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Chemistry Structure and Properties

Nivaldo J. Tro

Chapter 16

Chemical Equilibrium - all with Video Answers

Educators

Chapter Questions

01:35

Problem 1

How does a developing fetus get oxygen in the womb?

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01:10

Problem 2

What is dynamic equilibrium? Why is it called dynamic?

Bailey Mccarthy Riley
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00:25

Problem 3

Give the general expression for the equilibrium constant of the follow-
ing generic reaction:
$$a A+b B \rightleftharpoons c \mathrm{C}+d \mathrm{D}$$

Ronald Prasad
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01:01

Problem 4

What is the significance of the equilibrium constant? What does a
large equilibrium constant tell us about a reaction? A small one?

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02:33

Problem 5

What happens to the value of the equilibrium constant for a reaction
if the reaction equation is reversed? Multiplied by a constant?

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01:19

Problem 6

If two reactions sum to an overall reaction, and the equilibrium constants for the two reactions are $K_{1}$ and $K_{2},$ what is the equilibrium
constant for the overall reaction?

Bailey Mccarthy Riley
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01:20

Problem 7

Explain the difference between $K_{c}$ and $K_{\mathrm{p}}$ . For a given reaction, how
are the two constants related?

Amy Jiang
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01:18

Problem 8

What units should you use when expressing concentrations or partial
pressures in the equilibrium constant? What are the units of
$K_{\mathrm{p}}$ and $K_{c}^{2}$ Explain.

Ronald Prasad
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00:48

Problem 9

Why do we omit the concentrations of solids and liquids from equilib-
rium expressions?

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01:48

Problem 10

Does the value of the equilibrium constant depend on the initial con-
centrations of the reactants and products? Do the equilibrium concen-
trations of the reactants and products depend on their initial
concentrations? Explain.

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03:03

Problem 11

Explain how you might deduce the equilibrium constant for a reaction
in which you know the initial concentrations of the reactants and
products and the equilibrium concentration of only one reactant or
product.

Amy Jiang
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01:47

Problem 12

What is the definition of the reaction quotient $(Q)$ for a reaction? What
does $Q$ measure?

Bailey Mccarthy Riley
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01:14

Problem 13

What is the value of $Q$ when each reactant and product is in its standard
state? (See Section 10.10 for the definition of standard states.)

Ronald Prasad
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00:55

Problem 14

In what direction does a reaction proceed for each condition:
$$(\mathrm{b})Q>K ; \text { and }(\mathrm{c}) Q=K ?$$

Ronald Prasad
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02:44

Problem 15

Many equilibrium calculations involve finding the equilibrium concen-
trations of reactants and products given their initial concentrations and
the equilibrium constant. Outline the general procedure used in solving
these kinds of problems.

Ronald Prasad
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03:09

Problem 16

In equilibrium problems involving equilibrium constants that are small
relative to the initial concentrations of reactants, we can often assume
that the quantity $x$ (which represents how far the reaction proceeds to-.ward products) is small. When this assumption is made, we can ignore
the quantity $x$ when it is subtracted from a large number but not when it
is multiplied by a large number. In other words, $2.5-x \approx 2.5,$ but
$2.5 x \neq 2.5 .$ Explain why we can ignore a small $x$ in the first case but not
in the second.

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01:10

Problem 17

What happens to a chemical system at equilibrium when equilibrium is
disturbed?

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01:01

Problem 18

What is the effect of a change in concentration of a reactant or product
on a chemical reaction initially at equilibrium?

Bailey Mccarthy Riley
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03:03

Problem 19

What is the effect of a change in volume on a chemical reaction (that in-
cludes gaseous reactants or products) initially at equilibrium?

Ronald Prasad
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02:33

Problem 20

What is the effect of a temperature change on a chemical reaction ini-
tially at equilibrium? How does the effect differ for an exothermic reac-
tion compared to an endothermic one?

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01:23

Problem 21

Write an expression for the equilibrium constant of each chemical
equation.
\begin{equation}
\begin{array}{l}{\text { a. } \operatorname{SbCl}_{5}(g) \Longrightarrow \operatorname{SbCl}_{3}(g)+\mathrm{Cl}_{2}(g)} \\ {\text { b. } 2 \mathrm{BrNO}(g) \rightleftharpoons 2 \mathrm{NO}(g)+\mathrm{Br}_{2}(g)}
\end{array}\end{equation}
\begin{equation}
\begin{array}{l}{\text { c. } \operatorname{CH}_{4}(g) \Longrightarrow \operatorname2 \mathrm{H}_{2} \mathrm{S}(g)+\mathrm{CS}_{2}(g)} \\ {\text { d. } 2 \mathrm{CO}(g) \rightleftharpoons \mathrm{O}_{2}(g)+\mathrm2 \mathrm{CO}_{2}(g)}
\end{array}\end{equation}

Ronald Prasad
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00:53

Problem 22

Find and fix each mistake in the equilibrium constant expressions.
\begin{equation}a.\quad2 \mathrm{H}_{2} \mathrm{S}(g) \rightleftharpoons 2 \mathrm{H}_{2}(g)+\mathrm{S}_{2}(g) K_{c}=\frac{\left[\mathrm{H}_{2}\right]\left[\mathrm{S}_{2}\right]}{\left[\mathrm{H}_{2} \mathrm{S}\right]}\end{equation}
\begin{equation}b.\quad \mathrm{CO} \mathrm{}(g) \rightleftharpoons C \mathrm{L}_{2}(g)+\mathrm{COCI}_{2}(g) K_{e}=\frac{\left[\mathrm{CO}_{2}\right]\left[\mathrm{C1}_{2}\right]}{\left[\mathrm{COC1}_{2} \mathrm{}\right]}\end{equation}

Ronald Prasad
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01:19

Problem 23

When this reaction comes to equilibrium, will the concentrations
reactants or products be greater? Does the answer to this question
pend on the initial concentrations of the reactants and products?
\begin{equation}\mathrm{A}(g)+\mathrm{B}(g) \rightleftharpoons 2 \mathrm{C}(g) \quad K_{\mathrm{c}}=1.4 \times 10^{-5}\end{equation}

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02:35

Problem 24

Ethene $\left(\mathrm{C}_{2} \mathrm{H}_{4}\right)$ can be halogenated by this reaction:
\begin{equation}\mathrm{C}_{2} \mathrm{H}_{4}(g)+\mathrm{X}_{2}(g) \Longrightarrow \mathrm{C}_{2} \mathrm{H}_{4} \mathrm{X}_{2}(g)\end{equation}
where $\mathrm{X}_{2}$ can be $\mathrm{Cl}_{2}($ green $), \mathrm{Br}_{2}$ (brown), or $\mathrm{I}_{2}$ (purple). Examine the
three figures representing equilibrium concentrations in this reaction at
the same temperature for the three different halogens. Rank the equilib-
rium constants for the three reactions from largest to smallest.

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03:04

Problem 25

$\mathrm{H}_{2}$ and $\mathrm{I}_{2}$ are combined in a flask and allowed to react according to
the reaction:
$$\mathrm{H}_{2}(g)+\mathrm{I}_{2}(g) \rightleftharpoons 2 \mathrm{Hl}(g)$$
Examine the figures (sequential in time) and answer the questions:
\begin{equation}\begin{array}{l}{\text { a. Which figure represents the point at which equilibrium is reached? }} \\ {\text { b. How would the series of figures change in the presence of a catalyst? }} \\ {\text { c. Would there be different amounts of reactants and products in the }} \\ {\text { final figure (vi) in the presence of a catalyst? }}\end{array}\end{equation}

Ronald Prasad
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01:31

Problem 26

A chemist trying to synthesize a particular compound attempts two dif-
ferent synthesis reactions. The equilibrium constants for the two reac-
tions are 23.3 and $2.2 \times 10^{4}$ at room temperature. However, upon
carrying out both realtions for 15 minutes, the chemist finds that the re-
action with the smaller equilibrium constant produces more of the de-
sired product. Explain how this might be possible.

