3. Chemical Reactions

Limiting Reagent

Introduction to Limiting Reactant and Excess Reactant

Calculate the theoretical yield of the product (in moles) for each 
initial amount of reactants. 
Ti(s) + 2 Cl2( g)¡TiCl4(s) 
b. 7 mol Ti, 17 mol Cl2

How many grams of each product result from the following reactions, and how many grams of which reactant is left over? 
(a)

Acrylonitrile (C­3H3N) is the starting material for many synthetic carpets and fabrics. It is produced by the following reaction:&nbsp;2 C3H6 (g) + 2 NH3 (g) + 3 O2 (g) &nbsp;→ 2 C3H3N (g)&nbsp;+&nbsp;6 H2O (g)If 12.0 g C3H6, 10.0 g NH­3, and 5.0 g O2 react, what mass of acrylonitrile can be produced, assuming 100% yield?

When benzene 1C6H62 reacts with bromine 1Br22, bromobenzene
1C6H5Br2 is obtained:
C6H6 + Br2¡C6H5Br + HBr
(a) When 30.0 g of benzene reacts with 65.0 g of bromine, what
is the theoretical yield of bromobenzene?

The following diagram represents the reaction of A2 (red spheres) with B2 (blue spheres):
<img src="https://lightcat-files.s3.amazonaws.com/problem_images/98775a1cebe51e0c-1668519900111.jpg" alt="" />
(a) Write a balanced equation for the reaction, and identify the limiting reactant. 
(b) How many moles of product can be made from 1.0 mol of A2 and 1.0 mol of B

Ammonia and hydrogen chloride react to form solid
ammonium chloride:
NH31g2 + HCl1g2¡NH4Cl1s2
Two 2.00-L flasks at 25 °C are connected by a valve,
as shown in the drawing. One flask contains 5.00 g
of NH31g2, and the other contains 5.00 g of HCl(g). When
the valve is opened, the gases react until one is completely
consumed. (a) Which gas will remain in the system after
the reaction is complete?

For the reaction shown, calculate the theoretical yield of 
product (in grams) for each initial amount of reactants. 
2 Al(s) + 3 Cl2( g)¡2 AlCl3(s) 
c. 0.235 g Al, 1.15 g Cl2

Elemental phosphorus reacts with chlorine gas according to the
equation:
P4(s) + 6 Cl2( g)¡4 PCl3(l )
A reaction mixture initially contains 45.69 g P4 and 131.3 g Cl2.
Once the reaction has occurred as completely as possible, what
mass (in g) of the excess reactant remains?

The reaction between ethyl iodide and hydroxide ion in
ethanol 1C2H5OH2 solution, C2H5I1alc2 + OH- 1alc2 ¡
C2H5OH1l2 + I - 1alc2, has an activation energy of
86.8 kJ>mol and a frequency factor of 2.10 * 1011 M-1 s-1.
(c) Which reagent in
the reaction is limiting, assuming the reaction proceeds to
completion?

Limiting Reagents and Percent Yield

Nitrogen 1N22 and hydrogen 1H22 react to form ammonia
1NH32. Consider the mixture of N2 and H2 shown in the
accompanying diagram. The blue spheres represent N, and
the white ones represent H.
(d) Are any reactant molecules left over, based on the diagram?

When magnesium metal is burned in air (Figure 3.6), two 
products are produced. One is magnesium oxide, MgO. The 
other is the product of the reaction of Mg with molecular 
nitrogen, magnesium nitride. When water is added to magnesium 
nitride, it reacts to form magnesium oxide and ammonia 
gas. (d) Magnesium nitride can 
also be formed by reaction of the metal with ammonia at high 
temperature. Write a balanced equation for this reaction. If a 
6.3-g Mg ribbon reacts with 2.57 g NH31g2 and the reaction 
goes to completion, which component is the limiting reactant? 
What mass of H21g2 is formed in the reaction?

