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Holt Chemistry

R.Thomas Myers, Keith Oldham,Savatore Tocci

Chapter 9

Stoichiometry - all with Video Answers

Educators

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Chapter Questions

01:27

Problem 1

Define stoichiometry.

Rithvik Manne
Rithvik Manne
Numerade Educator
01:33

Problem 2

Compare the limiting reactant and the
excess reactant for a reaction.

Matthew Lueckheide
Matthew Lueckheide
Numerade Educator
01:31

Problem 3

Compare the actual yield and the theoretical
yield from a reaction.

Rithvik Manne
Rithvik Manne
Numerade Educator
01:55

Problem 4

How is percentage yield calculated?

Matthew Lueckheide
Matthew Lueckheide
Numerade Educator
01:07

Problem 5

Why is the term limiting used to describe the
limiting reactant?

Rithvik Manne
Rithvik Manne
Numerade Educator
01:44

Problem 6

Why is it necessary to use mole ratios in
solving stoichiometry problems?

Matthew Lueckheide
Matthew Lueckheide
Numerade Educator
03:20

Problem 7

What is the key conversion factor needed
to solve all stoichiometry problems?

Pahk Thepchatri
Pahk Thepchatri
Numerade Educator
01:13

Problem 9

Why is a balanced chemical equation
needed to solve stoichiometry problems?

Rithvik Manne
Rithvik Manne
Numerade Educator
01:56

Problem 9

Use the balanced equation below to write
mole ratios for the situations that follow.
$$2 \mathrm{H}_{2}(g)+\mathrm{O}_{2}(\mathrm{g}) \rightarrow 2 \mathrm{H}_{2} \mathrm{O}(g)$$
\begin{equation}\begin{array}{l}{\text { a. calculating mol } \mathrm{H}_{2} \mathrm{O} \text { given mol } \mathrm{H}_{2}} \\ {\text { b. calculating mol } \mathrm{O}_{2} \text { given mol } \mathrm{H}_{2} \mathrm{O}} \\ {\text { c. calculating mol } \mathrm{H}_{2} \text { given mol } \mathrm{O}_{2}}\end{array}\end{equation}

Rithvik Manne
Rithvik Manne
Numerade Educator
00:45

Problem 10

Write the conversion factor needed to
convert from g $\mathrm{O}_{2}$ to $\mathrm{L} \mathrm{O}_{2}$ if the density
of $\mathrm{O}_{2}$ is 1.429 $\mathrm{g} / \mathrm{L}$ .

Matthew Lueckheide
Matthew Lueckheide
Numerade Educator
00:37

Problem 11

What conversion factor is used to convert from volume of a gas directly to moles at STP?

Rithvik Manne
Rithvik Manne
Numerade Educator
03:32

Problem 12

Describe a general plan for solving all stoichiometry problems in three steps.

Matthew Lueckheide
Matthew Lueckheide
Numerade Educator
02:40

Problem 13

Explain why cost is often a major factor in
choosing a limiting reactant.

Ronald Prasad
Ronald Prasad
Numerade Educator
02:43

Problem 14

Give two reasons why the actual yield from
chemical reactions is less than 100$\% .$

Matthew Lueckheide
Matthew Lueckheide
Numerade Educator
01:08

Problem 15

Describe the relationship between the
limiting reactant and the theoretical yield.

Rithvik Manne
Rithvik Manne
Numerade Educator
05:41

Problem 16

What are three areas of a car's operation or
design that depend on stoichiometry?

Matthew Lueckheide
Matthew Lueckheide
Numerade Educator
01:30

Problem 17

Describe what might happen if too much or too little gas generant is used in an air bag.

Rithvik Manne
Rithvik Manne
Numerade Educator
02:49

Problem 18

Why is the ratio of fuel to air in a car's engine important in controlling pollution?

Matthew Lueckheide
Matthew Lueckheide
Numerade Educator
03:32

Problem 20

Under what conditions will exhaust from a
car's engine contain high levels of carbon
monoxide?

