3. Chemical Reactions

Empirical Formula

Elemental Analysis: Empirical and Molecular Formulas

Empirical Formula & Molecular Formula Determination From Percent Composition

Calculate the empirical formula for each stimulant based on its
elemental mass percent composition.
a. nicotine (found in tobacco leaves): C 74.03%, H 8.70%,
N 17.27%

What are the molecular and empirical formulas for each of
the following compounds?
Write the molecular formula for the following compound.
<img src="https://lightcat-files.s3.amazonaws.com/problem_images/7426cb5052f71ed3-1660563479727.jpg" alt="" />

The elemental mass percent composition of ascorbic acid (vitamin
C) is 40.92% C, 4.58% H, and 54.50% O. Determine the
empirical formula of ascorbic acid.

Determine the empirical formulas of the compounds with
the following compositions by mass:
(b) 57.5% Na, 40.0% O, and 2.5% H

Introduction to Combustion Analysis, Empirical Formula & Molecular Formula Problems

The structural formulas of the compounds n-butane and 
isobutane are shown below. (b) Determine the empirical formula of each. 
<img src="https://lightcat-files.s3.amazonaws.com/problem_images/6c5393c016646bb8-1660322785308.jpg" alt="" />

A copper wire having a mass of 2.196 g was allowed to react with an excess of sulfur. The excess sulfur was then burned, yielding SO2 gas. The mass of the copper sulfide produced was 2.748 g.
(b) What is its empirical formula?

An herbicide is found to contain only C, H, N, and Cl. 
The complete combustion of a 100.0-mg sample of the 
herbicide in excess oxygen produces 83.16 mL of CO2 and 
73.30 mL of H2O vapor expressed at STP. A separate analysis 
shows that the sample also contains 16.44 mg of Cl. 
(c) What other information would you need to know about this 
compound to calculate its true molecular formula?

Give the empirical formula of each of the following compounds
if a sample contains (b) 2.10 g nickel and 0.58 g oxygen

Determine the empirical formula of each of the following 
compounds if a sample contains (a) 3.92 mol C, 5.99 mol H, 
and 2.94 mol O

Write the empirical formula corresponding to each of 
the following molecular formulas: (c) C4H8O2

The following diagram represents the collection of CO2 and 
H2O molecules formed by complete combustion of a hydrocarbon. 
What is the empirical formula of the hydrocarbon?

Silver metal reacts with chlorine (Cl2) to yield silver chlo-ride. If 2.00 g of Ag reacts with 0.657 g of Cl2, what is the empirical formula of silver chloride?

Determine the empirical formulas of the compounds with 
the following compositions by mass: 
(c) 60.0% C, 4.4% H, and the remainder O

Heating elemental cesium and platinum together for two days at 973 K gives a dark red ionic compound that is 57.67% Cs and 42.33% Pt. 
(a) What is the empirical formula of the compound?

How to calculate Empirical Formula? 3 Easy Steps

Molecular Formula  | Chemistry | Homework Help

A chemist decomposes samples of several compounds; the
masses of their constituent elements are listed. Calculate the
empirical formula for each compound.
b. 2.677 g Ba, 3.115 g Br

Determine the molecular and empirical formulas of the following: 
(b) the compound silicon tetrachloride, 
which has a silicon atom and four chlorine atoms and is used in 
the manufacture of computer chips

Two substances have the same molecular and empirical formulas.
Does this mean that they must be the same compound?

A compound composed of carbon, hydrogen, and chlorine contains 4.19 x 1023 hydrogen atoms. If 9.00 g of the compound also contains 55.0% chlorine by mass, what is the empirical formula?

Write the empirical formula corresponding to each of 
the following molecular formulas: (b) C8H10

The elemental mass percent composition of ibuprofen (a nonsteroidal
anti-inflammatory drug [NSAID]) is 75.69% C, 8.80% H,
and 15.51% O. Determine the empirical formula of ibuprofen.

What are the empirical formulas of each of the following substances?
(c) Zircon, a mineral from which cubic zirconia is made: 34.91% O, 15.32% Si, 49.77% Zr

Determine the empirical formulas of the compounds with
the following compositions by mass:
(a) 74.0% C, 8.7% H, and 17.3% N

Dimethylhydrazine, a colorless liquid used as a rocket fuel, is 40.0% C, 13.3% H, and 46.7% N. What is the empirical formula? (LO 3.11) 
(a) CH4N9 
(b) CH2N
(c) C2H4N 
(d) C2H5N2

What are the empirical formulas of substances with the following mass percent compositions? 
(b) Ilmenite (a titanium-containing ore): 31.63% O, 31.56% Ti, 36.81% Fe

Ferrocene, a substance proposed for use as a gasoline additive, has the percent composition 5.42% H, 64.56% C, and 30.02% Fe. What is the empirical formula of ferrocene?