Consider the mixture of propane, C3H8, and O2 shown here. 
(c) How many molecules of CO2, H2O, C3H8, 
and O2 will be present if the reaction goes to completion? 
<img src="https://lightcat-files.s3.amazonaws.com/problem_images/444553f22916b742-1660582038536.jpg" alt="" />

How To: Find Limiting Reagent (Easy steps w/practice problem)

If 2.0 mol CH3CH2CH2COOH, 2.0 mol C4H10, and 2.0 mol
C6H6 are completely combusted in oxygen, which one
produces the least? Explain.

The reaction of tungsten hexachloride (WCl6) with bismuth gives hexatungsten dodecachloride (W6Cl12). WCl6 + Bi ---> W6Cl12 + BiCl3 Unbalanced
(c) When 228 g of WCl6 react with 175 g of Bi, how much W6Cl12 is formed based on the limiting reactant?

How many grams of each product result from the following reactions, and how many grams of which reactant is left over? 
(b)

Solutions of sulfuric acid and lead(II) acetate react to form solid
lead(II) sulfate and a solution of acetic acid. If 5.00 g of sulfuric
acid and 5.00 g of lead(II) acetate are mixed, calculate the number
of grams of sulfuric acid present in the mixture after the reaction is complete.

When a mixture of 10.0 g of acetylene 1C2H22 and 10.0 g of
oxygen 1O22 is ignited, the resulting combustion reaction
produces CO2 and H2O. 
(c) How many grams of C2H2 are present after the reaction is complete?

Calculate the theoretical yield of product (in moles) for each 
initial amount of reactants. 
3 Mn(s) + 2 O2( g)¡Mn3O4(s) 
b. 4 mol Mn, 7 mol O2

Assume that you have 1.39 mol of H2 and 3.44 mol of N2. How many grams of ammonia (NH3) can you make, and how many grams of which reactant will be left over?

3 H2 + N2 --> NH3

Solutions of sodium carbonate and silver nitrate react to
form solid silver carbonate and a solution of sodium nitrate.
A solution containing 3.50 g of sodium carbonate is mixed
with one containing 5.00 g of silver nitrate. How many grams
of sodium carbonate are present after the reaction is complete?

Zinc sulfide reacts with oxygen according to the reaction:
2 ZnS(s) + 3 O2( g)¡2 ZnO(s) + 2 SO2( g)
A reaction mixture initially contains 4.2 mol ZnS and 6.8 mol
O2. Once the reaction has occurred as completely as possible,
what amount (in moles) of the excess reactant remains?

Sodium borohydride, NaBH4, a substance used in the synthesis of many pharmaceutical agents, can be prepared by reaction of NaH with B2H6 according to the equation 2 NaH + B2H6 ---> 2 NaBH4
(b) Which reactant is limiting, and how many grams of the excess reactant will be left over?

Limestone (CaCO3) reacts with hydrochloric acid according to the equation CaCO3 + 2 HCl ---> CaCl2 + H2O + CO2. If 1.00 mol of CO2 has a volume of 22.4 L under the reaction conditions, how many liters of gas can be formed by reaction of 2.35 g of CaCO3 with 2.35 g of HCl? Which reactant is limiting?

How to Find Limiting Reactants | How to Pass Chemistry

Aluminum hydroxide reacts with sulfuric acid as follows: 
2 Al1OH231s2 + 3 H2SO41aq2¡Al21SO4231aq2 + 6 H2O1l2 
How many moles of 
the excess reactant remain after the completion of the reaction?

Consider the mixture of ethanol, C2H5OH, and O2 shown in
the accompanying diagram. 
(c) How many molecules of CO2, H2O, C2H5OH, and O2 will
be present if the reaction goes to completion?
<img src="https://lightcat-files.s3.amazonaws.com/problem_images/28814d81029dd10d-1660583326910.jpg" alt="" />

If 2.00 moles of nitrogen and 5.50 moles of hydrogen are placed in a reaction vessel and react to form ammonia, what is the theoretical yield of ammonia (NH3)? (LO 3.8) 
N2(g) + 3 H2(g) --> 2 NH3(g)
(a) 31.2 g 
(b) 62.3 g
(c) 93.7 g 
(d) 34.1

Hydrogen and chlorine react to yield hydrogen chloride: H2 + Cl2 ¡ 2 HCl. How many grams of HCl are formed from reaction of 3.56 g of H2 with 8.94 g of Cl2? Which reactant is limiting?

