Chemistry

Kenneth W Whitten

Chapter 17

Chemical Equilibrium - all with Video Answers

Educators

Chapter Questions

Problem 1

Define and illustrate the following terms: (a) reversible reaction, (b) static equilibrium, (c) equilibrium constant.

Nicole Smina

Nicole Smina

Numerade Educator

Problem 2

Equilibrium constants do not have units. Explain.

Nicole Smina

Numerade Educator

Problem 3

Distinguish between the terms static equilibrium and dynamic equilibrium. Which kind does a chemical equilibrium represent?

Nicole Smina

Numerade Educator

Problem 4

(a) Describe three examples of static equilibrium.
(b) Describe three examples of dynamic equilibrium (besides chemical equilibrium).

Manik Pulyani

Numerade Educator

Problem 5

Explain the significance of (a) a very large value of $K$,
(b) a very small value of $K$, and
(c) a value of $K$ of about 1 .

Nicole Smina

Numerade Educator

Problem 6

What can be said about the magnitude of the equilibrium constant in a reaction whose equilibrium lies far to the right? to the left?

Nicole Smina

Numerade Educator

Problem 7

What is the relationship between equilibrium and the rates of opposing processes?

Nicole Smina

Numerade Educator

Problem 8

What does the value of an equilibrium constant tell us about the time required for the reaction to reach equilibrium?

Nicole Smina

Numerade Educator

Problem 9

When giving the value of an equilibrium constant, it is necessary also to write the balanced chemical equation. Why? Give examples to illustrate your explanation.

Nicole Smina

Numerade Educator

Problem 10

(a) How is the equilibrium constant related to the forward and reverse rate constants? (b) Can the rate expressions
for forward and reverse reactions be written from the balanced chemical equation? Explain. (c) Can the equilibrium constant expression be written from the balanced chemical equation? Explain.

Manik Pulyani

Numerade Educator

Problem 11

(a) Sketch a set of curves similar to those in Figure $17-2$ for concentration changes with time for a reaction
$$
2 \mathrm{~A}(\mathrm{~g})+\mathrm{B}(\mathrm{g}) \rightleftharpoons \mathrm{C}(\mathrm{g})+2 \mathrm{D}(\mathrm{g})
$$
assuming that $K$ is much greater than 1 . In each case, assume that $\mathrm{A}$ and $\mathrm{B}$ start at the same concentration and that no $\mathrm{C}$ or $\mathrm{D}$ are present. (b) Repeat part (a) for the case that $K$ is much less than $1 .$

Nicole Smina

Numerade Educator

Problem 12

(a) Sketch a set of curves similar to those in Figure $17-2$ for concentration changes with time for a reaction
$$
3 \mathrm{~A}(\mathrm{~g})+\mathrm{B}(\mathrm{g}) \rightleftharpoons 2 \mathrm{C}(\mathrm{g})
$$
assuming that $K$ is much greater than $1 .$ In each case, assume that $\mathrm{A}$ and $\mathrm{B}$ start at the same concentration and that no $\mathrm{C}$ is present. (b) Repeat part (a) for the case that $K$ is much less than 1

Lucy Chang

Numerade Educator

Problem 13

At some temperature, the reaction
$$
\mathrm{N}_{2}(\mathrm{~g})+3 \mathrm{H}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NH}_{3}(\mathrm{~g})
$$
has an equilibrium constant $K_{c}$ numerically equal to $1 .$ State whether each of the following is true or false, and explain
why.
(a) An equilibrium mixture must have the $\mathrm{H}_{2}$ concentration three times that of $\mathrm{N}_{2}$ and the $\mathrm{NH}_{3}$ concentration twice that of $\mathrm{H}_{2}$. (b) An equilibrium mixture must have the $\mathrm{H}_{2}$ concentration three times that of $\mathrm{N}_{2}$. (c) A mixture in which the $\mathrm{H}_{2}$ concentration is three times that of $\mathrm{N}_{2}$ and the $\mathrm{NH}_{3}$ concentration is twice that of $\mathrm{N}_{2}$ could be an equilibrium mixture. (d) A mixture in which the concentration of each reactant and each product is $1 M$ is an equilibrium mixture. (e) Any mixture in which the concentrations of all reactants and products are equal is an equilibrium mixture.
(f) An equilibrium mixture must have equal concentrations of all reactants and products.

Amruta Pandit

Numerade Educator

Problem 14

Why do we omit concentrations of pure solids and pure liquids from equilibrium constant expressions?

Nicole Smina

Numerade Educator

Problem 15

Consider the following compounds, in the states indicated, as possible reactants or products in a chemical reaction. Which of these compounds would be omitted from the equilibrium constant expression? $\mathrm{H}_{2} \mathrm{O}(\mathrm{s}), \mathrm{H}_{2} \mathrm{O}(\ell), \mathrm{H}_{2} \mathrm{O}(\mathrm{g})$,
$\mathrm{HCl}(\mathrm{g}), \mathrm{HCl}(\mathrm{aq}), \mathrm{NaHCO}_{3}(\mathrm{~s}), \mathrm{CH}_{3} \mathrm{OH}(\ell), \mathrm{CH}_{3} \mathrm{OH}(\mathrm{aq})$
$\mathrm{Cl}_{2}(\mathrm{aq}), \mathrm{N}_{2}(\mathrm{~g}), \mathrm{NH}_{3}(\ell), \mathrm{CO}(\mathrm{g})$, and $\mathrm{Fe}_{2} \mathrm{O}_{3}(\mathrm{~s}) .$

Nicole Smina

Numerade Educator

Problem 16

Consider the following compounds, in the states indicated, as possible reactants or products in a chemical reaction. Which of these compounds would be omitted from the equilibrium constant expression? Explain. $\mathrm{CaCO}_{3}(\mathrm{~s})$ $\mathrm{H}_{2} \mathrm{SO}_{4}(\ell), \mathrm{NaOH}(\mathrm{s}), \mathrm{NaOH}(\mathrm{aq}), \mathrm{O}_{2}(\mathrm{~g}), \mathrm{CH}_{3} \mathrm{COOH}(\ell)$
$\mathrm{CH}_{3} \mathrm{COOH}(\mathrm{aq}), \mathrm{HI}(\mathrm{g}), \mathrm{HCl}(\mathrm{aq}), \mathrm{I}_{2}(\mathrm{~s}), \mathrm{C}($ graphite $)$, and
$\mathrm{SO}_{3}(\mathrm{~g})$

Manik Pulyani

Numerade Educator

Problem 17

Write the expression for $K_{c}$ for each of the following reactions:
(a) $\mathrm{CO}_{2}(\mathrm{~g})+\mathrm{H}_{2}(\mathrm{~g}) \rightleftharpoons \mathrm{CO}(\mathrm{g})+\mathrm{H}_{2} \mathrm{O}(\mathrm{g})$
(b) $\mathrm{SrCO}_{3}(\mathrm{~s}) \rightleftharpoons \mathrm{SrO}(\mathrm{s})+\mathrm{CO}_{2}(\mathrm{~g})$
(c) $2 \mathrm{CHCl}_{3}(\mathrm{~g})+3 \mathrm{H}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{CH}_{4}(\mathrm{~g})+3 \mathrm{Cl}_{2}(\mathrm{~g})$
(d) $\mathrm{H}_{2}(\mathrm{~g})+\mathrm{I}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{HI}(\mathrm{g})$
(e) $2 \mathrm{NOCl}(\mathrm{g}) \rightleftharpoons 2 \mathrm{NO}(\mathrm{g})+\mathrm{Cl}_{2}(\mathrm{~g})$