Matthew Lueckheide
Matthew Lueckheide
Numerade Educator
01:25

Problem 21

What is the function of the catalytic converter in the exhaust system?

Rithvik Manne
Rithvik Manne
Numerade Educator
02:02

Problem 21

The chemical equation for the formation of water is
$$2 \mathrm{H}_{2}+\mathrm{O}_{2} \rightarrow 2 \mathrm{H}_{2} \mathrm{O}$$
\begin{equation}\begin{array}{l}{\text { a. If } 3.3 \mathrm{mol} \mathrm{O}_{2} \text { are used, how many moles }} \\ {\text { of } \mathrm{H}_{2} \text { are needed? }} \\ {\text { b. How many moles } \mathrm{O}_{2} \text { must react with }} \\ {\text { excess } \mathrm{H}_{2} \text { to form } 6.72 \mathrm{mol} \mathrm{H}_{2} \mathrm{O} \text { ? }} \\ {\text { c. If you wanted to make } 8.12 \mathrm{mol} \mathrm{H}_{2} \mathrm{O},} \\ {\text { how many moles of } \mathrm{H}_{2} \text { would you need? }}\end{array}\end{equation}

Rithvik Manne
Rithvik Manne
Numerade Educator
05:44

Problem 22

The reaction between hydrazine, $\mathrm{N}_{2} \mathrm{H}_{4}$ and dinitrogen tetroxide is sometimes used in rocket propulsion. Balance the equation below, then use it to answer the following
questions.
$$\mathrm{N}_{2} \mathrm{H}_{4}(l)+\mathrm{N}_{2} \mathrm{O}_{4}(l) \longrightarrow \mathrm{N}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(g)$$
\begin{equation}\begin{array}{l}{\text { a. How many moles } \mathrm{H}_{2} \mathrm{O} \text { are produced as }} \\ {1.22 \times 10^{3} \mathrm{mol} \mathrm{N}_{2} \text { are formed? }} \\ {\text { b. How many moles } \mathrm{N}_{2} \mathrm{H}_{4} \text { must react with }} \\ {1.45 \times 10^{3} \mathrm{mol} \mathrm{N}_{2} \mathrm{O}_{4} ?} \\ {\text { c. If } 2.13 \times 10^{3} \mathrm{mol} \mathrm{N}_{2} \mathrm{O}_{4} \text { completely react, }} \\ {\text { how many moles of } \mathrm{N}_{2} \text { form? }}\end{array}\end{equation}

Matthew Lueckheide
Matthew Lueckheide
Numerade Educator
02:41

Problem 23

Aluminum reacts with oxygen to form
aluminum oxide.
\begin{equation}\begin{array}{l}{\text { a. How many moles of } \mathrm{O}_{2} \text { are needed to }} \\ {\text { react with } 1.44 \text { mol of aluminum? }} \\ {\text { b. How many moles of aluminum oxide can }} \\ {\text { be made if } 5.23 \text { mol Al completely react? }}\end{array}\end{equation}

Rithvik Manne
Rithvik Manne
Numerade Educator
06:58

Problem 24

Calcium carbide, $\mathrm{CaC}_{2},$ reacts with water to
form acetylene.
$$\mathrm{CaC}_{2}(s)+2 \mathrm{H}_{2} \mathrm{O}(l) \rightarrow \mathrm{C}_{2} \mathrm{H}_{2}(g)+\mathrm{Ca}(\mathrm{OH})_{2}(s)$$
\begin{equation}\begin{array}{l}{\text { a. How many grams of water are needed to }} \\ {\text { react with } 485 \text { g of calcium carbide? }} \\ {\text { b. How many grams of } \mathrm{CaC}_{2} \text { could make }} \\ {\text { 23.6 g } \mathrm{C}_{2} \mathrm{H}_{2} \text { ? }} \\ {\text { c. If } 55.3 \mathrm{g} \mathrm{Ca}(\mathrm{OH})_{2} \text { are formed, how many }} \\ {\text { grams of water reacted? }}\end{array}\end{equation}