Find the limiting reactant for each initial amount of reactants.
4 Al(s) + 3 O2( g)¡2 Al2O3(s)
a. 1 mol Al, 1 mol O2
b. 4 mol Al, 2.6 mol O2
c. 16 mol Al, 13 mol O2
d. 7.4 mol Al, 6.5 mol O2

Iron(II) sulfide reacts with hydrochloric acid according to the
reaction:
FeS(s) + 2 HCl(aq)¡FeCl2(s) + H2S(g)
A reaction mixture initially contains 0.223 mol FeS and
0.652 mol HCl. Once the reaction has occurred as completely as
possible, what amount (in moles) of the excess reactant
remains?

Consider the mixture of ethanol, C2H5OH, and O2 shown in
the accompanying diagram. (b) Which reactant is the limiting reactant?
<img src="https://lightcat-files.s3.amazonaws.com/problem_images/afe8ef67b911bc42-1660582767574.jpg" alt="" />

Nitrogen monoxide and oxygen react to form nitrogen dioxide.
Consider the mixture of NO and O2 shown in the accompanying
diagram. The blue spheres represent N, and the red ones
represent O. (a) How many molecules of NO2 can be formed,
assuming the reaction goes to completion?

Iron(III) oxide reacts with carbon monoxide according to the
equation:
Fe2O3(s) + 3 CO(g)¡2 Fe(s) + 3 CO2( g)
A reaction mixture initially contains 22.55 g Fe2O3 and 14.78 g
CO. Once the reaction has occurred as completely as possible,
what mass (in g) of the excess reactant remains?

One of the steps in the commercial process for converting
ammonia to nitric acid is the conversion of NH3 to NO:
4 NH31g2 + 5 O21g2¡4 NO1g2 + 6 H2O1g2
In a certain experiment, 2.00 g of NH3 reacts with 2.50 g of
O2. (a) Which is the limiting reactant?

How to Find Limiting Reactant (Quick & Easy) Examples, Practice Problems, Practice Questions

Solutions of sodium carbonate and silver nitrate react to
form solid silver carbonate and a solution of sodium nitrate.
A solution containing 3.50 g of sodium carbonate is mixed
with one containing 5.00 g of silver nitrate. How many grams
of silver carbonate are present after the reaction is complete?

Aluminum hydroxide reacts with sulfuric acid as follows:
2 Al1OH231s2 + 3 H2SO41aq2¡Al21SO4231aq2 + 6 H2O1l2
Which is the limiting reactant when 0.500 mol Al1OH23 and
0.500 mol H2SO4 are allowed to react?

For the reaction shown, calculate the theoretical yield of the 
product (in grams) for each initial amount of reactants. 
Ti(s) + 2 F2( g)¡TiF4(s) 
c. 0.233 g Ti, 0.288 g F2

Gaseous iodine pentafluoride, IF5, can be prepared by the 
reaction of solid iodine and gaseous fluorine: 
I21s2 + 5 F21g2¡2 IF51g2 
A 5.00-L flask containing 10.0 g of I2 is charged with 
10.0 g of F2, and the reaction proceeds until one of 
the reagents is completely consumed. After the reaction 
is complete, the temperature in the flask is 125 °C. 
(d) What is the total mass of reactants and products in the flask?

Solutions of sulfuric acid and lead(II) acetate react to form solid
lead(II) sulfate and a solution of acetic acid. If 5.00 g of sulfuric
acid and 5.00 g of lead(II) acetate are mixed, calculate the number
of grams of lead(II) acetate present in the mixture after the reaction is complete.

Treatment of gold metal with BrF3 and KF produces Br2 and
KAuF4, a salt of gold. Find the mass of the gold salt that
forms when a 73.5-g mixture of equal masses of all three reactants
is prepared.