Bailey Mccarthy Riley
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03:43

Problem 27

This reaction has an equilibrium constant of $K_{\mathrm{p}}=2.26 \times 10^{4}$ at 298 $\mathrm{K}$
\begin{equation}\mathrm{CO}(g)+2 \mathrm{H}_{2}(g) \rightleftharpoons \mathrm{CH}_{3} \mathrm{OH}(g)\end{equation}
Calculate $K_{\mathrm{p}}$ for each reaction and predict whether reactants or products
will be favored at equilibrium.
\begin{equation}\begin{array}{l}{\text { a. } \mathrm{CH}_{3} \mathrm{OH}(g) \rightleftharpoons \mathrm{CO}(g)+2 \mathrm{H}_{2}(g)} \\ {\text { b. } \frac{1}{2} \mathrm{CO}(g)+\mathrm{H}_{2}(g) \rightleftharpoons \frac{1}{2} \mathrm{CH}_{3} \mathrm{OH}(g)} \\ {\text { c. } 2 \mathrm{CH}_{3} \mathrm{OH}(g) \rightleftharpoons 2 \mathrm{CO}(g)+4 \mathrm{H}_{2}(g)}\end{array}\end{equation}

Amy Jiang
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01:41

Problem 28

This reaction has an equilibrium constant of $K_{\mathrm{p}}=2.2 \times 10^{6}$ at 298 $\mathrm{K}$
\begin{equation}2 \mathrm{COF}_{2}(g) \rightleftharpoons \mathrm{CO}_{2}(g)+\mathrm{CF}_{4}(g)\end{equation}
Calculate $K_{\mathrm{p}}$ for each reaction and predict whether reactants or products
will be favored at equilibrium.
\begin{equation}\begin{array}{l}{\text { a. } \operatorname{COF}_{2}(g) \rightleftharpoons \frac{1}{2} \mathrm{CO}_{2}(g)+\frac{1}{2} \mathrm{CF}_{4}(g)} \\ {\text { b. } 6 \mathrm{COF}_{2}(g) \rightleftharpoons 3 \mathrm{CO}_{2}(g)+3 \mathrm{CF}_{4}(g)} \\ {\text { c. } 2 \mathrm{CO}_{2}(g)+2 \mathrm{CF}_{4}(g) \rightleftharpoons 4 \mathrm{COF}_{2}(g)}\end{array}\end{equation}

Ronald Prasad
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02:05

Problem 29

Consider the reactions and their respective equilibrium constants.
\begin{equation}\mathrm{NO}(g)+\frac{1}{2} \mathrm{Br}_{2}(g) \rightleftharpoons \operatorname{NOBr}(g) \quad K_{p}=5.3\end{equation}
\begin{equation}
2 \mathrm{NO}(g) \rightleftharpoons \mathrm{N}_{2}(g)+\mathrm{O}_{2}(g) \quad \quad K_{\mathrm{p}}=2.1 \times 10^{30}\end{equation}
Use these reactions and their equilibrium constants to predict the equi-
librium constant for the following reaction:
\begin{equation}\mathrm{N}_{2}(g)+\mathrm{O}_{2}(g)+\mathrm{Br}_{2}(g) \rightleftharpoons 2 \mathrm{NOBr}(g)\end{equation}

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Problem 30

Use the following reactions and their equilibrium constants to predict
the equilibrium constant for this reaction: 2 $\mathrm{A}(s) \rightleftharpoons 3 \mathrm{D}(g)$
\begin{equation}\mathrm{A}(s) \rightleftharpoons \frac{1}{2} \mathrm{B}(g)+\mathrm{C}(g) \quad K_{1}=0.0334\end{equation}
\begin{equation}3 \mathrm{D}(g) \rightleftharpoons \mathrm{B}(g)+2 \mathrm{C}(g) \quad K_{2}=2.35\end{equation}

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02:21

Problem 31

Calculate $K_{\mathrm{p}}$ for each reaction.
\begin{equation}\begin{array}{l}{\text { a. } \mathrm{I}_{2}(g) \rightleftharpoons 2 \mathrm{I}(g) \quad K_{\mathrm{p}}=6.26 \times 10^{-22}(\mathrm{at} 298 \mathrm{K})} \\ {\text { b. } \mathrm{CH}_{4}(g)+\mathrm{H}_{2} \mathrm{O}(g) \stackrel{\mathrm{K}_{\mathrm{p}}}{\rightleftharpoons} \mathrm{CO}(g)+3 \mathrm{H}_{2}(g)}\quad K_{\mathrm{p}}=7.7 \times 10^{24}(at\ 298 \mathrm{K})\end{array}\end{equation}
\begin{equation}\mathrm {c.}{N}_{2}(g)+\mathrm{O}_{2}(g) \rightleftharpoons 2 \mathrm{NO}(g) \quad K_{c}=4.10 \times 10^{-31}(\mathrm{at} 298 \mathrm{K})\end{equation}

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02:15

Problem 32

Calculate $K_{\mathrm{c}}$ for each reaction.
\begin{equation}\begin{array}{l}{\text { a. } \mathrm{N}_{2} \mathrm{O}_{4}(g) \rightleftharpoons 2 \mathrm{NO}_{2}(g) \quad K_{c}=5.9 \times 10^{-3}(\mathrm{at} 298 \mathrm{K})} \\ {\text { b. } \mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \rightleftharpoons 2 \mathrm{NH}_{3}(g) \quad K_{\mathrm{c}}=3.7 \times 10^{8}(\mathrm{at} 298 \mathrm{K})} \\ {\text { c. } \mathrm{N}_{2}(g)+\mathrm{O}_{2}(g) \rightleftharpoons 2 \mathrm{NO}(g) \quad K_{\mathrm{c}}=4.10 \times 10^{-31}(\mathrm{at} 298 \mathrm{K})}\end{array}\end{equation}

Ronald Prasad
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00:59

Problem 33

Write an equilibrium expression for each chemical equation involving
one or more solid or liquid reactants or products.
\begin{equation}
\begin{array}{l}{\text { a. } \mathrm{CO}_{3}^{2-}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{HCO}_{3}^{-}(a q)+\mathrm{OH}^{-}(a q)} \\ {\text { b. } 2 \mathrm{KClO}_{3}(s) \rightleftharpoons 2 \mathrm{KCl}(s)+3 \mathrm{O}_{2}(g)}\end{array}
\end{equation}\begin{equation}\begin{array}{l}{\text { c. } \mathrm{HF}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{H}_{3} \mathrm{O}^{+}(a q)+\mathrm{F}^{-}(a q)} \\ {\text { d. } \mathrm{NH}_{3}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{NH}_{4}^{+}(a q)+\mathrm{OH}^{-}(a q)}\end{array}\end{equation}

Ronald Prasad
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00:52

Problem 34

Find and fix the mistake in the equilibrium expression.
\begin{equation}\mathrm{PCl}_{5}(g) \rightleftharpoons \mathrm{PCl}_{3}(l)+\mathrm{Cl}_{2}(g)\end{equation}
\begin{equation}
K_{\mathrm{c}}=\frac{\left[\mathrm{PCl}_{3}\right]\left[\mathrm{Cl}_{2}\right]}{\left[\mathrm{PCl}_{5}\right]}
\end{equation}

Ronald Prasad
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00:46

Problem 35

Consider the reaction:
\begin{equation}\mathrm{CO}(g)+2 \mathrm{H}_{2}(g) \rightleftharpoons \mathrm{CH}_{3} \mathrm{OH}(g)\end{equation}
An equilibrium mixture of this reaction at a certain temperature has
$[\mathrm{CO}]=0.105 \mathrm{M},\left[\mathrm{H}_{2}\right]=0.114 \mathrm{M},$ and $\left[\mathrm{CH}_{3} \mathrm{OH}\right]=0.185 \mathrm{M} .$
What is the value of the equilibrium constant $\left(K_{\mathrm{c}}\right)$ at this temperature?

Ronald Prasad
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01:23

Problem 36

Consider the reaction:
\begin{equation}\mathrm{NH}_{4} \mathrm{HS}(s) \rightleftharpoons \mathrm{NH}_{3}(g)+\mathrm{H}_{2} \mathrm{S}(g)\end{equation}
An equilibrium mixture of this reaction at a certain temperature has
$\left[\mathrm{NH}_{3}\right]=0.278 \mathrm{M}$ and $\left[\mathrm{H}_{2} \mathrm{S}\right]=0.355 \mathrm{M} .$ What is the value of the
equilibrium constant $\left(K_{\mathrm{c}}\right)$ at this temperature?