Nicole Smina

Numerade Educator

Problem 18

Write the expression for $K_{c}$ for each of the following reactions:
(a) $2 \mathrm{H}_{2} \mathrm{O}(\mathrm{g})+2 \mathrm{SO}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{H}_{2} \mathrm{~S}(\mathrm{~g})+3 \mathrm{O}_{2}(\mathrm{~g})$
(b) $4 \mathrm{NH}_{3}(\mathrm{~g})+5 \mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons 4 \mathrm{NO}(\mathrm{g})+6 \mathrm{H}_{2} \mathrm{O}(\mathrm{g})$
(c) $\mathrm{PCl}_{3}(\mathrm{~g})+\mathrm{Cl}_{2}(\mathrm{~g}) \rightleftharpoons \mathrm{PCl}_{5}(\mathrm{~g})$
(d) $\mathrm{NaF}(\mathrm{s})+\mathrm{H}_{2} \mathrm{SO}_{4}(\ell) \rightleftharpoons \mathrm{NaHSO}_{4}(\mathrm{~s})+\mathrm{HF}(\mathrm{g})$
(e) $2 \mathrm{SO}_{2}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{SO}_{3}(\mathrm{~g})$

Manik Pulyani

Numerade Educator

Problem 19

Write the expression for $K_{c}$ for each of the following reactions:
(a) $2 \mathrm{CO}(\mathrm{g})+\mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{CO}_{2}(\mathrm{~g})$
(b) $2 \mathrm{NO}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NO}(\mathrm{g})+\mathrm{O}_{2}(\mathrm{~g})$
(c) $2 \mathrm{HBr}(\mathrm{g}) \rightleftharpoons \mathrm{H}_{2}(\mathrm{~g})+\mathrm{Br}_{2}(\ell)$
(d) $\mathrm{P}_{4}(\mathrm{~g})+3 \mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons \mathrm{P}_{4} \mathrm{O}_{6}(\mathrm{~s})$
(e) $\mathrm{N}_{2}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NO}(\mathrm{g})$

Nicole Smina

Numerade Educator

Problem 20

Write the expression for $K_{c}$ for each of the following reactions:
(a) $2 \mathrm{H}_{2} \mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{H}_{2} \mathrm{O}(\mathrm{g})+\mathrm{O}_{2}(\mathrm{~g})$
(b) $2 \mathrm{ZnS}(\mathrm{s})+3 \mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{Zn} \mathrm{O}(\mathrm{s})+2 \mathrm{SO}_{2}(\mathrm{~g})$
(c) $\mathrm{NH}_{3}(\mathrm{~g})+\mathrm{HCl}(\mathrm{g}) \rightleftharpoons \mathrm{NH}_{4} \mathrm{Cl}(\mathrm{s})$
(d) $\mathrm{N}_{2} \mathrm{O}_{4}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NO}_{2}(\mathrm{~g})$
(e) $2 \mathrm{Cl}_{2}(\mathrm{~g})+2 \mathrm{H}_{2} \mathrm{O}(\mathrm{g}) \rightleftharpoons 4 \mathrm{HCl}(\mathrm{g})+\mathrm{O}_{2}(\mathrm{~g})$

Nicole Smina

Numerade Educator

Problem 21

Write the expression for $K_{c}$ for each of the following reactions:
(a) $\mathrm{T} \mathrm{Cl}_{3}(\mathrm{~s}) \rightleftharpoons \mathrm{TlCl}(\mathrm{s})+\mathrm{Cl}_{2}(\mathrm{~g})$
(b) $\mathrm{CuCl}_{+}{ }^{2-}(\mathrm{aq}) \rightleftharpoons \mathrm{Cu}^{2+}(\mathrm{aq})+4 \mathrm{Cl}^{-}(\mathrm{aq})$
(c) $3 \mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{O}_{3}(\mathrm{~g})$
(d) $4 \mathrm{H}_{3} \mathrm{O}^{+}(\mathrm{aq})+2 \mathrm{Cl}^{-}(\mathrm{aq})+\mathrm{MnO}_{2}(\mathrm{~s}) \rightleftharpoons$
$\mathrm{Mn}^{2+}(\mathrm{aq})+6 \mathrm{H}_{2} \mathrm{O}(\ell)+\mathrm{Cl}_{2}(\mathrm{aq})$

Ronald Prasad

Numerade Educator

Problem 22

On the basis of the equilibrium constant values, choose the reactions in which the products are favored.
(a) $\mathrm{NH}_{3}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\ell) \rightleftharpoons \mathrm{NH}_{4}^{+}(\mathrm{aq})+\mathrm{OH}^{-}(\mathrm{aq})$
$K=1.8 \times 10^{-5}$
(b) $\mathrm{Au}^{+}(\mathrm{aq})+2 \mathrm{CN}^{-}(\mathrm{aq}) \rightleftharpoons\left[\mathrm{Au}(\mathrm{CN})_{2}\right]^{-}(\mathrm{aq})$
$K=2 . \times 10^{38}$
(c) $\mathrm{PbC}_{2} \mathrm{O}_{4}(\mathrm{~s}) \rightleftharpoons \mathrm{Pb}^{2+}(\mathrm{aq})+\mathrm{C}_{2} \mathrm{O}_{4}^{2-}(\mathrm{aq})$
$K=4.8$
(d) $\mathrm{HS}^{-}(\mathrm{aq})+\mathrm{H}^{+}(\mathrm{aq}) \rightleftharpoons \mathrm{H}_{2} \mathrm{~S}(\mathrm{aq})$
$K=1.0 \times 10^{7}$

Nicole Smina

Numerade Educator

Problem 23

On the basis of the equilibrium constant values, choose the reactions in which the reactants are favored.
(a) $\mathrm{H}_{2} \mathrm{O}(\ell) \rightleftharpoons \mathrm{H}^{+}(\mathrm{aq})+\mathrm{OH}^{-}(\mathrm{aq})$
$K=1.0 \times 10^{-14}$
(b) $\left[\mathrm{AlF}_{6}\right]^{3-}(\mathrm{aq}) \rightleftharpoons \mathrm{Al}^{3+}(\mathrm{aq})+6 \mathrm{~F}^{-}$ (aq) $\quad K=2 \times 10^{-24}$
(c) $\mathrm{Ca}_{3}\left(\mathrm{PO}_{4}\right)_{2}(\mathrm{~s}) \rightleftharpoons 3 \mathrm{Ca}^{2+}(\mathrm{aq})+2 \mathrm{PO}_{+}{ }^{3-}(\mathrm{aq})$
$K=1 . \times 10^{-25}$
(d) $2 \mathrm{Fe}^{3+}(\mathrm{aq})+3 \mathrm{~S}^{2-}(\mathrm{aq}) \rightleftharpoons \mathrm{Fe}_{2} \mathrm{~S}_{3}(\mathrm{~s}) \quad K=1 . \times 10^{8 \mathrm{~s}}$

Ronald Prasad

Numerade Educator

Problem 24

The reaction between nitrogen and oxygen to form $\mathrm{NO}(\mathrm{g})$ is represented by the chemical equation
$$
\mathrm{N}_{2}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NO}(\mathrm{g})
$$
Equilibrium concentrations of the gases at $1500 \mathrm{~K}$ are $1.7 \times 10^{-3} \mathrm{~mol} / \mathrm{L}$ for $\mathrm{O}_{2}, 6.4 \times 10^{-3} \mathrm{~mol} / \mathrm{L}$ for $\mathrm{N}_{2}$, and
$1.1 \times 10^{-5} \mathrm{~mol} / \mathrm{L}$ for $\mathrm{NO}$. Calculate the value of $K_{\mathrm{c} a t}$
$1500 \mathrm{~K}$ from these data.