Matthew Lueckheide
Matthew Lueckheide
Numerade Educator
06:15

Problem 25

Oxygen can be prepared by heating potassium chlorate.
$$2 \mathrm{KClO}_{3}(s) \rightarrow 2 \mathrm{KCl}(s)+3 \mathrm{O}_{2}(g)$$
\begin{equation}\begin{array}{l}{\text { a. What mass of } \mathrm{O}_{2} \text { can be made from heat- }} \\ {\text { ing } 125 \text { g of } \mathrm{KClO}_{3} ?} \\ {\text { b. How many grams of } \mathrm{KClO}_{3} \text { are needed }} \\ {\text { to make } 293 \mathrm{g} \mathrm{g}_{2} \text { ? }} \\ {\text { c. How many grams of KCl could form from }} \\ {20.8 \mathrm{g} \mathrm{KClO}_{3} ?}\end{array}\end{equation}

Rithvik Manne
Rithvik Manne
Numerade Educator
View

Problem 26

How many grams of aluminum oxide can be
formed by the reaction of 38.8 $\mathrm{g}$ of aluminum with oxygen?

Miguel Perez
Miguel Perez
Numerade Educator
03:36

Problem 27

Use the equation provided to answer the
questions that follow. The density of oxygen
gas is 1.428 $\mathrm{g} / \mathrm{L}$ .
$$2 \mathrm{KClO}_{3}(s) \rightarrow 2 \mathrm{KCl}(s)+3 \mathrm{O}_{2}(g)$$
\begin{equation}\begin{array}{l}{\text { a. What volume of oxygen can be made }} \\ {\text { from } 5.00 \times 10^{-2} \text { mol of } \mathrm{KClO}_{3} ?} \\ {\text { b. How many grams } \mathrm{KClO}_{3} \text { must react to }} \\ {\text { form } 42.0 \mathrm{mL} \mathrm{O}_{2} \text { ? }} \\ {\text { c. How many milliliters of } \mathrm{O}_{2} \text { will form at }} \\ {\text { STP from } 55.2 \mathrm{g} \mathrm{KClO}_{3} ?}\end{array}\end{equation}

Ronald Prasad
Ronald Prasad
Numerade Educator
04:46

Problem 28

Hydrogen peroxide, $\mathrm{H}_{2} \mathrm{O}_{2},$ decomposes to
form water and oxygen.
\begin{equation}\begin{array}{l}{\text { a. How many liters of } \mathrm{O}_{2} \text { can be made }} \\ {\text { from } 342 \mathrm{g} \mathrm{H}_{2} \mathrm{O}_{2} \text { if the density of } \mathrm{O}_{2} \text { is }} \\ {1.428 \mathrm{g} / \mathrm{L} ?} \\ {\text { b. The density of } \mathrm{H}_{2} \mathrm{O}_{2} \text { is } 1.407 \mathrm{g} / \mathrm{mL}, \text { and }} \\ {\text { the density of } \mathrm{O}_{2} \text { is } 1.428 \mathrm{g} / \mathrm{L} . \text { How }} \\ {\text { many liters of } \mathrm{O}_{2} \text { can be made from }} \\ {55 \mathrm{mL} \mathrm{H}_{2} \mathrm{O}_{2} ?}\end{array}\end{equation}

Matthew Lueckheide
Matthew Lueckheide
Numerade Educator
06:07

Problem 29

Use the equation provided to answer the questions that follow.
$$2 \mathrm{NO}+\mathrm{O}_{2} \longrightarrow 2 \mathrm{NO}_{2}$$
\begin{equation}\begin{array}{l}{\text { a. How many molecules of } \mathrm{NO}_{2} \text { can form }} \\ {\text { from } 1.11 \mathrm{mol} \mathrm{O}_{2} \text { and excess } \mathrm{NO} \text { ? }} \\ {\text { b. How many molecules of NO will react }} \\ {\text { with } 25.7 \mathrm{g} \mathrm{O}_{2} ?} \\ {\text { c. How many molecules of } \mathrm{O}_{2} \text { are needed to }} \\ {\text { make } 3.76 \times 10^{22} \text { molecules } \mathrm{NO}_{2} ?}\end{array}\end{equation}

