: Given Anhydrous sodium carbonate : Na2CO3 Sodium carbonate decahydrate: Na2CO3 ·10 H2O…

Q: What the percentage yield of carbon dioxide

Q: A 6.7283 g sample of a hydrate of MgSO4 was heated to drive off all of the water of hydration. The…

A: The first step is to calculate the mass of water that was lost when the hydrate was heated. This can…

Q: A combustion analysis of a 0.4647-g sample of a compound known to contain only carbon, hydrogen, and…

Q: A 0.125 g sample of unknown hydrocarbon is prepared for combustion analysis. After the hydrocarbon…

Q: Consider the following equation: KOH(s) + CO₂(g) → K₂CO₃(s) + H₂O(l) Calculate the mass in grams of…

Q: Consider the following reaction: 10 KNO3(s) + 8 C(s) + 3 S(s) → 2 K2CO3(s) + 3 K2SO4(s) + 6…

A: Given equation: 10 KNO3(s) + 8 C(s) + 3 S(s) → 2 K2CO3(s) + 3 K2SO4(s) + 6 CO2(g) + 5 N2(g)…

Q: A binary compound of the elements X and Y is 1/3X by mass. The molar mass of element X is ¾ the…

A: Empirical Formula It is the simplest possible ratio of atoms present in a compound. To get the…

Q: Small quantities of oxygen can be prepared in the laboratory by heating potassium chlorate,…

A: For a chemical reaction to calculate the amount of product formed we can use stoichiometric…

Q: A candle flame produces easily seen specks of soot near the edges of the flame, especially when the…

A: Empirical formula: The simplest positive integer ratio of atoms present in a compound is known as…

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: A compound has an empirical formula of C2H4O and a molar mass of 88.g/mole. What is the molecular…

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

Q: Assume 100% yield. a) 10.0 g of copper sulfate are formed. b) H2SO4 is the limiting reagent. c)…

Q: Combustion analysis of 1.800 g of an unknown compound containing carbon, hydrogen, and oxygen…

A: Mass of the unknown compound = 1.800 gMass of the CO2 formed= 3.129 gMass of the H2O formed=…

Q: A 5.17 g sample of a compound with the formula CxHyOz is combusted and yields 13.0 g CO2 and 2.29 g…

Q: What is the molecular formula of a compound

A: Given :- molar mass of compound = 220 g/mol Empirical formula = P2O3. To find :…

Q: The mineral bauxite, which is mostly Al2O3, is the principal industrial source of aluminum metal.…

A: 1 ton = 106 g So, 9 ton = 9 x 106 g

Q: When 4.464 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 14.01 grams…

Q: How many grams of HCI (36.46g mol) is obtained from 71g of 79% by mass pure H,PO (98 g mol"") if the…

A: The reaction given is CaCl2 (s) + H3PO4 (l) --------> Ca3(PO4)2 (s) + HCl (g) Balancing ; Since…

Q: A molecule has an empirical formula of Ch2. 1.34 moles of the compound give 530.76 g of CO2 upon…

A: Given : We have to calculate the molecular formula.

Q: Histamine is the chemical messenger that antihistamine cold and allergy medicines try to block.…

A: Given: Histamine contains only C, H and N. Mass of Histamine combusted = 0.765 g. Mass of CO2 formed…

Q: A compound has an empirical formula of CH2. An independent analysis gave a value of 70 g/mol for its…

A: Empirical formula is defined as the simplest positive integer ratio of each atom that are supposed…

Q: An Unknown compound contains only carbon, hydrogen, nitrogen, and oxygen (C, H, N, & O). Complete…

A: We have to predict the empirical formula for benzocaine.

Q: If 0.100 g of a compound containing C, H, and O is combusted completed in an excess of oxygen and…

A: Mass of the Carbon can be calculated as

Q: Calculate the mass percent of carbon in glucose (C6H12O6).

A: Dear student, since you have asked multiple questions but according to guidelines we will solve 1st…

Q: Calculate the mass percent of 0.389 g of silicon (Si) that reacts with oxygen to form 0.832 g…

A: Given that: Si = 0.389g and SiO2 = 0.832 g…

Q: Caffeine, an extremely popular chemical amongst students and teachers alike, is composed of four…

A: Given, carbon 49.48 % hydrogen 5.19 % nitrogen 28.85 % oxygen 16.48 %

Q: s 7.86 g CO2 and 2.14 g H20. Calculate the empirical formula and molecular ula of acid given that…

A: Mass of acid = 5.24 g Mass of CO2 = 7.86 g Mass of H2O = 2.14 g

Q: An unknown hydrocarbon, which contains only C and H, is tested by combustion analysis to determine…

A: The simplest whole number ratio of the atoms in the compounds is given by the empirical formula.