Bailey Mccarthy Riley
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05:07

Problem 37

Consider the reaction:
\begin{equation}\mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \rightleftharpoons 2 \mathrm{NH}_{3}(g)\end{equation}
Complete the table. Assume that all concentrations are equilibrium
concentrations in $\mathrm{M} .$

Amy Jiang
Amy Jiang
Numerade Educator
04:18

Problem 38

Consider the reaction:
\begin{equation}\mathrm{H}_{2}(g)+\mathrm{I}_{2}(g) \rightleftharpoons 2 \mathrm{HI}(g)\end{equation}
Complete the table. Assume that all concentrations are equilibrium
concentrations in $\mathrm{M} .$

Bailey Mccarthy Riley
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01:05

Problem 39

Consider the reaction:
\begin{equation}2 \mathrm{NO}(g)+\mathrm{Br}_{2}(g) \Longrightarrow 2 \operatorname{NOBr}(g) \atop K_{\mathrm{p}}=28.4 \mathrm{at} 298 \mathrm{K}\end{equation}
In a reaction mixture at equilibrium, the partial pressure of NO is 108
torr and that of $\mathrm{Br}_{2}$ is 126 torr. What is the partial pressure of NOBr
in this mixture?

Ronald Prasad
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01:46

Problem 40

Consider the reaction:
\begin{equation}\begin{aligned} \mathrm{SO}_{2} \mathrm{Cl}_{2}(g) \Longrightarrow & \mathrm{SO}_{2}(g)+\mathrm{Cl}_{2}(g) \\ & K_{\mathrm{p}}=2.91 \times 10^{3} \mathrm{at} 298 \mathrm{K} \end{aligned}\end{equation}
In a reaction at equilibrium, the partial pressure of $\mathrm{SO}_{2}$ is 137 torr and
that of $\mathrm{Cl}_{2}$ is 285 torr. What is the partial pressure of $\mathrm{SO}_{2} \mathrm{Cl}_{2}$ in thismixture?

Ronald Prasad
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01:17

Problem 41

For the reaction $\mathrm{A}(g) \rightleftharpoons 2 \mathrm{B}(g),$ a reaction vessel initially containsonly $\mathrm{A}$ at a pressure of $P_{\mathrm{A}}=1.32$ atm. At equilibrium,
$P_{\mathrm{A}}=0.25$ atm. Calculate the value of $K_{\mathrm{P}}$ . (Assume no changes in
volume or temperature.)

Ronald Prasad
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02:25

Problem 42

For the reaction $2 \mathrm{A}(g) \rightleftharpoons \mathrm{B}(g)+2 \mathrm{C}(g),$ a reaction vessel initially
contains only $\mathrm{A}$ at a pressure of $P_{\mathrm{A}}=225 \mathrm{mm} \mathrm{Hg} .$ At equilibrium,$P_{\mathrm{A}}=55 \mathrm{mmHg}$ . Calculate the value of $K_{\mathrm{P}}$ . (Assume no changes in vol-
ume or temperature.)

Ronald Prasad
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02:35

Problem 43

Consider the reaction:
$$\mathrm{Fe}^{3+}(a q)+\mathrm{SCN}^{-}(a q) \rightleftharpoons \mathrm{FeSCN}^{2+}(a q)$$
A solution is made containing an initial $\left[\mathrm{Fe}^{3+}\right]$ of $1.0 \times 10^{-3} \mathrm{M}$ and an
initial $\left[\mathrm{SCN}^{-}\right]$ of $8.0 \times 10^{-4} \mathrm{M}$ . At equilibrium, $\left[\mathrm{FeSCN}^{2+}\right]=$
$1.7 \times 10^{-4} \mathrm{M} .$ Calculate the value of the equilibrium constant $\left(K_{\mathrm{c}}\right)$

Amy Jiang
Amy Jiang
Numerade Educator
02:22

Problem 44

Consider the reaction:
$$\mathrm{SO}_{2} \mathrm{Cl}_{2}(g) \rightleftharpoons \mathrm{SO}_{2}(g)+\mathrm{Cl}_{2}(g)$$
A reaction mixture is made containing an initial $\mathrm{SO}_{2} \mathrm{Cl}_{2} ]$ of 0.020 $\mathrm{M}$ .
At equilibrium, $\left[\mathrm{Cl}_{2}\right]=1.2 \times 10^{-2} \mathrm{M} .$ Calculate the value of the equilibrium constant $\left(K_{\mathrm{c}}\right)$ .

Bailey Mccarthy Riley
Bailey Mccarthy Riley
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04:06

Problem 45

Consider the reaction:
$$\mathrm{H}_{2}(g) \rightleftharpoons \mathrm{I}_{2}(g)+2 \mathrm{HI}(g)$$
A reaction mixture in a 3.67 $\mathrm{L}$ flask at a certain temperature initially
contains 0.763 $\mathrm{g} \mathrm{H}_{2}$ and 96.9 $\mathrm{g} \mathrm{I}_{2}$ . At equilibrium, the flask contains
90.4 $\mathrm{g}$ HI. Calculate the equilibrium constant $\left(K_{c}\right)$ for the reaction at this
temperature.

Ronald Prasad
Ronald Prasad
Numerade Educator
03:39

Problem 46

Consider the reaction:
$$\mathrm{CO}(g)+2 \mathrm{H}_{2}(g) \rightleftharpoons \mathrm{CH}_{3} \mathrm{OH}(g)$$
A reaction mixture in a 5.19 $\mathrm{L}$ flask at a certain temperature contains
26.9 $\mathrm{g} \mathrm{CO}$ and 2.34 $\mathrm{g} \mathrm{H}_{2} .$ At equilibrium, the flask contains 8.65 $\mathrm{g}$
$\mathrm{CH}_{3} \mathrm{OH}$ . Calculate the equilibrium constant $\left(K_{\mathrm{c}}\right)$ for the reaction at this
temperature.

Ronald Prasad
Ronald Prasad
Numerade Educator
01:15

Problem 47

Consider the reaction:
$$\mathrm{NH}_{4} \mathrm{HS}(s) \Longrightarrow \mathrm{NH}_{3}(g)+\mathrm{H}_{2} \mathrm{S}(g)$$
At a certain temperature, $K_{\mathrm{c}}=8.5 \times 10^{-3} .$ A reaction mixture at this
temperature containing solid $\mathrm{NH}_{4} \mathrm{HS}$ has $\left[\mathrm{NH}_{3}\right]=0.166 \mathrm{M}$ and
$\left[\mathrm{H}_{2} \mathrm{S}\right]=0.166 \mathrm{M} .$ Will more of the solid form, or will some of the existing solid decompose as equilibrium is reached?

Ronald Prasad
Ronald Prasad
Numerade Educator
01:12

Problem 48

Consider the reaction:
$$\begin{array}{c}{2 \mathrm{H}_{2} \mathrm{S}(g) \Longrightarrow 2 \mathrm{H}_{2}(g)+\mathrm{S}_{2}(g)} \\ {K_{\mathrm{p}}=2.4 \times 10^{-4} \mathrm{at} 1073 \mathrm{K}}\end{array}$$
A reaction mixture contains 0.112 atm of $\mathrm{H}_{2}, 0.055$ atm of $\mathrm{S}_{2},$ and 0.445
atm of $\mathrm{H}_{2} \mathrm{S} .$ Is the reaction mixture at equilibrium? If not, in what direction will the reaction proceed?

Ronald Prasad
Ronald Prasad
Numerade Educator
05:52

Problem 49

Silver sulfate dissolves in water according to the reaction:$$\begin{aligned} \mathrm{Ag}_{2} \mathrm{SO}_{4}(s) \rightleftharpoons 2 \mathrm{Ag}^{+}(a q)+\mathrm{SO}_{4}^{2-}(a q) & \\ K_{\mathrm{c}}=& 1.1 \times 10^{-5} \mathrm{at} 298 \mathrm{K} \end{aligned}$$
A 1.5 $\mathrm{L}$ solution contains 6.55 $\mathrm{g}$ of dissolved silver sulfate. If additional
solid silver sulfate is added to the solution, will it dissolve?