Rithvik Manne
Rithvik Manne
Numerade Educator
07:06

Problem 30

Use the equation provided to answer the questions that follow.
$$2 \mathrm{Na}+2 \mathrm{H}_{2} \mathrm{O} \longrightarrow 2 \mathrm{NaOH}+\mathrm{H}_{2}$$
\begin{equation}\begin{array}{l}{\text { a. How many molecules of } \mathrm{H}_{2} \text { could be }} \\ {\text { made from } 27.6 \mathrm{g} \mathrm{H}_{2} \mathrm{O} \text { ? }} \\ {\text { b. How many atoms of Na will completely }} \\ {\text { react with } 12.9 \mathrm{g} \mathrm{H}_{2} \mathrm{O} \text { ? }} \\ {\text { c. How many molecules of } \mathrm{H}_{2} \text { could form }} \\ {\text { when } 6.59 \times 10^{20} \text { atoms Na react? }}\end{array}\end{equation}

Matthew Lueckheide
Matthew Lueckheide
Numerade Educator
02:12

Problem 31

In the reaction shown below, 4.0 mol of NO
is reacted with 4.0 mol $\mathrm{O}_{2}$

\begin{equation}\begin{array}{l}{\text { a. Which is the excess reactant, and which is }} \\ {\text { the limiting reactant? }} \\ {\text { b. What is the theoretical yield, in units of }} \\ {\text { mol, of } \mathrm{NO}_{2} ?}\end{array}\end{equation}

David Collins
David Collins
Numerade Educator
08:26

Problem 32

In the reaction shown below, 64 $\mathrm{g} \mathrm{CaC}_{2}$ is
reacted with 64 $\mathrm{g} \mathrm{H}_{2} \mathrm{O} .$
$$\mathrm{CaC}_{2}(s)+2 \mathrm{H}_{2} \mathrm{O}(l) \rightarrow \mathrm{C}_{2} \mathrm{H}_{2}(g)+\mathrm{Ca}(\mathrm{OH})_{2}(s)$$
\begin{equation}\begin{array}{l}{\text { a. Which is the excess reactant, and which is }} \\ {\text { the limiting reactant? }} \\ {\text { b. What is the theoretical yield of } C_{2} \mathrm{H}_{2} ?} \\ {\text { c. What is the theoretical yield of } \mathrm{Ca}(\mathrm{OH})_{2} ?}\end{array}\end{equation}

Matthew Lueckheide
Matthew Lueckheide
Numerade Educator
07:28

Problem 33

In the reaction shown below, 28 g of nitrogen are reacted with 28 g of hydrogen.
\begin{equation}\begin{array}{l}{\text { a. Which is the excess reactant, and which is }} \\ {\text { the limiting reactant? }} \\ {\text { b. What is the theoretical yield of ammonia? }} \\ {\text { c. How many grams of the excess reactant }} \\ {\text { remain? }}\end{array}\end{equation}

Dr. Satish Ingale
Dr. Satish Ingale
Numerade Educator
03:57

Problem 34

Reacting 991 mol of $\mathrm{SiO}_{2}$ with excess carbon yields 30.0 $\mathrm{kg}$ of $\mathrm{SiC.}$ What is the percentage yield?
$$\mathrm{SiO}_{2}+3 \mathrm{C} \rightarrow \mathrm{SiC}+2 \mathrm{CO}$$

Matthew Lueckheide
Matthew Lueckheide
Numerade Educator
03:05

Problem 35

If 156 $\mathrm{g}$ of sodium nitrate react, and 112 $\mathrm{g}$ of
sodium nitrite are recovered, what is the percentage yield?
$$2 \mathrm{NaNO}_{3}(s) \longrightarrow 2 \mathrm{NaNO}_{2}(s)+\mathrm{O}_{2}(g)$$

Rithvik Manne
Rithvik Manne
Numerade Educator
03:00

Problem 36

If 185 g of magnesium are recovered from
the decomposition of 1000.0 g of magnesium
chloride, what is the percentage yield?