Manik Pulyani

Numerade Educator

Problem 25

At elevated temperatures, $\mathrm{BrF}_{5}$ establishes the following equilibrium.
$$
2 \mathrm{BrF}_{3}(\mathrm{~g}) \rightleftharpoons \mathrm{Br}_{2}(\mathrm{~g})+5 \mathrm{~F}_{2}(\mathrm{~g})
$$
The equilibrium concentrations of the gases at $1500 \mathrm{~K}$ are $0.0064 \mathrm{~mol} / \mathrm{L}$ for $\mathrm{BrF}_{5}, 0.0018 \mathrm{~mol} / \mathrm{L}$ for $\mathrm{Br}_{2}$, and
$0.0090 \mathrm{~mol} / \mathrm{L}$ for $\mathrm{F}$, Calculate the value of $K$.

Ronald Prasad

Numerade Educator

Problem 26

At some temperature the reaction
$$
\mathrm{PCl}_{3}(\mathrm{~g})+\mathrm{Cl}_{2}(\mathrm{~g}) \rightleftharpoons \mathrm{PCl}_{5}(\mathrm{~g})
$$
is at equilibrium when the concentrations of $\mathrm{PCl}_{3}, \mathrm{Cl}_{2}$, and $\mathrm{PCl}_{5}$ are $10,9.0$, and $12 \mathrm{~mol} / \mathrm{L}$, respectively. Calculate the value of $K$. for this reaction at that temperature.

Manik Pulyani

Numerade Educator

Problem 27

For the reaction
$$
\mathrm{CO}(\mathrm{g})+\mathrm{H}_{2} \mathrm{O}(\mathrm{g}) \rightleftharpoons \mathrm{CO}_{2}(\mathrm{~g})+\mathrm{H}_{2}(\mathrm{~g})
$$
the value of the equilibrium constant, $K_{c}$, is $1.845$ at a given temperature. We place $0.500$ mole $\mathrm{CO}$ and $0.500 \mathrm{~mole} \mathrm{H}_{2} \mathrm{O}$ in a 1.00-L container at this temperature, and allow the reaction to reach equilibrium. What will be the equilibrium concentrations of all substances present?

Ronald Prasad

Numerade Educator

Problem 28

Given: $\mathrm{A}(\mathrm{g})+\mathrm{B}(\mathrm{g}) \rightleftharpoons \mathrm{C}(\mathrm{g})+2 \mathrm{D}(\mathrm{g})$
One mole of $\mathrm{A}$ and one mole of $\mathrm{B}$ are placed in a $0.400$ -liter container. After equilibrium has been established, $0.20 \mathrm{~mole}$ of $\mathrm{C}$ is present in the container. Calculate the equilibrium constant, $K_{0}$, for the reaction.

Manik Pulyani

Numerade Educator

Problem 29

Nitrogen reacts with hydrogen to form ammonia.
$$
\mathrm{N}_{2}(\mathrm{~g})+3 \mathrm{H}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NH}_{3}(\mathrm{~g})
$$
An equilibrium mixture at a given temperature is found to contain $0.31 \mathrm{~mol} / \mathrm{L} \mathrm{N}_{2}, 0.50 \mathrm{~mol} / \mathrm{L} \mathrm{H}_{2}$, and $0.14 \mathrm{~mol} / \mathrm{L}$
$\mathrm{NH}_{3} .$ Calculate the value of $K_{c}$ at the given temperature.

Ronald Prasad

Numerade Educator

Problem 30

For the following equation, $K_{c}=7.9 \times 10^{11}$ at $500 . \mathrm{K}$.
$$
\mathrm{H}_{2}(\mathrm{~g})+\mathrm{Br}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{HBr}(\mathrm{g})
$$
(a) ${ }_{2} \mathrm{H}_{2} 1 \mathrm{~g} 2+\frac{1}{2} \mathrm{Br}_{2} 1 \mathrm{~g} 2 \rightleftharpoons \mathrm{HBr}$ Ig $2 \quad K_{c}=?$
(b) $2 \mathrm{HBr}(\mathrm{g}) \rightleftharpoons \mathrm{H}_{2}(\mathrm{~g})+\mathrm{Br}_{2}(\mathrm{~g}) \quad K_{\mathrm{c}}=?$
(c) $4 \mathrm{HBr}(\mathrm{g}) \rightleftharpoons 2 \mathrm{H}_{2}(\mathrm{~g})+2 \mathrm{Br}_{2}(\mathrm{~g}) \quad K=?$

Manik Pulyani

Numerade Educator

Problem 31

The equilibrium constant for the gas-phase reaction
$$
2 \mathrm{SO}_{2}+\mathrm{O}_{2} \rightleftharpoons 2 \mathrm{SO}_{3}
$$
is $K_{c}=279$ at a given high temperature. What is the value of the equilibrium constant for each of the following reactions at this temperature?
(a) $2 \mathrm{SO}_{3} \rightleftharpoons 2 \mathrm{SO}_{2}+\mathrm{O}_{2}$
(b) $\mathrm{SO}_{2}+\frac{1}{2} \mathrm{O}_{2} \rightleftharpoons \mathrm{SO}_{3}$

Ronald Prasad

Numerade Educator

Problem 32

A A sealed tube initially contains $9.84 \times 10^{-4} \mathrm{~mol} \mathrm{H}_{2}$ and $1.38 \times 10^{-3} \mathrm{~mol} \mathrm{I}_{2} .$ It is kept at $350 .{ }^{\circ} \mathrm{C}$ until the reaction
$$
\mathrm{H}_{2}(\mathrm{~g})+\mathrm{I}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{HI}(\mathrm{g})
$$
comes to equilibrium. At equilibrium, $4.73 \times 10^{-4} \mathrm{~mol} \mathrm{I}_{2}$ is present. Calculate (a) the numbers of moles of $\mathrm{H}_{2}$ and HI present at equilibrium; (b) the equilibrium constant, $K_{c}$, for the reaction.