Amy Jiang
Amy Jiang
Numerade Educator
02:10

Problem 50

Nitrogen dioxide reacts with itself according to the reaction:
\begin{equation}2 \mathrm{NO}_{2}(g) \Longrightarrow \mathrm{N}_{2} \mathrm{O}_{4}(g)\end{equation}
\begin{equation}K_{\mathrm{p}}=6.7 \text { at } 298 \mathrm{K}\end{equation}
A 2.25 $\mathrm{L}$ container contains 0.055 $\mathrm{mol}$ of $\mathrm{NO}_{2}$ and 0.082 $\mathrm{mol}$ of $\mathrm{N}_{2} \mathrm{O}_{4}$
at 298 $\mathrm{K}$ . Is the reaction at equilibrium? If not, in what direction will the
reaction proceed?

Ronald Prasad
Ronald Prasad
Numerade Educator
03:37

Problem 51

Consider the reaction and the associated equilibrium constant:
$$a \mathrm{A}(g) \rightleftharpoons b \mathrm{B}(g) \quad K_{\mathrm{c}}=4.0$$
Find the equilibrium concentrations of $\mathrm{A}$ and $\mathrm{B}$ for each value of $a$
and $b$ . Assume that the initial concentration of $\mathrm{A}$ in each case is 1.0 $\mathrm{M}$
and that no $\mathrm{B}$ is present at the beginning of the reaction.
\begin{equation}\begin{array}{l}{\text { a. } a=1 ; b=1} \\ {\text { b. } a=2 ; b=2} \\ {\text { c. } a=1 ; b=2}\end{array}\end{equation}

Ronald Prasad
Ronald Prasad
Numerade Educator
06:15

Problem 52

Consider the reaction and the associated equilibrium constant:
$$a \mathrm{A}(g)+b \mathrm{B}(g) \rightleftharpoons c \mathrm{C}(g) \quad K_{\mathrm{c}}=5.0$$
Find the equilibrium concentrations of $\mathrm{A}, \mathrm{B},$ and $\mathrm{C}$ for each value of $a$
$b,$ and $c$ . Assume that the initial concentrations of $\mathrm{A}$ and $\mathrm{B}$ are each
1.0 $\mathrm{M}$ and that no product is present at the beginning of the reaction.
\begin{equation}
\begin{array}{l}{\text { a. } a=1 ; b=1 ; c=2} \\ {\text { b. } a=1 ; b=1 ; c=1} \\ {\text { c. } a=2 ; b=1 ; c=1 \text { (set up equation for } x ; \text { don't solve) }}\end{array}
\end{equation}

Ronald Prasad
Ronald Prasad
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02:29

Problem 53

For the reaction $K=0.513$ at 500 $\mathrm{K}$
$$\mathrm{N}_{2} \mathrm{O}_{4}(g) \rightleftharpoons 2 \mathrm{NO}_{2}(g)$$
If a reaction vessel initially contains an $\mathrm{N}_{2} \mathrm{O}_{4}$ concentration of 0.0500
$\mathrm{M}$ at $500 \mathrm{K},$ what are the equilibrium concentrations of $\mathrm{N}_{2} \mathrm{O}_{4}$ and
$\mathrm{NO}_{2}$ at 500 $\mathrm{K}$ ?

Ronald Prasad
Ronald Prasad
Numerade Educator
03:01

Problem 54

For the reaction, $K_{c}=255$ at 1000 $\mathrm{K}$ .
$$\mathrm{CO}(g)+\mathrm{Cl}_{2}(g) \rightleftharpoons \mathrm{COCl}_{2}(g)$$If a reaction mixture initially contains a CO concentration of 0.1500
$\mathrm{M}$ and a $\mathrm{Cl}_{2}$ concentration of 0.175 $\mathrm{M}$ at $1000 \mathrm{K},$ what are the equi-
librium concentrations of $\mathrm{CO}, \mathrm{Cl}_{2},$ and $\mathrm{COCl}_{2}$ at 1000 $\mathrm{K}$ ?

Ronald Prasad
Ronald Prasad
Numerade Educator
03:08

Problem 55

Consider the reaction:.$$\mathrm{NiO}(s)+\mathrm{CO}(g) \rightleftharpoons \mathrm{Ni}(s)+\mathrm{CO}_{2}(g) \quad K_{\mathrm{c}}=4.0 \times 10^{3} \text { at } 1500 \mathrm{K}$$
If a mixture of solid nickel (II) oxide and 0.20 M carbon monoxide
comes to equilibrium at 1500 $\mathrm{K}$ , what is the equilibrium concentration
of $\mathrm{CO}_{2} ?$

Amy Jiang
Amy Jiang
Numerade Educator
02:14

Problem 56

Consider the reaction:
$$\mathrm{CO}(g)+\mathrm{H}_{2} \mathrm{O}(g) \rightleftharpoons \mathrm{CO}_{2}(g)+\mathrm{H}_{2}(g) \quad K_{\mathrm{c}}=102 \text { at } 500 \mathrm{K}$$
If a reaction mixture initially contains 0.110 $\mathrm{M} \mathrm{CO}$ and 0.110 $\mathrm{M}$
$\mathrm{H}_{2} \mathrm{O},$ what is the equilibrium concentration of each of the reactants
and products?

Ronald Prasad
Ronald Prasad
Numerade Educator
02:58

Problem 57

Consider the reaction:
$$\begin{array}{c}{\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \Longrightarrow \mathrm{H}_{3} \mathrm{O}^{+}(a q)+\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}^{-}(a q)} \\ {K_{\mathrm{c}}=1.8 \times 10^{-5} \mathrm{at} 25^{\circ} \mathrm{C}}\end{array}$$
If a solution initially contains $0.210 \mathrm{M} \mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2},$ what is the equi-
librium concentration of $\mathrm{H}_{3} \mathrm{O}^{+}$ at $25^{\circ} \mathrm{C}$ ?

Ronald Prasad
Ronald Prasad
Numerade Educator
03:43

Problem 58

Consider the reaction:
$$\mathrm{SO}_{2} \mathrm{Cl}_{2}(g) \rightleftharpoons \mathrm{SO}_{2}(g)+\mathrm{Cl}_{2}(g) \quad K_{\mathrm{c}}=2.99 \times 10^{-7} \text { at } 227^{\circ} \mathrm{C}$$
If a reaction mixture initially contains $0.175 \mathrm{M} \mathrm{SO}_{2} \mathrm{Cl}_{2},$ what is the
equilibrium concentration of $\mathrm{Cl}_{2}$ at $227^{\circ} \mathrm{C}$ ?

Bailey Mccarthy Riley
Bailey Mccarthy Riley
Numerade Educator
04:58

Problem 59

Consider the reaction:
$$\mathrm{Br}_{2}(g)+\mathrm{Cl}_{2}(g) \rightleftharpoons 2 \mathrm{BrCl}(g) \quad K_{\mathrm{P}}=1.11 \times 10^{-4} \mathrm{at} 150 \mathrm{K}$$
A reaction mixture initially contains a Br_ partial pressure of 755 torr
and a $\mathrm{Cl}_{2}$ partial pressure of 735 torr at 150 $\mathrm{K}$ . Calculate the equilibrium
partial pressure of BrCl.

Ronald Prasad
Ronald Prasad
Numerade Educator
03:39

Problem 60

Consider the reaction:
$$\mathrm{CO}(g)+\mathrm{H}_{2} \mathrm{O}(g) \Longrightarrow \mathrm{CO}_{2}(g)+\mathrm{H}_{2}(g) \quad K_{\mathrm{p}}=0.0611\ at \ 2000 \mathrm{K}$$
A reaction mixture initially contains a CO partial pressure of 1344 torr
and a $\mathrm{H}_{2} \mathrm{O}$ partial pressure of 1766 torr at 2000 $\mathrm{K}$ . Calculate the equilib-
rium partial pressures of each of the products.