Q: A chemical reaction calls for 0.125 moles of sodium acetate, NaC2H3O2. What mass, in grams, of…

A: The relationship between number of moles (n) and mass of a substance is given by: n=MassMolar…

Q: A 3.06 mg sample of a compound containing carbon, hydrogen, and oxygen underwent combustion…

A: Empirical formula: Formula containing atoms in smallest possible integer ratio Molecular formula:…

Q: Consider the following equation: KOH(s) + CO₂(g) → K₂CO₃(s) + H₂O(l) Calculate the mass in grams of…

Q: From the equation O2 + 2C = 2CO. If 2.73 moles of C are reacted with an excess of O2, How many moles…

A: The balanced equation is given below:

Q: a) Elemental analysis of an unknown sample shows its mass composition to be 49.45% carbon (C),…

A: a. What is the molecular formula of the unknown compound?Carbon (C)4.12 moles (divide 49.45g to…

Q: Determine the theoretical yield, in grams, of Fe2(CO3)3 produced from the complete reaction of 1.72…

A: The reaction taking place is 2 Fe(NO3)3 + 3 Na2CO3 ------> Fe2(CO3)3 + 6 NaNO3 Hence from the…

Q: What is the correct balanced equation for octane (C8H18)?

A: The balanced chemical equation for the oxidation of Octane (C8H18) C8H18(g) + 252O2(g) →8CO2(g) +…

Q: The reaction 2 Sb + 3 Cl2 → 2 SbCl3 has an 88.3% yield. If 4.93 g of SbCl3 is desired, what mass of…

A: The reaction is given as, 2 Sb + 3 Cl2 →2 SbCl3Yield (%) = Actual YieldTheoretical Yield x 100

Concept explainers

Mole Concept

Mole concept is a method to determine the amount of any substance that consists of some elemental particles using a grouping unit called ‘mole’. The mole concept enables one to handle the large amount of small elementary particles. The mole concept can be used in many calculations related to mole calculation, molar amount, mole ratio, and so on, which are significant in chemistry.

Question

[Roferences)
A compound containing only carbon, hydrogen, and oxygen is subjected to elemental analysis. Upon complete combustion, a 0.2350-g sample of the compound produced
0.304 g of CO2 and 0.1244 g of H2O. What is the empirical formula of the compound?
CH2O3
O C4H8O5
O C3H6O3
O C2H2O
O C3H3O
Submit Answer
Try Another Version
1 Item attempt remaining

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 Given

VIEW

Step 2 Calculations

VIEW

Step by step

Solved in 2 steps with 1 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

When 5.974 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 18.74 grams of CO2 and 7.675 grams of H2O were produced.In a separate experiment, the molar mass of the compound was found to be 56.11 g/mol. Determine the empirical formula and the molecular formula of the hydrocarbon.
When a 10.0 g sample of an unknown organic acid is subjected to combustion analysis 21.2 grams of CO2 and 3.25 g of H2O are produced. The molar mass of the acid is 165. What are the empirical formula and the molecular formula of the acid?
2. What is the compound's empirical formula if a 0.234 g sample of the compound was burned in air to produce 0.72 g of CO₂ and 0.32 g of H₂O? The compound contains only H and C. The empirical molar mass of the compound is between 70.00 g/mol and 72.00 g/mol.
An unknown compound that is composed of C, H and O atoms was submitted to a lab for determination of formula. Combustion in air of 1.230 g of the unknown compound yields 2.162 g CO2 and 1.033 g H2O. What is the empirical formula of the unknown compound?
[A table of molecular weights is given below.]How many grams of Ba(OH)2 can be produced by the reaction of 40.00 grams of Ba3N2 and 20.00 grams of H2O according to the equation below?Ba3N2 + 6 H2O → 3 Ba(OH)2 + 2 NH3Answer grams of Ba(OH)2When the reaction is complete it is found that only 39.77 grams of Ba(OH)2 were produced? Determine the %Yield for this reaction.Answer % YieldMolecular WeightsBa3N2 440.004 g/molH2O 18.015 g/molBa(OH)2 171.344 g/molNH3 17.031 g/mol
Combustion analysis of 2.796 g of an unknown compound containing carbon, hydrogen, and oxygen produced 5.597 g of CO2 and 2.268 g of H2O. What is the empirical formula of the compound?
Condisder the balanced chemical equation shown. A table of molecular weights is given below.2 SiF4 (g) + Na2CO3 (s) + H2O (l) → Na2SiF6 (s) + SiO2 (s) + CO2 (g) + 2 HF (g)• How many grams of Na2SiF6 can be produced by the reaction of 70.00 grams of SiF4 and an excess amount of all other reactants?Answer in grams of Na2SiF6Molecular WeightsSiF4 104.077 g/molNa2CO3 105.988 g/molH2O 18.015 g/molNa2SiF6 188.053 g/molSiO2 60.083 g/molCO2 44.009 g/molHF 20.006 g/mol
oron trichloride is prepared from the following reaction: 2B2O3+6Cl2+3C⟶4BCl3+3CO2 3.337 g B2O3 is mixed with 9.907 g Cl2 and 2.587 g of C.
An organic compound with a formula mass of 181.45 amu contains carbon, hydrogen, and chlorine. When 1.000 g of this compound is burned in a combustion apparatus, 1.456 g of CO2 and 0.149 g of H₂O are produced. Determine the empirical and molecular formulas of this compound.
Cryolite (Na3AlF6) is used in the production of aluminum from its ores. It is made by the reaction 6 NaOH + Al2O3 + 12 HF → 2 Na3AlF6 + 9 H2O Calculate the mass of cryolite that can be prepared by the complete reaction of 287 g Al2O3.
Balance the equation C3 H6 (g) + O2(g) ---> CO2 (g) + O(g)
How many grams of KCIO3 are needed to form 26.2 g of O, ? 2 KCIO, (s) → 2 KCI(s) + 3 0,(g) Ston 1