Ronald Prasad

Numerade Educator

Problem 33

NO and $\mathrm{O}_{2}$ are mixed in a container of fixed volume kept at $1000 \mathrm{~K}$. Their initial concentrations are $0.0200 \mathrm{~mol} / \mathrm{L}$ and $0.0300 \mathrm{~mol} / \mathrm{L}$, respectively. When the reaction
$$
2 \mathrm{NO}(\mathrm{g})+\mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NO}_{2}(\mathrm{~g})
$$
has come to equilibrium, the concentration of $\mathrm{NO}_{2}$ is $2.2 \times 10^{-3} \mathrm{~mol} / \mathrm{L}$. Calculate (a) the concentration of $\mathrm{NO}$ at equilibrium, (b) the concentration of $\mathrm{O}_{2}$ at equilibrium, and (c) the equilibrium constant, $K_{c}$, for the reaction.

Manik Pulyani

Numerade Educator

Problem 34

Antimony pentachloride decomposes in a gas-phase reaction at high temperatures.
$$
\mathrm{SbCl}_{5}(\mathrm{~g}) \rightleftharpoons \mathrm{SbCl}_{3}(\mathrm{~g})+\mathrm{Cl}_{2}(\mathrm{~g})
$$
(a) At some temperature, an equilibrium mixture in a 5.00-L container is found to contain $6.91 \mathrm{~g}$ of $\mathrm{SbCl}_{5}, 16.45 \mathrm{~g}$ of $\mathrm{SbCl}_{3}$, and $5.11 \mathrm{~g}$ of $\mathrm{Cl}_{2}$. Evaluate $K_{\mathrm{c}}$. (b) If $25.0$ grams of $\mathrm{SbCl}_{5}$ is placed in the $5.00-\mathrm{L}$ container and allowed to establish equilibrium at the temperature in part (a), what will be the equilibrium concentrations of all species?

Lucy Chang

Numerade Educator

Problem 35

At standard temperature and pressure, the reaction indicated by the following equation has an equilibrium constant, $K_{c}$ equal to $0.021 .$
Calculate the equilibrium constant, $K_{c}$, for the reverse equation.

Ronald Prasad

Numerade Educator

Problem 36

The following reaction has an equilibrium constant, $K_{c}$ equal to 1538 at $1800 .^{\circ} \mathrm{C}$
$$
2 \mathrm{NO}(\mathrm{g})+\mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NO}_{2}(\mathrm{~g})
$$
Calculate the equilibrium constant, $K_{c}$, for the reverse equation.

Nicole Smina

Numerade Educator

Problem 37

Define the reaction quotient, $Q .$ Distinguish between $Q$ and $K$.

Nicole Smina

Numerade Educator

Problem 38

Why is it useful to compare $Q$ with $K ?$ What is the situation when (a) $Q=K ?$ (b) $Q<K$ ? (c) $Q>K$ ?

Nicole Smina

Numerade Educator

Problem 39

How does the form of the reaction quotient compare with that of the equilibrium constant? What is the difference between these two expressions?

Nicole Smina

Numerade Educator

Problem 40

If the reaction quotient is larger than the equilibrium constant, what will happen to the reaction? What will happen if $Q<K ?$

Nicole Smina

Numerade Educator

Problem 41

$K_{c}=19.9$ for the reaction
$$
\mathrm{Cl}_{2}(\mathrm{~g})+\mathrm{F}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{ClF}(\mathrm{g})
$$
What will happen in a reaction mixture originally containing $\left[\mathrm{Cl}_{2}\right]=0.5 \mathrm{~mol} / \mathrm{L},\left[\mathrm{F}_{2}\right]=0.2 \mathrm{~mol} / \mathrm{L}$, and $[\mathrm{CIF}]=$
$7.3 \mathrm{~mol} / \mathrm{L} ?$

Ronald Prasad

Numerade Educator

Problem 42

The concentration equilibrium constant for the gas-phase reaction
$$
\mathrm{H}_{2} \mathrm{CO} \rightleftharpoons \mathrm{H}_{2}+\mathrm{CO}
$$
has the numerical value $0.50$ at a given temperature. $\mathrm{A}$ mixture of $\mathrm{H}_{2} \mathrm{CO}, \mathrm{H}_{2}$, and $\mathrm{CO}$ is introduced into a flask at this temperature. After a short time, analysis of a small sample of the reaction mixture shows the concentrations to be $\left[\mathrm{H}_{2} \mathrm{CO}\right]=0.50 M,\left[\mathrm{H}_{2}\right]=0.80 M$, and $[\mathrm{CO}]=0.25 M$
Classify each of the following statements about this reaction mixture as true or false.
(a) The reaction mixture is at equilibrium.
(b) The reaction mixture is not at equilibrium, but no further reaction will occur.
(c) The reaction mixture is not at equilibrium, but will move toward equilibrium by using up more $\mathrm{H}_{2} \mathrm{CO}$.
(d) The forward rate of this reaction is the same as the reverse rate.

Manik Pulyani

Numerade Educator

Problem 43

The value of $K_{c}$ at $25^{\circ} \mathrm{C}$ for
$$
\text { C(graphite) }+\mathrm{CO}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{CO}(\mathrm{g})
$$
is $3.7 \times 10^{-23}$. Describe what will happen if $3.5 \mathrm{~mol}$ of $\mathrm{CO}$ and $3.5 \mathrm{~mol}$ of $\mathrm{CO}_{2}$ are mixed in a $1.5-\mathrm{L}$ graphite container with a suitable catalyst to make the reaction "go" at this temperature.

Ronald Prasad

Numerade Educator

Problem 44

For the reaction described by the equation
$$
\mathrm{N}_{2}(\mathrm{~g})+\mathrm{C}_{2} \mathrm{H}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{HCN}(\mathrm{g})
$$
$K_{c}=2.3 \times 10^{-4}$ at $300 .{ }^{\circ} \mathrm{C}$. What is the equilibrium concentration of hydrogen cyanide if the initial concentrations of $\mathrm{N}_{2}$ and acetylene $\left(\mathrm{C}_{2} \mathrm{H}_{2}\right)$ were $3.5 \mathrm{~mol} / \mathrm{L}$ and $2.5 \mathrm{~mol} / \mathrm{L}$,
respectively?

Lucy Chang

Numerade Educator

Problem 45

The equilibrium constant, $K_{c}$, for the reaction
$$
\mathrm{Br}_{2}(\mathrm{~g})+\mathrm{F}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{BrF}(\mathrm{g})
$$
is $55.3 .$ What are the equilibrium concentrations of all these gases if the initial concentrations of bromine and fluorine were both $0.220 \mathrm{~mol} / \mathrm{L}$ ?

Ronald Prasad

Numerade Educator

Problem 46

$K_{\mathrm{c}}=96.2$ at $400 . \mathrm{K}$ for the reaction
$$
\mathrm{PCl}_{3}(\mathrm{~g})+\mathrm{Cl}_{2}(\mathrm{~g}) \rightleftharpoons \mathrm{PCl}_{5}(\mathrm{~g})
$$
What is the concentration of $\mathrm{Cl}_{2}$ at equilibrium if the initial concentrations were $0.22 \mathrm{~mol} / \mathrm{L}$ for $\mathrm{PCl}_{3}$ and $5.5 \mathrm{~mol} / \mathrm{L}$
for $\mathrm{Cl}_{2} ?$

Manik Pulyani

Numerade Educator

Problem 47

$K_{c}=5.85 \times 10^{-3}$ at $25^{\circ} \mathrm{C}$ for the reaction
$$
\mathrm{N}_{2} \mathrm{O}_{4}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NO}_{2}(\mathrm{~g})
$$
Twenty-two (22.0) grams of $\mathrm{N}_{2} \mathrm{O}_{4}$ is confined in a $5.00-\mathrm{L}$ flask at $25^{\circ} \mathrm{C}$. Calculate (a) the number of moles of $\mathrm{NO}_{2}$ present at equilibrium and (b) the percentage of the original $\mathrm{N}_{2} \mathrm{O}_{4}$ that is dissociated.