Ronald Prasad
Ronald Prasad
Numerade Educator
05:15

Problem 61

Consider the reaction:
$$\mathrm{A}(g) \rightleftharpoons \mathrm{B}(g)+\mathrm{C}(g)$$
Find the equilibrium concentrations of $\mathrm{A}, \mathrm{B},$ and $\mathrm{C}$ for each value of $K_{\mathrm{cr}}$
Assume that the initial concentration of $\mathrm{A}$ in each case is 1.0 $\mathrm{M}$ and that
the reaction mixture initially contains no products. Make any appropriate
simplifying assumptions.
$\begin{equation}\begin{array}{l}{\text { a. } K_{\mathrm{c}}=1.0} \\ {\text { b. } K_{\mathrm{c}}=0.0010} \\ {\text { c. } K_{\mathrm{c}}=1.0 \times 10^{-5}}\end{array}\end{equation}$

Ronald Prasad
Ronald Prasad
Numerade Educator
04:45

Problem 62

Consider the reaction:
$$
\mathrm{A}(g) \rightleftharpoons 2 \mathrm{~B}(g)
$$
Find the equilibrium partial pressures of $\mathrm{A}$ and $\mathrm{B}$ for each value $\operatorname{of} K$ Assume that the initial partial pressure of $\mathrm{B}$ in each case is $1.0 \mathrm{~atm}$ and that the initial partial pressure of $\mathrm{A}$ is 0.0 atm. Make any appropriate simplifying assumptions.
a. $K_{c}=1.0$
b. $K_{c}=1.0 \times 10^{-4}$
c. $K_{c}=1.0 \times 10^{5}$

Ronald Prasad
Ronald Prasad
Numerade Educator
00:51

Problem 63

Consider this reaction at equilibrium:
$$\operatorname{CO}(g)+\mathrm{Cl}_{2}(g) \rightleftharpoons \operatorname{COCl}_{2}(g)$$
Predict whether the reaction will shift left, shift right, or remain un-
changed after each disturbance:
\begin{equation}\begin{array}{l}{\text { a. } \mathrm{COCl}_{2} \text { is added to the reaction mixture. }} \\ {\text { b. } \mathrm{Cl}_{2} \text { is added to the reaction mixture. }} \\ {\text { c. } \mathrm{COCl}_{2} \text { is removed from the reaction mixture. }}\end{array}\end{equation}

Ronald Prasad
Ronald Prasad
Numerade Educator
00:52

Problem 64

Consider this reaction at equilibrium:
$$2 \mathrm{BrNO}(g) \rightleftharpoons 2 \mathrm{NO}(g)+\mathrm{Br}_{2}(g)$$
Predict whether the reaction will shift left, shift right, or remain un-
changed after each disturbance.
\begin{equation}\begin{array}{l}{\text { a. } \mathrm{NO} \text { is added to the reaction mixture. }} \\ {\text { b. BrNO is added to the reaction mixture. }} \\ {\text { c. } \mathrm{Br}_{2} \text { is removed from the reaction mixture. }}\end{array}\end{equation}

Ronald Prasad
Ronald Prasad
Numerade Educator
01:05

Problem 65

Consider this reaction at equilibrium:
$$2 \mathrm{KClO}_{3}(s) \rightleftharpoons 2 \mathrm{KCl}(s)+3 \mathrm{O}_{2}(g)$$
Predict whether the reaction will shift left, shift right, or remain
unchanged after each disturbance.
\begin{equation}\begin{array}{l}{\text { a. } \mathrm{O}_{2} \text { is removed from the reaction mixture. }} \\ {\text { b. } \mathrm{KCl} \text { is added to the reaction mixture. }} \\ {\text { c. } \mathrm{KClO}_{3} \text { is added to the reaction mixture. }} \\ {\text { d. } \mathrm{O}_{2} \text { is added to the reaction mixture. }}\end{array}\end{equation}

Ronald Prasad
Ronald Prasad
Numerade Educator
00:58

Problem 66

Consider this reaction at equilibrium:
$$\mathrm{C}(s)+\mathrm{H}_{2} \mathrm{O}(g) \rightleftharpoons \mathrm{CO}(g)+\mathrm{H}_{2}(g)$$
Predict whether the reaction will shift left, shift right, or remain un-
changed after each disturbance.
\begin{equation}\begin{array}{l}{\text { a. } C \text { is added to the reaction mixture. }} \\ {\text { b. } \mathrm{H}_{2} \mathrm{O} \text { is condensed and removed from the reaction mixture. }} \\ {\text { c. } \mathrm{CO} \text { is added to the reaction mixture. }} \\ {\text { d. } \mathrm{H}_{2} \text { is removed trom the reaction mixture. }}\end{array}\end{equation}

Ronald Prasad
Ronald Prasad
Numerade Educator
01:47

Problem 67

Each reaction is allowed to come to equilibrium, and then the volume
is changed as indicated. Predict the effect (shift right, shift left, or no
effect) of the indicated volume change.
\begin{equation}\begin{array}{l}{\text { a. } \mathrm{I}_{2}(g) \rightleftharpoons 2 \mathrm{I}(g)(\text { volume is increased) }} \\ {\text { b. } 2 \mathrm{H}_{2} \mathrm{S}(g) \rightleftharpoons 2 \mathrm{H}_{2}(g)+\mathrm{S}_{2}(g)(\text { volume is decreased) }} \\ {\text { c. } \mathrm{I}_{2}(g)+\mathrm{Cl}_{2}(g) \rightleftharpoons 2 \mathrm{ICl}(g) \text { (volume is decreased) }}\end{array}\end{equation}

Amy Jiang
Amy Jiang
Numerade Educator
02:38

Problem 68

Each reaction is allowed to come to equilibrium, and then the volume
is changed as indicated. Predict the effect (shift right, shift left, or no
effect) of the indicated volume change.
\begin{equation}\begin{array}{l}{\text { a. } \mathrm{CO}(g)+\mathrm{H}_{2} \mathrm{O}(g) \rightleftharpoons \mathrm{CO}_{2}(g)+\mathrm{H}_{2}(g) \text { (volume is decreased) }} \\ {\text { b. } \mathrm{PCl}_{3}(g)+\mathrm{Cl}_{2}(g) \rightleftharpoons \mathrm{PCl}_{5}(g)(\text { volume is increased) }} \\ {\text { c. } \mathrm{CaCO}_{3}(s) \rightleftharpoons \mathrm{CaO}(s)+\mathrm{CO}_{2}(g)(\text { volume is increased) }}\end{array}\end{equation}

Bailey Mccarthy Riley
Bailey Mccarthy Riley
Numerade Educator
02:06

Problem 69

This reaction is endothermic.
$$\mathrm{C}(s)+\mathrm{CO}_{2}(g) \rightleftharpoons 2 \mathrm{CO}(g)$$
Predict the effect (shift right, shift left, or no effect) of increasing and
decreasing the reaction temperature. How does the value of the equilibrium constant depend on temperature?

Amy Jiang
Amy Jiang
Numerade Educator
01:33

Problem 70

This raction is exothermic.
$$\quad C_{6} \mathrm{H}_{12} \mathrm{O}_{6}(s)+6 \mathrm{O}_{2}(g) \Longrightarrow 6 \mathrm{CO}_{2}(g)+6 \mathrm{H}_{2} \mathrm{O}(g)$$
Predict the effect (shift right, shift left, or no effect) of increasing and
decreasing the reaction temperature. How does the value of the equilibrium constant depend on temperature?

Ronald Prasad
Ronald Prasad
Numerade Educator
01:45

Problem 71

Coal, which is primarily carbon, can be converted to natural gas, primari-
ly $\mathrm{CH}_{4, \text { by the exothermic reaction: }}$
$$\mathrm{C}(s)+2 \mathrm{H}_{2}(g) \rightleftharpoons \mathrm{CH}_{4}(g)$$
Which disturbance favors $\mathrm{CH}_{4}$ at equilibrium?
\begin{equation}\begin{array}{l}{\text { a. adding more } \mathrm{C} \text { to the reaction mixture }} \\ {\text { b. adding more } \mathrm{H}_{2} \text { to the reaction mixture }} \\ {\text { c. raising the temperature of the reaction mixture }} \\ {\text { d. } \text { lowering the volume of the reaction mixture }} \\ {\text { e. adding a catalyst to the reaction mixture }} \\ {\text { f. adding neon gas to the reaction mixture }}\end{array}\end{equation}