Finding and Calculating an Empirical Formula of a Compound | How to Pass Chemistry

A chemist decomposes samples of several compounds; the
masses of their constituent elements are listed. Calculate the
empirical formula for each compound.
c. 2.128 g Be, 7.557 g S, 15.107 g O

C2H4O2

The empirical formula for this compound is CH2O.

 The empirical formula for this compound is HO. 

Ozone, O3, is not a compound.

 Correct, in this case the molecular formula is the simplest whole number ratio. 

The empirical formula for this compound is BH3.

 Empirical formulas give the relative number of atoms of each element in a compound. 

 Which of the following could be both a molecular formula and an empirical formula? 

The following diagram represents the collection of elements
formed by a decomposition reaction. 
(b) Could you draw a diagram representing the molecules
of the compound that had been decomposed? Why or why
not?
<img src="https://lightcat-files.s3.amazonaws.com/problem_images/c31ae922710a20c5-1664221006383.jpg" alt="" />

The following diagram represents the collection of elements
formed by a decomposition reaction. (a) If the blue spheres
represent N atoms and the red ones represent O atoms,
what was the empirical formula of the original compound?
<img src="https://lightcat-files.s3.amazonaws.com/problem_images/049fecb73fc819c2-1661537187093.jpg" alt="" />

What is the empirical formula of stannous fluoride, the first fluoride compound added to toothpaste to protect teeth against decay? Its mass percent composition is 24.25% F, 75.75% Sn.

The structural formulas of the compounds n-butane and
isobutane are shown below. 
(c) Which formulas—empirical, molecular, or structural—allow
you determine these are different compounds?
<img src="https://lightcat-files.s3.amazonaws.com/problem_images/a6ce146a3f4bd618-1660564610422.jpg" alt="" />

Calculate the empirical formula for each natural flavor based on 
its elemental mass percent composition. 
b. vanillin (responsible for the taste and smell of vanilla): 
C 63.15%, H 5.30%, O 31.55%

Elemental analysis of a sample of an ionic compound showed 2.82 g of Na, 4.35 g of Cl, and 7.83 g of O. What is the empirical formula of the compound?

A 45.2-mg sample of phosphorus reacts with selenium to form
131.6 mg of the selenide. Determine the empirical formula of
phosphorus selenide.

Reaction of gaseous fluorine with compound X yields a sin- gle product Y, whose mass percent composition is 61.7% F and 38.3% Cl. (a) What is a probable molecular formula for product Y, and what is a probable formula for X?

A compound that contains only carbon, hydrogen, and oxygen is composed of 48.64% C and 43.2% O by mass. What is the empirical formula of this compound?

Combustion analysis of a 31.472 mg sample of the widely used flame retardant Decabrom gave 1.444 mg of CO2. Is the molecular formula of Decabrom C12Br10 or C12Br10O?

What are the empirical formulas of substances with the following mass percent compositions? 
(c) Sodium thiosulfate (photographic “fixer”): 30.36% O, 29.08% Na, 40.56% S

Give the empirical formula of each of the following compounds 
if a sample contains (c) 26.56% K, 35.41% Cr, and 38.03% O by mass.

Calculate the empirical formula for each natural flavor based on
its elemental mass percent composition.
a. methyl butyrate (component of apple taste and smell):
C 58.80%, H 9.87%, O 31.33%

What are the empirical formulas of each of the following substances?
(b) Magnetite, a naturally occurring magnetic mineral: 72.36% Fe, 27.64% O

A chemist decomposes samples of several compounds; the
masses of their constituent elements are listed. Calculate the
empirical formula for each compound.
a. 1.245 g Ni, 5.381 g I

Write the empirical formula corresponding to each of
the following molecular formulas: (a) Al2Br6

 typically consist of a metal and a nonmetal attracted to each other by electrostatic forces. 

 Covalent compounds are characterized by two or more nonmetals sharing electrons. 

 typically consist of a metal and a nonmetal held together by shared electrons. 

 form when two nonmetals share electrons upon forming a chemical bond. 