Ronald Prasad

Numerade Educator

Problem 48

The reaction of iron and water vapor results in an equilibrium
$$
3 \mathrm{Fe}(\mathrm{s})+4 \mathrm{H}_{2} \mathrm{O}(\mathrm{g}) \rightleftharpoons \mathrm{Fe}_{3} \mathrm{O}_{4}(\mathrm{~s})+4 \mathrm{H}_{2}(\mathrm{~g})
$$
and an equilibrium constant, $K_{c}$, of $4.6$ at $850 .{ }^{\circ} \mathrm{C}$. What is the concentration of hydrogen present at equilibrium if the reaction is initiated with $26 \mathrm{~g}$ of $\mathrm{H}_{2} \mathrm{O}$ and excess $\mathrm{Fe}$ in $\mathrm{a}$ $10.0$ -liter container?

Manik Pulyani

Numerade Educator

Problem 49

The reaction of iron and water vapor results in an equilibrium
$$
3 \mathrm{Fe}(\mathrm{s})+4 \mathrm{H}_{2} \mathrm{O}(\mathrm{g}) \rightleftharpoons \mathrm{Fe}_{3} \mathrm{O}_{4}(\mathrm{~s})+4 \mathrm{H}_{2}(\mathrm{~g})
$$
and an equilibrium constant, $K_{c}$, of $4.6$ at $850 .{ }^{\circ} \mathrm{C}$. What is the concentration of water present at equilibrium if the reaction is initiated with $6.5 \mathrm{~g}$ of $\mathrm{H}_{2}$ and excess iron oxide, $\mathrm{Fe}_{3} \mathrm{O}_{4}$, in a $15.0$ -liter container?

Ronald Prasad

Numerade Educator

Problem 50

Carbon dioxide reacts with hot carbon in the form of graphite. The equilibrium constant, $K_{c}$, for the reaction is $10.0$ at $850 .{ }^{\circ} \mathrm{C} .$
$$
\mathrm{CO}_{2}(\mathrm{~g})+\mathrm{C}(\text { graphite }) \rightleftharpoons 2 \mathrm{CO}(\mathrm{g})
$$
If $22.5 \mathrm{~g}$ of carbon monoxide is placed in a $2.50$ -L graphite container and heated to $850 .{ }^{\circ} \mathrm{C}$, what is the mass of carbon dioxide at equilibrium?

Manik Pulyani

Numerade Educator

Problem 51

Carbon dioxide reacts with hot carbon in the form of graphite. The equilibrium constant, $K_{c}$, for the reaction is $10.0$ at $850{ }^{\circ} \mathrm{C}$.
$$
\mathrm{CO}_{2}(\mathrm{~g})+\mathrm{C}(\text { graphite }) \rightleftharpoons 2 \mathrm{CO}(\mathrm{g})
$$
If $35.0 \mathrm{~g}$ of carbon dioxide and $65.0 \mathrm{~g}$ of graphite are placed in a 2.50-L reaction vessel and heated to $850 .{ }^{\circ} \mathrm{C}$, what is the mass of carbon monoxide at equilibrium?

Ronald Prasad

Numerade Educator

Problem 52

A $72.5$ -gram sample of HI was placed in a $1.50$ -L reaction vessel and allowed to come to equilibrium as illustrated in the following equation
$$
2 \mathrm{HI}(\mathrm{g}) \rightleftharpoons \mathrm{H}_{2}(\mathrm{~g})+\mathrm{I}_{2}(\mathrm{~g})
$$
The equilibrium constant, $K_{c}$, is $0.8$ 30. Calculate the concentration of each species present at equilibrium.

Manik Pulyani

Numerade Educator

Problem 53

State LeChatelier's Principle. Which factors have an effect on a system at equilibrium? How does the presence of a catalyst affect a system at chemical equilibrium? Explain your answer.

Nicole Smina

Numerade Educator

Problem 54

What will be the effect of increasing the total pressure on the equilibrium conditions for (a) a chemical equation that has more moles of gaseous products than gaseous reactants, (b) a chemical equation that has more moles of gaseous reactants than gaseous products, (c) a chemical equation that has the same number of moles of gaseous reactants and gaseous products, and (d) a chemical equation in which all reactants and products are pure solids, pure liquids, or in an aqueous solution?

Mubashshir Ansari

Mubashshir Ansari

Numerade Educator

Problem 55

Suppose the following exothermic reaction is allowed to reach equilibrium.
$$
\mathrm{A}(\mathrm{g})+3 \mathrm{~B}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{C}(\mathrm{g})+3 \mathrm{D}(\mathrm{g})
$$
Then we make each of the following changes, and allow the reaction to re-establish equilibrium. Tell whether the amount of $\mathrm{B}$ present at the new equilibrium will be (i) greater than, (ii) less than, or (iii) the same as the amount of $\mathrm{B}$ before the change was imposed.
(a) The temperature is decreased while the volume is kept constant;
(b) more $\mathrm{A}$ is added;
(c) more $\mathrm{C}$ is added;
(d) a small amount of $\mathrm{D}$ is removed;
(e) the pressure is increased by decreasing the volume.

Ronald Prasad

Numerade Educator

Problem 56

Suppose the following exothermic reaction is allowed to reach equilibrium.
$$
\mathrm{A}(\mathrm{g})+3 \mathrm{~B}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{C}(\mathrm{g})+3 \mathrm{D}(\mathrm{g})
$$
Then we make each of the following changes and allow the reaction to reestablish equilibrium. For each change, tell whether the value of the equilibrium constant will be
(i) greater than, (ii) less than, or (iii) the same as before the change was imposed.
(a) The temperature is increased while the volume is kept constant;
(b) more $\mathrm{A}$ is added;
(c) more $\mathrm{C}$ is added;
(d) a small amount of $\mathrm{D}$ is removed;
(e) the pressure is decreased by increasing the volume.

Mubashshir Ansari

Mubashshir Ansari

Numerade Educator

Problem 57

What would be the effect on an equilibrium mixture of $\mathrm{Br}_{2}, \mathrm{~F}_{2}$, and $\mathrm{Br} \mathrm{F}_{5}$ if the total pressure of the system were decreased?
$$
2 \mathrm{BrF}_{3}(\mathrm{~g}) \rightleftharpoons \mathrm{Br}_{2}(\mathrm{~g})+5 \mathrm{~F}_{2}(\mathrm{~g})
$$

Ronald Prasad

Numerade Educator

Problem 58

What would be the effect on an equilibrium mixture of carbon, oxygen, and carbon monoxide if the total pressure of the system were decreased?
$$
2 \mathrm{C}(\mathrm{s})+\mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{CO}(\mathrm{g})
$$

Nicole Smina

Numerade Educator

Problem 59

A weather indicator can be made with a hydrate of cobalt(II) chloride, which changes color as a result of the following reaction.
$$
\left[\mathrm{Co}\left(\mathrm{OH}_{2}\right)_{6}\right] \mathrm{Cl}_{2}(\mathrm{~s}) \rightleftharpoons\left[\mathrm{Co}\left(\mathrm{OH}_{2}\right)_{4}\right] \mathrm{Cl}_{2}(\mathrm{~s})+2 \mathrm{H}_{2} \mathrm{O}(\mathrm{g})
$$
$\mathbf{1}$
blos
Does a pink color indicate "moist" or "dry" air? Explain.