Ronald Prasad
Ronald Prasad
Numerade Educator
02:08

Problem 72

Coal can be used to generate hydrogen gas (a potential fuel) by the endo-
thermic reaction:
$$\mathrm{C}(s)+\mathrm{H}_{2} \mathrm{O}(g) \rightleftharpoons \operatorname{cog}(g)+\mathrm{H}_{2}(g)$$
If this reaction mixture is at equilibrium, predict whether each disturbance will result in the formation of additional hydrogen gas, the formation of less hydrogen gas, or have no effect on the quantity of hydrogen
gas.
\begin{equation}
\begin{array}{l}{\text { a. adding } C \text { to the reaction mixture }} \\ {\text { b. adding } \mathrm{H}_{2} \mathrm{O} \text { to the reaction mixture }} \\ {\text { c. raising the temperature of the reaction mixture }} \\ {\text { d. increasing the volume of the reaction mixture }} \\ {\text { e. adding a catalyst to the reaction mixture }} \\ {\text { f. adding an inert gas to the reaction mixture }}\end{array}
\end{equation}

Ronald Prasad
Ronald Prasad
Numerade Educator
03:44

Problem 73

Carbon monoxide replaces oxygen in oxygenated hemoglobin according to the reaction:
$$\mathrm{HbO}_{2}(a q)+\mathrm{CO}(a q) \rightleftharpoons \mathrm{HbCO}(a q)+\mathrm{O}_{2}(a q)$$
a. Use the reactions and associated equilibrium constants at body tem-
perature to find the equilibrium constant for the reaction just shown.
$$\begin{array}{ll}{\mathrm{Hb}(a q)+\mathrm{O}_{2}(a q) \Longrightarrow \mathrm{Hb}_{2}(a q)} & {K_{c}=1.8} \\ {\mathrm{Hb}(a q)+\mathrm{CO}(a q) \rightleftharpoons \mathrm{HbCO}(a q)} & {K_{\mathrm{c}}=306}\end{array}$$
b. Suppose that an air mixture becomes polluted with carbon monoxide at a level of 0.10$\%$ . Assuming the air contains 20.0$\%$ oxygen and
that the oxygen and carbon monoxide ratios that dissolve in the
blood are identical to the ratios in the air, what is the ratio of HbCO
to HbO $_{2}$ in the bloodstream? Comment on the toxicity of carbon
monoxide.

Ronald Prasad
Ronald Prasad
Numerade Educator
07:16

Problem 74

Nitrogen monoxide is a pollutant in the lower atmosphere that
irritates the eyes and lungs and leads to the formation of acid rain.
Nitrogen monoxide forms naturally in the atmosphere according to
the endothermic reaction:
\begin{equation}\mathrm{N}_{2}(g)+\mathrm{O}_{2}(g) \rightleftharpoons 2 \mathrm{NO}(g) \quad K_{\mathrm{n}}=4.1 \times 10^{-31} \mathrm{at} 298 \mathrm{K}\end{equation}
Use the ideal gas law to calculate the concentrations of nitrogen and
oxygen present in air at a pressure of 1.0 atm and a temperature of 298
K. Assume that nitrogen composes 78$\%$ of air by volume and that oxygen composes 21$\%$ of air. Find the "natural" equilibrium concentration
of NO in air in units of molecules/cm^{3} . \text { How would you expect this concentration to change in an automobile engine in which combustion is occurring.

Ronald Prasad
Ronald Prasad
Numerade Educator
07:44

Problem 75

The reaction $\mathrm{CO}_{2}(g)+\mathrm{C}(s) \rightleftharpoons 2 \mathrm{CO}(g)$ has $\mathrm{K}_{\mathrm{p}}=5.78$ at 1200 $\mathrm{K}$
\begin{equation}\begin{array}{l}{\text { a. Calculate the total pressure at equilibrium when } 4.45 \text { g of } \mathrm{CO}_{2} \text { is in- }} \\ {\text { troduced into a } 10.0 \text { L container and heated to } 1200 \mathrm{K} \text { in the presence }} \\ {\text { of } 2.00 \mathrm{g} \text { of graphite. }} \\ {\text { b. Repeat the calculation of part a in the presence of 0.50 } \mathrm{g} \text { of graphite. }}\end{array}\end{equation}

Ronald Prasad
Ronald Prasad
Numerade Educator
10:22

Problem 76

A mixture of water and graphite is heated to 600 $\mathrm{K}$ . When the system
comes to equilibrium, it contains 0.13 mol of $\mathrm{H}_{2}, 0.13$ mol of $\mathrm{CO}, 0.43$
mol of $\mathrm{H}_{2} \mathrm{O},$ and some graphite. Some $\mathrm{O}_{2}$ is added to the system, and a
spark is applied so that the $\mathrm{H}_{2}$ reacts completely with the $\mathrm{O}_{2}$ . Find the
amount of $\mathrm{CO}$ in the flask when the system returns to equilibrium.

Bailey Mccarthy Riley
Bailey Mccarthy Riley
Numerade Educator
04:23

Problem 77

At $650 \mathrm{K},$ the reaction $\mathrm{MgCO}_{3}(s) \rightleftharpoons \mathrm{MgO}(s)+\mathrm{CO}_{2}(g)$ has
$K_{\mathrm{p}}=0.026 . \mathrm{A} 10.0 \mathrm{L}$ container at 650 $\mathrm{K}$ has 1.0 $\mathrm{g}$ of $\mathrm{MgO}(s)$ and $\mathrm{CO}_{2}$
at $\mathrm{P}=0.0260$ atm. The container is then compressed to a volume of
0.100 $\mathrm{L} .$ Find the mass of $\mathrm{MgCO}_{3}$ that is formed.

Ronald Prasad
Ronald Prasad
Numerade Educator
02:29

Problem 78

A system at equilibrium contains $\mathrm{I}_{2}(g)$ at a pressure of 0.21 $\mathrm{atm}$ and $\mathrm{I}(g)$ at
a pressure of 0.23 atm. The system is then compressed to half its volume.
Find the pressure of each gas when the system returns to equilibrium.

Bailey Mccarthy Riley
Bailey Mccarthy Riley
Numerade Educator
01:38

Problem 79

Consider the exothermic reaction:
$$\mathrm{C}_{2} \mathrm{H}_{4}(g)+\mathrm{Cl}_{2}(g) \rightleftharpoons \mathrm{C}_{2} \mathrm{H}_{4} \mathrm{Cl}_{2}(g)$$
If you were trying to maximize the amount of $\mathrm{C}_{2} \mathrm{H}_{4} \mathrm{Cl}_{2}$ produced,
which tactic might you try? Assume that the reaction mixture reaches
equilibrium.
\begin{equation}\begin{array}{l}{\text { a. increasing the reaction volume }} \\ {\text { b. removing } \mathrm{C}_{2} \mathrm{H}_{4} \mathrm{Cl}_{2} \text { from the reaction mixture as it forms }} \\ {\text { c. lowering the reaction temperature }} \\ {\text { d. adding } \mathrm{Cl}_{2}}\end{array}\end{equation}

Amy Jiang
Amy Jiang
Numerade Educator
01:41

Problem 80

Consider the endothermic reaction:
$$\mathrm{C}_{2} \mathrm{H}_{4}(g)+\mathrm{I}_{2}(g) \rightleftharpoons \mathrm{C}_{2} \mathrm{H}_{4} \mathrm{I}_{2}(g)$$
If you were trying to maximize the amount of $\mathrm{C}_{2} \mathrm{H}_{4} \mathrm{I}_{2}$ produced,
which tactic might you try? Assume that the reaction mixture reaches
equilibrium.
\begin{equation}
\begin{array}{l}{\text { a. decreasing the reaction volume }} \\ {\text { b. removing I }_{2} \text { from the reaction mixture }} \\ {\text { c. raising the reaction temperature }} \\ {\text { d. adding } C_{2} H_{4} \text { to the reaction mixture }}\end{array}
\end{equation}

Ronald Prasad
Ronald Prasad
Numerade Educator
05:13

Problem 81

Consider the reaction:
$$\quad \mathrm{H}_{2}(g)+\mathrm{I}_{2}(g) \rightleftharpoons 2 \mathrm{HI}(g)$$
A reaction mixture at equilibrium at 175 $\mathrm{K}$ contains $P_{\mathrm{H}_{2}}=0.958 \mathrm{atm}$$P_{\mathrm{I}_{2}}=0.877 \mathrm{atm},$ and $P_{\mathrm{HI}}=0.020 \mathrm{atm} . \mathrm{A}$ second reaction mixture,
also at $175 \mathrm{K},$ contains $P_{\mathrm{H}_{2}}=P_{\mathrm{I}_{2}}=0.621 \mathrm{atm},$ and $P_{\mathrm{HI}}=0.101 \mathrm{atm}$
Is the second reaction at equilibrium? If not, what will be the partial
pressure of HI when the reaction reaches equilibrium at 175 $\mathrm{K}$ ?