Matthew Lueckheide
Matthew Lueckheide
Numerade Educator
02:59

Problem 37

How many grams of $\mathrm{NaNO}_{2}$ form when
256 $\mathrm{g} \mathrm{NaNO}_{3}$ react? The yield is 91$\% .$
$$2 \mathrm{NaNO}_{3}(s) \longrightarrow 2 \mathrm{NaNO}_{2}(s)+\mathrm{O}_{2}(g)$$

Rithvik Manne
Rithvik Manne
Numerade Educator
03:52

Problem 38

How many grams of Al form from 9.73 g of
aluminum oxide if the yield is 91$\% ?$
$$\mathrm{Al}_{2} \mathrm{O}_{3}+3 \mathrm{C} \rightarrow 2 \mathrm{Al}+3 \mathrm{CO}$$

Matthew Lueckheide
Matthew Lueckheide
Numerade Educator
03:58

Problem 39

Iron and CO are made by heating 4.56 $\mathrm{kg}$ of
iron ore, $\mathrm{Fe}_{2} \mathrm{O}_{3},$ and carbon. The yield of
iron is 88$\% .$ How many kilograms of iron
are made?

Rithvik Manne
Rithvik Manne
Numerade Educator
02:12

Problem 40

Assume that 44.3 $\mathrm{g} \mathrm{Na}_{2} \mathrm{O}$ are formed during
the inflation of an air bag. How many liters
of $\mathrm{CO}_{2}($ density $=1.35 \mathrm{g} / \mathrm{L})$ are needed to
completely react with the $\mathrm{Na}_{2} \mathrm{O}$ ?
$$\mathrm{Na}_{2} \mathrm{O}(s)+2 \mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(g) \rightarrow 2 \mathrm{NaHCO}_{3}(s)$$

Matthew Lueckheide
Matthew Lueckheide
Numerade Educator
13:34

Problem 41

Assume that 59.5 $\mathrm{L} \mathrm{N}_{2}$ with a density of
0.92 $\mathrm{g} / \mathrm{L}$ are needed to fill an air bag.
\begin{equation}\begin{array}{l}{\text { a. What mass of } \mathrm{NaN}_{3} \text { is needed to form }} \\ {\text { this volume of nitrogen? }} \\ {\text { b. How many liters of } \mathrm{N}_{2} \text { are actually made }} \\ {\text { from 65.7 g } \mathrm{NaN}_{3} \text { if the yield is } 94 \% ?}\end{array}\end{equation}
\begin{equation}\begin{array}{l}{\text { c. What mass of } \mathrm{NaN}_{3} \text { is actually needed to }} \\ {\text { form } 59.5 \mathrm{L} \mathrm{N}_{2} \text { ? }}\end{array}\end{equation}

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
05:00

Problem 42

Write a balanced equation for the combus-
tion of octane, $\mathrm{C}_{8} \mathrm{H}_{18},$ with oxygen to obtain
carbon dioxide and water. What is the mole
ratio of oxygen to octane?

Matthew Lueckheide
Matthew Lueckheide
Numerade Educator
03:24

Problem 43

What mass of oxygen is required to burn
688 g of octane, $\mathrm{C}_{8} \mathrm{H}_{18},$ completely?

Rithvik Manne
Rithvik Manne
Numerade Educator
03:34

Problem 44

How many liters of $\mathrm{O}_{2},$ density $1.43 \mathrm{g} / \mathrm{L},$ are
needed for the complete combustion of
$1.00 \mathrm{L} \mathrm{C}_{8} \mathrm{H}_{18},$ density 0.700 $\mathrm{g} / \mathrm{mL} ?$

Matthew Lueckheide
Matthew Lueckheide
Numerade Educator
01:51

Problem 45

Nitrogen dioxide from exhaust reacts with
oxygen to form ozone. What mass of ozone
could be formed from 4.55 $\mathrm{g} \mathrm{NO}_{2} ?$ If only
4.58 $\mathrm{g} \mathrm{O}_{3}$ formed, what is the percentage
yield?
$$\mathrm{NO}_{2}(g)+\mathrm{O}_{2}(g) \rightarrow \mathrm{NO}(g)+\mathrm{O}_{3}(g)$$