Ronald Prasad

Numerade Educator

Problem 60

Predict whether the equilibrium for the photosynthesis reaction described by the equation
$$
\begin{aligned}
6 \mathrm{CO}_{2}(\mathrm{~g})+6 \mathrm{H}_{2} \mathrm{O}() \rightleftharpoons \mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}(\mathrm{~s}) &+6 \mathrm{O}_{2}(\mathrm{~g}) \\
\Delta H^{0} &=2801.69 \mathrm{~kJ} / \mathrm{mol}
\end{aligned}
$$
would (i) shift to the right, (ii) shift to the left, or
(iii) remain unchanged if (a) $\left[\mathrm{CO}_{2}\right]$ were decreased;
(b) $P_{\mathrm{O}_{2}}$ were increased; (c) one half of the $\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}$ were removed; (d) the total pressure were decreased; (e) the temperature were increased; (f) a catalyst were added.

Mubashshir Ansari

Mubashshir Ansari

Numerade Educator

Problem 61

Q What would be the effect of increasing the temperature on each of the following systems at equilibrium?
(a) $\mathrm{H}_{2}(\mathrm{~g})+\mathrm{I}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{HI}(\mathrm{g})$
$\Delta H^{0}=-9.45 \mathrm{~kJ} / \mathrm{mol}$
(b) $\mathrm{PCl}_{5}(\mathrm{~g}) \rightleftharpoons \mathrm{PCl}_{3}(\mathrm{~g})+\mathrm{Cl}_{2}(\mathrm{~g})$
$\Delta H^{0}=92.5 \mathrm{~kJ} / \mathrm{mol}$
(c) $2 \mathrm{SO}_{2}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{SO}_{3}(\mathrm{~g}) \quad \Delta H^{0}=-198 \mathrm{~kJ} / \mathrm{mol}$
(d) $2 \mathrm{NOCl}(\mathrm{g}) \rightleftharpoons 2 \mathrm{NO}(\mathrm{g})+\mathrm{Cl}_{2}(\mathrm{~g})$
$\Delta H^{0}=75 \mathrm{~kJ} / \mathrm{mol}$
(e) $\mathrm{C}(\mathrm{s})+\mathrm{H}_{2} \mathrm{O}(\mathrm{g}) \rightleftharpoons \mathrm{CO}(\mathrm{g})+\mathrm{H}_{2}(\mathrm{~g}) \Delta H^{0}=131 \mathrm{~kJ} / \mathrm{mol}$

Ronald Prasad

Numerade Educator

Problem 62

What would be the effect of increasing the pressure by decreasing the volume on each of the following systems at equilibrium?
(a) $2 \mathrm{CO}(\mathrm{g})+\mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{CO}_{2}(\mathrm{~g})$
(b) $2 \mathrm{NO}(\mathrm{g}) \rightleftharpoons \mathrm{N}_{2}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g})$
(c) $\mathrm{N}_{2} \mathrm{O}_{4}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NO}_{2}(\mathrm{~g})$
(d) $\mathrm{Ni}(\mathrm{s})+4 \mathrm{CO}(\mathrm{g}) \rightleftharpoons \mathrm{Ni}(\mathrm{CO})_{4}(\mathrm{~g})$
(e) $\mathrm{N}_{2}(\mathrm{~g})+3 \mathrm{H}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NH}_{3}(\mathrm{~g})$

Mubashshir Ansari

Mubashshir Ansari

Numerade Educator

Problem 63

The value of $K_{c}$ is $0.020$ at $2870 .{ }^{\circ} \mathrm{C}$ for the reaction
$$
\mathrm{N}_{2}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NO}(\mathrm{g})
$$
There are $0.600$ mole of $\mathrm{N}_{2}, 0.400$ mole of $\mathrm{O}_{2}$, and $0.300$ mole of $\mathrm{NO}$ in a $1.00-$ liter container at $2870 .{ }^{\circ} \mathrm{C}$. Is the system at equilibrium or must the forward or reverse reaction occur to a greater extent to bring the system to equilibrium?

Ronald Prasad

Numerade Educator

Problem 64

Given: $\mathrm{A}(\mathrm{g})+\mathrm{B}(\mathrm{g}) \rightleftharpoons \mathrm{C}(\mathrm{g})+\mathrm{D}(\mathrm{g})$
(a) At equilibrium a $1.00$ -liter container was found to contain $1.60$ moles of $C, 1.60$ moles of $\mathrm{D}, 0.40$ mole of $\mathrm{A}$, and $0.40$ mole of $\mathrm{B} .$ Calculate the equilibrium constant for this reaction.
(b) If $0.20$ mole of $\mathrm{B}$ and $0.20 \mathrm{~mole}$ of $\mathrm{C}$ are added to this system, what will the new equilibrium concentration of A be?

Mubashshir Ansari

Mubashshir Ansari

Numerade Educator

Problem 65

Given: $\mathrm{A}(\mathrm{g})+\mathrm{B}(\mathrm{g}) \rightleftharpoons \mathrm{C}(\mathrm{g})+\mathrm{D}(\mathrm{g})$
When one mole of $\mathrm{A}$ and $\mathrm{one}$ mole of $\mathrm{B}$ are mixed and allowed to reach equilibrium at room temperature, the mixture is found to contain $\frac{2}{3}$ mole of $\mathrm{C}$.
(a) Calculate the equilibrium constant.
(b) If two moles of A were mixed with two moles of $\mathrm{B}$ and allowed to reach equilibrium, how many moles of $\mathrm{C}$ would be present at equilibrium?

Mubashshir Ansari

Mubashshir Ansari

Numerade Educator

Problem 65

Given: $\mathrm{A}(\mathrm{g})+\mathrm{B}(\mathrm{g}) \rightleftharpoons \mathrm{C}(\mathrm{g})+\mathrm{D}(\mathrm{g})$
When one mole of $\mathrm{A}$ and $\mathrm{one}$ mole of $\mathrm{B}$ are mixed and allowed to reach equilibrium at room temperature, the mixture is found to contain $\frac{2}{3}$ mole of $\mathrm{C}$.
(a) Calculate the equilibrium constant.
(b) If two moles of A were mixed with two moles of $\mathrm{B}$ and allowed to reach equilibrium, how many moles of $\mathrm{C}$ would be present at equilibrium?