Ronald Prasad
Ronald Prasad
Numerade Educator
04:55

Problem 82

Consider the reaction:
$$2 \mathrm{H}_{2} \mathrm{S}(g)+\mathrm{SO}_{2}(g) \rightleftharpoons 3 \mathrm{S}(s)+2 \mathrm{H}_{2} \mathrm{O}(g)$$
A reaction mixture initially containing 0.500 $\mathrm{M} \mathrm{H}_{2} \mathrm{S}$ and 0.500 $\mathrm{M}$
$\mathrm{SO}_{2}$ contains 0.0011 $\mathrm{M} \mathrm{H}_{2} \mathrm{O}$ at a certain temperature. A second reaction mixture at the same temperature initially contains
$\left[\mathrm{H}_{2} \mathrm{S}\right]=0.250 \mathrm{M}$ and $\left[\mathrm{SO}_{2}\right]=0.325 \mathrm{M} .$ Calculate the equilibrium
concentration of $\mathrm{H}_{2} \mathrm{O}$ in the second mixture at this temperature.

Kevin Chimex
Kevin Chimex
Numerade Educator
10:06

Problem 83

Ammonia can be synthesized according to the reaction:
$\mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \rightleftharpoons 2 \mathrm{NH}_{3}(g) \quad K_{\mathrm{p}}=5.3 \times 10^{-5}$ at 725 $\mathrm{K}$
A 200.0 L reaction container initially contains 1.27 $\mathrm{kg}$ of $\mathrm{N}_{2}$ and
0.310 $\mathrm{kg}$ of $\mathrm{H}_{2}$ at 725 $\mathrm{K}$ . Assuming ideal gas behavior, calculate the
mass of $\mathrm{NH}_{3}(\mathrm{in} \mathrm{g})$ present in the reaction mixture at equilibrium.
What is the percent yield of the reaction under these conditions?

Kevin Chimex
Kevin Chimex
Numerade Educator
08:13

Problem 84

Hydrogen can be extracted from natural gas according to the reaction:$\mathrm{CH}_{4}(g)+\mathrm{CO}_{2}(g) \rightleftharpoons 2 \mathrm{CO}(g)+2 \mathrm{H}_{2}(g) \quad K_{\mathrm{p}}=45 \times 10^{2} \mathrm{at} 825 \mathrm{K}$
An 85.0 L reaction container initially contains 22.3 $\mathrm{kg}$ of $\mathrm{CH}_{4}$ and 55.4$\mathrm{kg}$ of $\mathrm{CO}_{2}$ at 825 $\mathrm{K}$ . Assuming ideal gas behavior, calculate the mass of
$\mathrm{H}_{2}($ in $\mathrm{g})$ present in the reaction mixture at equilibrium. What is the percent yield of the reaction under these conditions?

Ronald Prasad
Ronald Prasad
Numerade Educator
02:06

Problem 85

The system described by the reaction: $\mathrm{CO}(g)+\mathrm{Cl}_{2}(g) \rightleftharpoons \mathrm{COCl}_{2}(g)$
is at equilibrium at a given temperature when $P_{\mathrm{CO}}=0.30 \mathrm{atm},$
$P_{\mathrm{Cl}_{2}}=0.10 \mathrm{atm},$ and $P_{\mathrm{COCl}_{2}}=$0.60 atm. An additional pressure of$\mathrm{Cl}_{2}(g)=0.40$ atm is added. Find the pressure of $\mathrm{CO}$ when the system
returns to equilibrium.

Ronald Prasad
Ronald Prasad
Numerade Educator
03:29

Problem 86

A reaction vessel at $27^{\circ} \mathrm{C}$ contains a mixture of $\mathrm{SO}_{2}(P=3.00 \mathrm{atm})$
and $\mathrm{O}_{2}(P=1.00$ atm $) .$ When a catalyst is added, this reaction takes
place: $2 \mathrm{SO}_{2}(g)+\mathrm{O}_{2}(g) \rightleftharpoons 2 \mathrm{SO}_{3}(g)$
At equilibrium, the total pressure is 3.75 atm. Find the value of $K_{\mathrm{c}}.$

Kevin Chimex
Kevin Chimex
Numerade Educator
04:11

Problem 87

At $70 \mathrm{K}, \mathrm{CCl}_{4}$ decomposes to carbon and chlorine. The $K_{\mathrm{p}}$ for the decomposition is $0.76 .$ Find the statting pressure of $\mathrm{CCl}_{4}$ at this tempera-
ture that will produce a total pressure of 1.0 atm at equilibrium.

Ronald Prasad
Ronald Prasad
Numerade Educator
03:05

Problem 88

The equilibrium constant for the reaction
$\mathrm{SO}_{2}(g)+\mathrm{NO}_{2}(g) \rightleftharpoons \mathrm{SO}_{3}(g)+\mathrm{NO}(g)$ is $3.0 .$ Find the amount of
$\mathrm{NO}_{2}$ that must be added to 2.4 $\mathrm{mol}$ of $\mathrm{SO}_{2}$ in order to form 1.2 mol of
$\mathrm{SO}_{3}$ at equilibrium.

Ronald Prasad
Ronald Prasad
Numerade Educator
03:07

Problem 89

A sample of $\mathrm{CaCO}_{3}(s)$ is introduced into a sealed container of volume
0.654 $\mathrm{L}$ and heated to 1000 $\mathrm{K}$ until equilibrium is reached. The $K_{\mathrm{P}}$ for
the reaction $\mathrm{CaCO}_{3}(s) \rightleftharpoons \mathrm{CaO}(s)+\mathrm{CO}_{2}(g)$ is $3.9 \times 10^{-2}$ at this
temperature. Calculate the mass of $\mathrm{CaO}(s)$ that is present at equilibrium.

Amy Jiang
Amy Jiang
Numerade Educator
03:16

Problem 90

An equilibrium mixture contains $\mathrm{N}_{2} \mathrm{O}_{4},(P=0.28 \mathrm{atm})$ and
$\mathrm{NO}_{2}(P=1.1 \mathrm{atm})$ at 350 $\mathrm{K}$ . The volume of the container is doubled at
constant temperature. Calculate the equilibrium pressures of the two
gases when the system reaches a new equilibrium.

Ronald Prasad
Ronald Prasad
Numerade Educator
04:13

Problem 91

Carbon monoxide and chlorine gas react to form phosgene:
$$\mathrm{CO}(g)+\mathrm{Cl}_{2}(g) \Longrightarrow \operatorname{COCl}_{2}(g) \quad K_{\mathrm{p}}=3.10 \mathrm{at} 700 \mathrm{K}$$
If a reaction mixture initially contains 215 torr of CO and 245 torr of
$\mathrm{Cl}_{2},$ what is the mole fraction of $\mathrm{COCl}_{2}$ when equilibrium is reached?

Ronald Prasad
Ronald Prasad
Numerade Educator
07:11

Problem 92

Solid carbon can react with gaseous water to form carbon monoxide gas
and hydrogen gas. The equilibrium constant for the reaction at 700.0 $\mathrm{K}$ is
$K_{\mathrm{p}}=1.60 \times 10^{-3} .$ If a 1.55 $\mathrm{L}$ reaction vessel initially contains 145 torr
of water at 700.0 $\mathrm{K}$ in contact with excess solid carbon, find the percent
by mass of hydrogen gas of the gaseous reaction mixture at equilibrium.

Ronald Prasad
Ronald Prasad
Numerade Educator
09:03

Problem 93

Consider the reaction:
$$
2 \mathrm{NO}(g)+\mathrm{O}_{2}(g) \rightleftharpoons 2 \mathrm{NO}_{2}(g)
$$
a. A reaction mixture at $175 \mathrm{~K}$ initially contains 522 torr of $\mathrm{NO}$ and 421 torr of $\mathrm{O}_{2}$. At equilibrium, the total pressure in the reaction mixture is 748 torr. Calculate $K_{\mathrm{p}}$ at this temperature.
b. A second reaction mixture at $175 \mathrm{~K}$ initially contains 255 torr of NO and 185 torr of $\mathrm{O}_{2}$. What is the equilibrium partial pressure of $\mathrm{NO}_{2}$ in this mixture?