Rithvik Manne
Rithvik Manne
Numerade Educator
05:54

Problem 46

How many grams $\mathrm{CO}_{2}$ form from the complete combustion of $1.00 \mathrm{L} \mathrm{C}_{8} \mathrm{H}_{18},$ density 0.700 $\mathrm{g} / \mathrm{mL} ?$ If only $1.90 \times 10^{3} \mathrm{g} \mathrm{CO}_{2}$ form, what is the percentage yield?

Matthew Lueckheide
Matthew Lueckheide
Numerade Educator
03:27

Problem 47

The following reaction can be used to
remove $\mathrm{CO}_{2}$ breathed out by astronauts in a
spacecraft.
$$2 \mathrm{LiOH}(s)+\mathrm{CO}_{2}(g) \rightarrow \mathrm{Li}_{2} \mathrm{CO}_{3}(s)+\mathrm{H}_{2} \mathrm{O}(l)$$
\begin{equation}\begin{array}{l}{\text { a. How many grams of carbon dioxide can }} \\ {\text { be removed by } 5.5 \text { mol LiOH? }} \\ {\text { b. How many milliliters } \mathrm{H}_{2} \mathrm{O} \text { (density }=} \\ {0.997 \mathrm{g} / \mathrm{mL} \text { ) could form from } 25.7 \mathrm{g} \text { LiOH? }} \\ {\text { c. How many molecules } \mathrm{H}_{2} \mathrm{O} \text { could be }} \\ {\text { made when } 3.28 \mathrm{g} \mathrm{CO}_{2} \text { react? }}\end{array}\end{equation}

Ronald Prasad
Ronald Prasad
Numerade Educator
03:10

Problem 48

How many liters $\mathrm{N}_{2},$ density $0.92 \mathrm{g} / \mathrm{L},$ can be
made by the decomposition of 2.05 $\mathrm{g} \mathrm{NaN}_{3} ?$
$$2 \mathrm{NaN}_{3}(s) \rightarrow 2 \mathrm{Na}(s)+3 \mathrm{N}_{2}(g)$$

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
03:21

Problem 49

The percentage yield of nitric acid is 95$\% .$ If
9.88 $\mathrm{kg}$ of nitrogen dioxide react, what mass
of nitric acid is isolated?
$$3 \mathrm{NO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(g) \rightarrow 2 \mathrm{HNO}_{3}(a q)+\mathrm{NO}(g)$$

Rithvik Manne
Rithvik Manne
Numerade Educator
05:11

Problem 50

If you get 25.3 milgal, what mass of carbon
dioxide is produced by the complete combus-
tion of $\mathrm{C}_{8} \mathrm{H}_{18}$ if you drive 5.40 $\mathrm{mi} ?$ (Hint:
$1 \mathrm{gal}=3.79 \mathrm{L}$ ; density of octane $=0.700 \mathrm{g} / \mathrm{mL} )$

Matthew Lueckheide
Matthew Lueckheide
Numerade Educator
02:13

Problem 51

Nitrogen monoxide, NO, reacts with oxygen
to form nitrogen dioxide. Then the nitrogen
dioxide reacts with oxygen to form nitrogen
monoxide and ozone. Write the balanced
equations. What is the theoretical yield in
grams of ozone from 4.55 g of nitrogen
monoxide with excess $\mathrm{O}_{2} ?$ (Hint: First calcu-
late the theoretical yield for NO $_{2}$ , then use
that value to calculate the yield for ozone.)

Ronald Prasad
Ronald Prasad
Numerade Educator
01:13

Problem 52

Why would it be unreasonable for an
amendment to the Clean Air Act to call for
0% pollution emissions from cars with
combustion engines?