Mubashshir Ansari

Mubashshir Ansari

Numerade Educator

Problem 66

Given: $\mathrm{A}(\mathrm{g}) \rightleftharpoons \mathrm{B}(\mathrm{g})+\mathrm{C}(\mathrm{g})$
(a) When the system is at equilibrium at $200 .{ }^{\circ} \mathrm{C}$, the concentrations are found to be: $[\mathrm{A}]=0.30 \mathrm{M},[\mathrm{B}]=[\mathrm{C}]=$
$0.25 M .$ Calculate $K_{c}$
(b) If the volume of the container in which the system is at equilibrium is suddenly doubled at $200 .{ }^{\circ} \mathrm{C}$, what will be the new equilibrium concentrations?
(c) Refer back to part (a). If the volume of the container is suddenly halved at $200 .{ }^{\circ} \mathrm{C}$, what will be the new equilibrium concentrations?

Mubashshir Ansari

Mubashshir Ansari

Numerade Educator

Problem 67

A The equilibrium constant, $K_{c}$ for the dissociation of phosphorus pentachloride is $9.3 \times 10^{-2}$ at $252^{\circ} \mathrm{C}$. How many moles and grams of $\mathrm{PCl}_{5}$ must be added to a $2.5$ -liter flask to obtain a $\mathrm{Cl}_{2}$ concentration of $0.17 \mathrm{M}$ ?
$$
\mathrm{PCl}_{3}(\mathrm{~g}) \rightleftharpoons \mathrm{PCl}_{3}(\mathrm{~g})+\mathrm{Cl}_{2}(\mathrm{~g})
$$

Ronald Prasad

Numerade Educator

Problem 68

At $25^{\circ} \mathrm{C}, K_{\mathrm{c}}$ is $5.84 \times 10^{-3}$ for the dissociation of dinitrogen tetroxide to nitrogen dioxide.
$$
\mathrm{N}_{2} \mathrm{O}_{4}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NO}_{2}(\mathrm{~g})
$$
(a) Calculate the equilibrium concentrations of both gases when $4.00$ grams of $\mathrm{N}_{2} \mathrm{O}_{4}$ is placed in a $2.00$ -liter flask at $25^{\circ} \mathrm{C}$.
(b) What will be the new equilibrium concentrations if the volume of the system is suddenly increased to $3.00$ liters at $25^{\circ} \mathrm{C}^{2}$
(c) What will be the new equilibrium concentrations if the volume is decreased to $1.00$ liter at $25^{\circ} \mathrm{C}$ ?

Manik Pulyani

Numerade Educator

Problem 69

Write the $K_{\mathrm{P}}$ expression for each reaction in Exercise $17 .$

Mubashshir Ansari

Mubashshir Ansari

Numerade Educator

Problem 70

Under what conditions would $K_{c}$ and $K_{p}$ for a reaction be numerically equal? Are $K_{c}$ and $K_{\mathrm{P}}$ numerically equal for any of the reactions in Exercises 17 and 18 ? Which ones?

Mubashshir Ansari

Mubashshir Ansari

Numerade Educator

Problem 71

$0.0100$ mol of $\mathrm{NH}_{4} \mathrm{Cl}$ and $0.0100 \mathrm{~mol}$ of $\mathrm{NH}_{3}$ are placed in a closed 2.00-L container and heated to $603 \mathrm{~K}$. At this temperature, all the $\mathrm{NH}_{4} \mathrm{Cl}$ vaporizes. When the reaction
$$
\mathrm{NH}_{4} \mathrm{Cl}(\mathrm{g}) \rightleftharpoons \mathrm{NH}_{3}(\mathrm{~g})+\mathrm{HCl}(\mathrm{g})
$$
has come to equilibrium, $5.8 \times 10^{-3} \mathrm{~mol}$ of $\mathrm{HCl}$ is present. Calculate (a) $K_{c}$ and (b) $K_{\mathrm{P}}$ for this reaction at $603 \mathrm{~K}$.

Mubashshir Ansari

Mubashshir Ansari

Numerade Educator

Problem 72

$\mathrm{CO}_{2}$ is passed over graphite at $500 . \mathrm{K}$. The emerging gas stream contains $4.0 \times 10^{-3}$ mol percent CO. The total pressure is $1.00 \mathrm{~atm}$. Assume that equilibrium is attained. Find $K_{\mathrm{P}}$ for the reaction
$$
\mathrm{C}(\mathrm{graphite})+\mathrm{CO}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{CO}(\mathrm{g})
$$

Mubashshir Ansari

Mubashshir Ansari

Numerade Educator

Problem 73

At $425^{\circ} \mathrm{C}$, the equilibrium partial pressures of $\mathrm{H}_{2}, \mathrm{I}_{2}$, and HI are $0.06443$ atm, $0.06540$ atm, and $0.4821$ atm, respectively. Calculate $K_{\mathrm{P}}$ for the following reaction at this temperature.
$$
2 \mathrm{HI}(\mathrm{g}) \rightleftharpoons \mathrm{H}_{2}(\mathrm{~g})+\mathrm{I}_{2}(\mathrm{~g})
$$

Shalini Tyagi

Numerade Educator

Problem 74

The equilibrium constant, $K_{\mathrm{p}}$, for the reaction indicated by the following equation is $0.715$ at $47^{\circ} \mathrm{C}$.
$$
\mathrm{N}_{2} \mathrm{O}_{4}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NO}_{2}(\mathrm{~g})
$$
Calculate the partial pressures of $\mathrm{N}_{2} \mathrm{O}_{4}$ and $\mathrm{NO}_{2}$ in an experiment in which $3.3$ moles of $\mathrm{N}_{2} \mathrm{O}_{4}$ is placed in a $5.0-\mathrm{L}$ flask and allowed to establish equilibrium at $47^{\circ} \mathrm{C}$.

Mubashshir Ansari

Mubashshir Ansari

Numerade Educator

Problem 75

The equilibrium constant, $K_{p}$, is $1.92$ at $252^{\circ} \mathrm{C}$ for the decomposition reaction of phosphorus pentachloride indicated in the following equation.
$$
\mathrm{PCl}_{3}(\mathrm{~g}) \rightleftharpoons \mathrm{PCl}_{3}(\mathrm{~g})+\mathrm{Cl}_{2}(\mathrm{~g})
$$
Calculate the partial pressures of all species present after $5.0$ moles of $\mathrm{PCl}_{5}$ is placed in an evacuated 4.0-liter container and equilibrium is reached at $252^{\circ} \mathrm{C}$.

Ronald Prasad

Numerade Educator

Problem 76

The following equilibrium partial pressures were measured at $750 .{ }^{\circ} \mathrm{C}: P_{\mathrm{H}_{2}}=0.387 \mathrm{~atm}, P_{\mathrm{CO}_{2}}=0.152 \mathrm{~atm}, P_{\mathrm{CO}}=$
$0.180 \mathrm{~atm}$, and $P_{\mathrm{H}_{2} \mathrm{O}}=0.252 \mathrm{~atm}$. What is the value of the
equilibrium constant, $K_{\mathrm{P}}$, for the reaction?
$$
\mathrm{H}_{2}+\mathrm{CO}_{2} \rightleftharpoons \mathrm{CO}+\mathrm{H}_{2} \mathrm{O}
$$

Nicole Smina

Numerade Educator

Problem 77

For the reaction
$$
\mathrm{H}_{2}(\mathrm{~g})+\mathrm{Cl}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{HCl}(\mathrm{g})
$$

Ronald Prasad

Numerade Educator

Problem 78

For the reaction
$$
\mathrm{Br}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{Br}(\mathrm{g})
$$
$K_{\mathrm{p}}=2550$. at $4000 \mathrm{~K}$. What is the value of $K_{\mathrm{e}}$ ?