Ronald Prasad
Ronald Prasad
Numerade Educator
05:18

Problem 94

Consider the reaction:
$$2 \mathrm{SO}_{2}(g)+\mathrm{O}_{2}(g) \rightleftharpoons 2 \mathrm{SO}_{3}(g) \quad K_{\mathrm{p}}=0.355 \text { at } 950 \mathrm{K}$$
A 2.75 L reaction vessel at 950 $\mathrm{K}$ initially contains 0.100 $\mathrm{mol}$ of $\mathrm{SO}_{2}$
and 0.100 $\mathrm{mol}$ of $\mathrm{O}_{2} .$ Calculate the total pressure (in atmospheres) in
the reaction vessel when equilibrium is reached.

Kevin Chimex
Kevin Chimex
Numerade Educator
03:23

Problem 95

Nitrogen monoxide reacts with chlorine gas according to the reaction:
$$2 \mathrm{NO}(g)+\mathrm{Cl}_{2}(g) \rightleftharpoons 2 \mathrm{NOCl}(g) \quad K_{\mathrm{p}}=0.27 \mathrm{at} 700 \mathrm{K}$$
A reaction mixture initially contains equal partial pressures of NO and
$\mathrm{Cl}_{2} .$ At equilibrium, the partial pressure of NOCl is 115 torr. What were
the initial partial pressures of $\mathrm{NO}$ and $\mathrm{Cl}_{2} ?$

Ronald Prasad
Ronald Prasad
Numerade Educator
01:53

Problem 96

At a given temperature, a system containing $\mathrm{O}_{2}(g)$ and some oxides of
nitrogen are described by these reactions:
$$\begin{aligned} 2 \mathrm{NO}(g)+\mathrm{O}_{2}(g) \Longrightarrow 2 \mathrm{NO}_{2}(g) & K_{\mathrm{p}}=10^{4} \\ 2 \mathrm{NO}_{2}(g) & \rightleftharpoons \mathrm{N}_{2} \mathrm{O}_{4}(g) \quad K_{\mathrm{p}}=0.10 \end{aligned}$$
A pressure of 1 atm of $\mathrm{N}_{2} \mathrm{O}_{4}(g)$ is placed in a container at this tempera-
ture. Predict which, if any, component (other than $\mathrm{N}_{2} \mathrm{O}_{4}$ ) will be present
at a pressure greater than 0.2 atm at equilibrium.

Kevin Chimex
Kevin Chimex
Numerade Educator
09:24

Problem 97

A sample of pure $\mathrm{NO}_{2}$ is heated to $337^{\circ} \mathrm{C},$ at which temperature it
partially dissociates according to the equation:
$$2 \mathrm{NO}_{2}(g) \rightleftharpoons 2 \mathrm{NO}(g)+\mathrm{O}_{2}(g)$$
At equilibrium the density of the gas mixture is 0.520 $\mathrm{g} / \mathrm{L}$ at 0.750
atm. Calculate $K_{\mathrm{c}}$ for the reaction.

Ronald Prasad
Ronald Prasad
Numerade Educator
03:13

Problem 98

When $\mathrm{N}_{2} \mathrm{O}_{5}(g)$ is heated, it dissociates into $\mathrm{N}_{2} \mathrm{O}_{3}(g)$ and $\mathrm{O}_{2}(g) \mathrm{ac}-$
cording to the reaction:
$$\begin{array}{c}{\mathrm{N}_{2} \mathrm{O}_{5}(g) \Longrightarrow \mathrm{N}_{2} \mathrm{O}_{3}(g)+\mathrm{O}_{2}(g)} \\ {K_{\mathrm{c}}=7.75 \text { at a given temperature }}\end{array}$$
The $\mathrm{N}_{2} \mathrm{O}_{3}(g)$ dissociates to give $\mathrm{N}_{2} \mathrm{O}(g)$ and $\mathrm{O}_{2}(g)$ according to the
reaction:
$$\begin{array}{c}{\mathrm{N}_{2} \mathrm{O}_{3}(g) \Longrightarrow \mathrm{N}_{2} \mathrm{O}(g)+\mathrm{O}_{2}(g)} \\ {K_{c}=4.00 \text { at the same temperature }}\end{array}$$
When 4.00 mol of $\mathrm{N}_{2} \mathrm{O}_{5}(g)$ is heated in a 1.00 $\mathrm{L}$ reaction vessel to this
temperature, the concentration of $\mathrm{O}_{2}(g)$ at equilibrium is 4.50 $\mathrm{moll}$ .
Find the concentrations of all the other species in the equilibrium system.

Ronald Prasad
Ronald Prasad
Numerade Educator
09:14

Problem 99

A sample of SO $_{3}$ is introduced into an evacuated sealed container and
heated to 600 $\mathrm{K}$ . The following equilibrium is established:
$$2 \mathrm{SO}_{3}(g) \rightleftharpoons 2 \mathrm{SO}_{2}(g)+\mathrm{O}_{2}(g)$$
The total pressure in the system is 3.0 atm, and the mole fraction of $\mathrm{O}_{2}$
is $0.12 .$ Find $K_{\mathrm{p}} .$

Kevin Chimex
Kevin Chimex
Numerade Educator
03:35

Problem 100

A reaction $\mathrm{A}(g) \rightleftharpoons \mathrm{B}(g)$ has an equilibrium constant of
$1.0 \times 10^{-4} .$ For which of the initial reaction mixtures is the $x$ is small
approximation most likely to apply?
\begin{equation}\begin{array}{l}{\text { a. }[\mathrm{A}]=0.0010 \mathrm{M} ;[\mathrm{B}]=0.00 \mathrm{M}} \\ {\text { b. }[\mathrm{A}]=0.00 \mathrm{M}_{ ;}[\mathrm{B}]=0.10 \mathrm{M}} \\ {\text { c. }[\mathrm{A}]=0.10 \mathrm{M} ;[\mathrm{B}]=0.10 \mathrm{M}} \\ {\text { d. }[\mathrm{A}]=0.10 \mathrm{M}_{ ;}[\mathrm{B}]=0.00 \mathrm{M}}\end{array}
\end{equation}

Bailey Mccarthy Riley
Bailey Mccarthy Riley
Numerade Educator
03:00

Problem 101

The reaction $\mathrm{A}(g) \rightleftharpoons 2 \mathrm{B}(g)$ has an equilibrium constant of
$K_{\mathrm{c}}=1.0$ at a given temperature. If a reaction vessel contains equal ini-
tial amounts (in moles) of $\mathrm{A}$ and $\mathrm{B},$ will the direction in wessel? Explain.
action proceeds depend on the volume of the reaction vessel? Explain.

Ronald Prasad
Ronald Prasad
Numerade Educator
01:16

Problem 102

A particular reaction has an equilibrium constant of $K_{\mathrm{p}}=0.50$ . A re
action mixture is prepared in which all the reactants and products are
in their standard states. In which direction will the reaction proceed?

Ronald Prasad
Ronald Prasad
Numerade Educator
01:36

Problem 103

Consider the reaction:
$$a \mathrm{A}(g) \rightleftharpoons b \mathrm{B}(g)$$
Each of the entries in the table represents equilibrium partial pressures
of $\mathrm{A}$ and $\mathrm{B}$ under different initial conditions. What are the values of $a$
and $b$ in the reaction?

Kevin Chimex
Kevin Chimex
Numerade Educator
03:16

Problem 104

Consider the simple one-step reaction:
$$\mathrm{A}(g) \rightleftharpoons \mathrm{B}(g)$$
Since the reaction occurs in a single step, the forward reaction has a rate
of $k_{\text { fort }}[A]$ and the reverse reaction has a rate of $k_{\text { rate }}[\mathrm{B}] .$ What happens to
the rate of the forward reaction when we increase the concentration of
A? How does this explain the reason behind Le Chatelier's principle?

Ronald Prasad
Ronald Prasad
Numerade Educator