Matthew Lueckheide
Matthew Lueckheide
Numerade Educator
02:04

Problem 53

Use stoichiometry to explain the following
problems that a lawn mower may have.
a. A lawn mower fails to start because the
engine floods.
b. A lawn mower stalls after starting cold
and idling

Rithvik Manne
Rithvik Manne
Numerade Educator
07:02

Problem 54

Design an experiment to measure the percentage yields for the reactions listed below. If your teacher approves your design, get the necessary materials, and carry out your plan.
a. $\mathrm{Zn}(s)+2 \mathrm{HCl}(a q) \rightarrow \mathrm{ZnCl}_{2}(a q)+\mathrm{H}_{2}(g)$
b. $2 \mathrm{NaHCO}_{3}(s) \longrightarrow$
$$
\mathrm{Na}_{2} \mathrm{CO}_{3}(s)+\mathrm{H}_{2} \mathrm{O}(g)+\mathrm{CO}_{2}(g)
$$
c. $\mathrm{CaCl}_{2}(a q)+\mathrm{Na}_{2} \mathrm{CO}_{3}(a q) \longrightarrow$
$$
\mathrm{CaCO}_{3}(s)+2 \mathrm{NaCl}(a q)
$$
d. $\mathrm{NaOH}(a q)+\mathrm{HCl}(a q) \longrightarrow$
$$
\mathrm{NaCl}(a q)+\mathrm{H}_{2} \mathrm{O}(l)
$$

Matthew Lueckheide
Matthew Lueckheide
Numerade Educator
03:21

Problem 55

Calculate the theoretical yield (in kg) of carbon dioxide emitted by a car in one year, assuming $1.20 \times 10^{4}$ mily, 25 milgal, and octane, $\mathrm{C}_{8} \mathrm{H}_{18},$ as the fuel, 0.700 $\mathrm{g} / \mathrm{mL}$ $(1 \mathrm{gal}=3.79 \mathrm{L})$

William Mills
William Mills
Numerade Educator
03:26

Problem 56

Use the following terms to create a concept
map: stoichiometry, excess reactant, theoretical yield, and mole ratio.

Matthew Lueckheide
Matthew Lueckheide
Numerade Educator
01:08

Problem 57

Describe the relationship between bond
length and bond energy.

Rithvik Manne
Rithvik Manne
Numerade Educator
01:16

Problem 58

Estimate the bond energy of a bond of
length 100 pm.

Matthew Lueckheide
Matthew Lueckheide
Numerade Educator
01:16

Problem 59

If the trend of the graph continues, what bond length will have an energy of $200 \mathrm{~kJ} / \mathrm{mol} ?$

Lottie Adams
Lottie Adams
Numerade Educator
01:37

Problem 60

The title of the graph does not provide much
information about the contents of the graph.
What additional information would be useful
to better understand and use this graph?

Matthew Lueckheide
Matthew Lueckheide
Numerade Educator
02:25

Problem 61

Graphing Calculator
Calculating Percentage Yield of a Chemical
Reaction
The graphing calculator can run a program
that calculates the percentage yield of a
chemical reaction when you enter the actual
yield and the theoretical yield. Using an
example in which the actual yield is 38.8 g
and the theoretical yield is 53.2 g, you will

calculate the percentage yield. First, the pro-
gram will carry out the calculation. Then

you can use it to make other calculations.
Go to Appendix C. If you are using a TI-83
Plus, you can download the program YIELD
and data and run the application as directed.

If you are using another calculator, your
teacher will provide you with keystrokes
and data sets to use. After you have run the
program, answer the questions.
Note: all answers are written with three
significant figures.
\begin{equation}\begin{array}{l}{\text { a. What is the percentage yield when the }} \\ {\text { actual yield is } 27.3 \mathrm{g} \text { and the theoretical }} \\ {\text { yield is } 44.6 \mathrm{g} \text { ? }} \\ {\text { b. What is the percentage yield when the }} \\ {\text { actual yield is } 5.40 \mathrm{g} \text { and the theoretical }} \\ {\text { c. What actual yield theoretical yield pair }} \\ {\text { produced the largest percentage yield? }}\end{array}\end{equation}

Smrithi Upadhyayula
Smrithi Upadhyayula
Numerade Educator