 Correct, many covalent compounds form when two nonmetals share electrons. 

 form when two metals share electrons upon forming a chemical bond 

 Review the formation of covalent bonds. 

Determine the empirical formulas of the compounds with
the following compositions by mass:
(a) 42.1% Na, 18.9% P, and 39.0% O

Determine the molecular and empirical formulas of the following:
(a) the organic solvent benzene, which has six carbon atoms
and six hydrogen atoms

Empirical Formula and Molecular Formula Introduction

Empirical Formula Example 1

Determine the empirical formula of each of the following
compounds if a sample contains (b) 12.0 g calcium and 2.8 g nitrogen

Write the empirical formula corresponding to each of 
the following molecular formulas: (e) C6H4Cl2

Writing Empirical Formula Practice Problems

Give the empirical formula of each of the following compounds
if a sample contains (a) 0.052 mol C, 0.103 mol
H, and 0.017 mol O

Determine the empirical formula of each of the following 
compounds if a sample contains (c) 89.14% Au and 10.86% O by mass.

What are the empirical formulas of each of the following substances?
(a) Ibuprofen, a headache remedy: 75.69% C, 15.51% O, 8.80% H

What are the empirical formulas of substances with the following mass percent compositions?
(a) Aspirin: 4.48% H, 60.00% C, 35.52% O

Under special conditions, sulfur reacts with anhydrous liquid
ammonia to form a binary compound of sulfur and nitrogen.
The compound is found to consist of 69.6% S and
30.4% N. Measurements of its molecular mass yield a value
of 184.3 g>mol. The compound occasionally detonates on
being struck or when heated rapidly. The sulfur and nitrogen
atoms of the molecule are joined in a ring. All the bonds in
the ring are of the same length. (a) Calculate the empirical
and molecular formulas for the substance.

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1. Intro to General Chemistry

2. Atoms & Elements

4. BONUS: Lab Techniques and Procedures

5. BONUS: Mathematical Operations and Functions

6. Chemical Quantities & Aqueous Reactions

7. Gases

8. Thermochemistry

9. Quantum Mechanics

10. Periodic Properties of the Elements

11. Bonding & Molecular Structure

12. Molecular Shapes & Valence Bond Theory

13. Liquids, Solids & Intermolecular Forces

14. Solutions

15. Chemical Kinetics

16. Chemical Equilibrium

17. Acid and Base Equilibrium

18. Aqueous Equilibrium

19. Chemical Thermodynamics

20. Electrochemistry

21. Nuclear Chemistry

22. Organic Chemistry

23. Chemistry of the Nonmetals

24. Transition Metals and Coordination Compounds

[BOOK CHEM] Clutch Version

The empirical formula gives the relative number of atoms.&nbsp;

Percent Yield

The Percent Yield determines how successful the product yield is in a chemical reaction.&nbsp;

Molecular Formula

The&nbsp;molecular formula gives the actual number of atoms.

Naming Ionic Compounds

An ionic compound is composed of a positive ion and a negative ion.&nbsp;

Functional Groups in Chemistry

The Functional Group is the portion of a molecule that is responsible for its chemical reactivity.&nbsp;

Naming Molecular Compounds

Molecular Compounds, also known as covalent compounds, contain only non-metals bonded together.&nbsp;

Naming Ionic Hydrates

An Ionic Hydrate is an ionic compound that is linked to at least one molecule of H2O.&nbsp;

Stoichiometry

Stoichiometry deals with the numerical relationship between compounds in a balanced chemical equation.

Writing Ionic Compounds

Determining the charges of a cation and anion are fundamental in Writing Ionic Compounds.

Polyatomic Ions

Polyatomic Ions are groups of multiple elements that possess a charge.

Balancing Chemical Equations

Balancing Chemical Equations is the first step in future chemical calculations.

Limiting Reagent

The Limiting Reagent represents the compound that is totally consumed in the reaction.&nbsp;

Combustion Analysis

Under Combustion Analysis, the empirical formula of a compound is determined through a combustion reaction.&nbsp;

Mass Percent

Mass Percent is the percentage of a particular element within a compound.&nbsp;

Combustion Apparatus

A Combustion Apparatus vaporizes a sample into gases to later determine its formula.

Naming Acids

Acids, for the most part, are covalent compounds that begin with a hydrogen.&nbsp;