Limiting Reactants and Percent Yield

Find the limiting reactant for each initial amount of reactants.
2 Na(s) + Br2( g)¡2 NaBr(s)
c. 2.5 mol Na, 1 mol Br2

How many grams of the dry-cleaning solvent 1,2-dichloroethane (also called ethylene chloride), C2H4Cl2, can be prepared by reaction of 15.4 g of ethylene, C2H4, with 3.74 g of Cl2?

(c) Why should you base your choice of which compound is
the limiting reactant on its number of initial moles, not on
its initial mass in grams?

The diagram represents a mixture of AB2 and B2 before it reacts to form AB3. (Red spheres = A, blue spheres = B.) Which reactant is limiting, and how many AB3 molecules are formed? (LO 3.7) <img src="https://lightcat-files.s3.amazonaws.com/problem_images/11845033f933917c-1668462149999.jpg" alt="" /> 
(a) B2 is limiting, and 10 molecules of AB3 are formed. 
(b) B2 is limiting, and 4 molecules of AB3 are formed. 
(c) AB2 is limiting, and 6 molecules of AB3 are formed. 
(d) AB2 is limiting, and 4 molecules of AB3 are formed

Limiting Reagent Example 1

Sodium borohydride, NaBH4, a substance used in the synthesis of many pharmaceutical agents, can be prepared by reaction of NaH with B2H6 according to the equation 2 NaH + B2H6 ---> 2 NaBH4
(a) How many grams of NaBH4 can be prepared by reaction between 8.55 g of NaH and 6.75 g of B2H6?

One of the steps in the commercial process for converting
ammonia to nitric acid is the conversion of NH3 to NO:
4 NH31g2 + 5 O21g2¡4 NO1g2 + 6 H2O1g2
In a certain experiment, 2.00 g of NH3 reacts with 2.50 g of
O2. (c) How many grams of the excess reactant
remain after the limiting reactant is completely consumed?

When a mixture of 10.0 g of acetylene 1C2H22 and 10.0 g of
oxygen 1O22 is ignited, the resulting combustion reaction
produces CO2 and H2O. 
(c) How many grams of CO2 are present after the reaction is complete?

GCSE Chemistry - What is a Limiting Reactant? Limiting/Excess Reactants Explained #27

Aluminum hydroxide reacts with sulfuric acid as follows: 
2 Al1OH231s2 + 3 H2SO41aq2¡Al21SO4231aq2 + 6 H2O1l2 
How many moles of 
Al21SO423 can form under these conditions?

Sodium hydroxide reacts with carbon dioxide as follows:
2 NaOH1s2 + CO21g2¡Na2CO31s2 + H2O1l2
How many moles of Na2CO3 can be produced?

Limiting Reagent Made Easy: Stoichiometry Tutorial Part 5

(b) Why are the amounts of products formed in a reaction
determined only by the amount of the limiting reactant?

Sodium hydroxide reacts with carbon dioxide as follows:
2 NaOH1s2 + CO21g2¡Na2CO31s2 + H2O1l2
How many moles of the excess reactant
remain after the completion of the reaction?

The reaction between solid aluminum and iron (III) chloride can generate temperatures reaching 3000 ºC and is used in welding metals.&nbsp;2 Al&nbsp;+&nbsp;Fe2O3 → Al2O­3 + 2 FeIf 150 g of Al are reacted with 432 g of Fe­2O3, what is the mass of the excess reactant remaining?&nbsp;

Consider the reaction:
2 CH3OH(g) + 3 O2( g)¡2 CO2( g) + 4 H2O(g)
Each of the molecular diagrams represents an initial mixture
of the reactants. How many CO2 molecules form from
the reaction mixture that produces the greatest amount of
products?
<img src="https://lightcat-files.s3.amazonaws.com/problem_images/6e1453f83e97d0cc-1659959846992.jpg" alt="" />

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[BOOK CHEM] Clutch Version

Empirical Formula

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.

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;