Manik Pulyani

Numerade Educator

Problem 79

A stream of gas containing $\mathrm{H}_{2}$ at an initial partial pressure of $0.200 \mathrm{~atm}$ is passed through a tube in which $\mathrm{CuO}$ is kept at
500. K. The reaction
$$
\mathrm{CuO}(\mathrm{s})+\mathrm{H}_{2}(\mathrm{~g}) \rightleftharpoons \mathrm{Cu}(\mathrm{s})+\mathrm{H}_{2} \mathrm{O}(\mathrm{g})
$$
comes to equilibrium. For this reaction, $K_{\mathrm{p}}=1.6 \times 10^{9}$. What is the partial pressure of $\mathrm{H}_{2}$ in the gas leaving the tube? Assume that the total pressure of the stream is unchanged.

Mubashshir Ansari

Mubashshir Ansari

Numerade Educator

Problem 80

In the distant future, when hydrogen may be cheaper than coal, steel mills may make iron by the reaction
$$
\mathrm{Fe}_{2} \mathrm{O}_{3}(\mathrm{~s})+3 \mathrm{H}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{Fe}(\mathrm{s})+3 \mathrm{H}_{2} \mathrm{O}(\mathrm{g})
$$
For this reaction, $\Delta H^{0}=96 \mathrm{~kJ} / \mathrm{mol}$ and $K_{\mathrm{c}}=8.11$ at $1000 . \mathrm{K}$. (a) What percentage of the $\mathrm{H}_{2}$ remains unreacted after the reaction has come to equilibrium at $1000 . \mathrm{K}$ ?
(b) Is this percentage greater or less if the temperature is decreased to below $1000 . \mathrm{K} ?$

Mubashshir Ansari

Mubashshir Ansari

Numerade Educator

Problem 81

What kind of equilibrium constant can be calculated from a $\Delta G^{0}$ value for a reaction involving only gases?

Mubashshir Ansari

Mubashshir Ansari

Numerade Educator

Problem 82

What must be true of the value of $\Delta G^{0}$ for a reaction if
(a) $K \gg 1$;
(b) $K=1$;
(c) $K \ll 1 ?$

Mubashshir Ansari

Mubashshir Ansari

Numerade Educator

Problem 83

A mixture of $3.00$ mol of $\mathrm{Cl}_{2}$ and $3.00 \mathrm{~mol}$ of $\mathrm{CO}$ is enclosed in a 5.00-L flask at $600 .{ }^{\circ} \mathrm{C}$. At equilibrium, $3.3 \%$ of the $\mathrm{Cl}_{2}$ has been consumed.
$$
\mathrm{CO}(\mathrm{g})+\mathrm{Cl}_{2}(\mathrm{~g}) \rightleftharpoons \mathrm{COCl}_{2}(\mathrm{~g})
$$
(a) Calculate $K_{\mathrm{c}}$ for the reaction at $600 .{ }^{\circ} \mathrm{C}$. (b) Calculate $\Delta G^{0}$ for the reaction at this temperature.

Mubashshir Ansari

Mubashshir Ansari

Numerade Educator

Problem 84

(a) Use the tabulated thermodynamic values of $\Delta H_{f}^{0}$ and $S^{0}$ to calculate the value of $K_{\mathrm{p}}$ at $25^{\circ} \mathrm{C}$ for the gas-phase reaction
$$
\mathrm{CO}+\mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{CO}_{2}+\mathrm{H}_{2}
$$
(b) Calculate the value of $K_{\mathrm{P}}$ for this reaction at $200 .{ }^{\circ} \mathrm{C}$, by the same method as in part (a). (c) Repeat the calculation of part (a), using tabulated values of $\Delta G_{f}^{0}$.

Mubashshir Ansari

Mubashshir Ansari

Numerade Educator

Problem 85

The equilibrium constant $K_{c}$ of the reaction
$$
\mathrm{H}_{2}(\mathrm{~g})+\mathrm{Br}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{HBr}(\mathrm{g})
$$
is $1.6 \times 10^{5}$ at $1297 \mathrm{~K}$ and $3.5 \times 10^{4}$ at $1495 \mathrm{~K}$. (a) Is $\Delta H^{0}$ for this reaction positive or negative? (b) Find $K_{c}$ for the reaction
$$
\frac{1}{2} \mathbf{H}_{2}(\mathrm{~g})+\frac{1}{2} \mathrm{Br}_{2}(\mathrm{~g}) \rightleftharpoons \mathrm{HBr}(\mathrm{g})
$$
at $1297 \mathrm{~K}$. (c) Pure HBr is placed in a container of constant volume and heated to $1297 \mathrm{~K}$. What percentage of the $\mathrm{HBr}$ is decomposed to $\mathrm{H}_{2}$ and $\mathrm{Br}_{2}$ at equilibrium?

Mubashshir Ansari

Mubashshir Ansari

Numerade Educator

Problem 86

The air pollutant sulfur dioxide can be partially removed from stack gases in industrial processes and converted to sulfur trioxide, the acid anhydride of commercially important sulfuric acid. Write the equation for the reaction, using the smallest whole-number coefficients. Calculate the value of the equilibrium constant for this reaction at $25^{\circ} \mathrm{C}$, from values of $\Delta G_{i}^{0}$ in Appendix $K$.

Manik Pulyani

Numerade Educator

Problem 87

The value of $\Delta H^{0}$ for the reaction in Exercise 86 is $-197.6$ $\mathrm{kJ} / \mathrm{mol} .$ (a) Predict qualitatively (i.e., without calculation) whether the value of $K_{\mathrm{p}}$ for this reaction at $500 .{ }^{\circ} \mathrm{C}$ would be greater than, the same as, or less than the value at room temperature $\left(25^{\circ} \mathrm{C}\right) .$ (b) Now calculate the value of $K_{\mathrm{P}}$ at $500 .{ }^{\circ} \mathrm{C} .$

Mubashshir Ansari

Mubashshir Ansari

Numerade Educator

Problem 88

The following is an example of an alkylation reaction that is important in the production of isooctane $(2,2,4-$ trimethylpentane) from two components of crude oil:
isobutane and isobutene. Isooctane is an antiknock additive for gasoline. The thermodynamic equilibrium constant, $K$, for this reaction at $25^{\circ} \mathrm{C}$ is $4.3 \times 10^{6}$, and $\Delta H^{0}$ is $-78.58 \mathrm{~kJ} / \mathrm{mol}$
(a) Calculate $\Delta G^{0}$ at $25^{\circ} \mathrm{C}$.
(b) Calculate $K$ at $800 .{ }^{\circ} \mathrm{C}$.
(c) Calculate $\Delta G^{0}$ at $800 .{ }^{\circ} \mathrm{C}$.
(d) How does the spontaneity of the forward reaction at $800 .{ }^{\circ} \mathrm{C}$ compare with that at $25^{\circ} \mathrm{C}$ ?
(e) Why do you think the reaction mixture is heated in the industrial preparation of isooctane?
(f) What is the purpose of the catalyst? Does it affect the forward reaction more than the reverse reaction?

Mubashshir Ansari

Mubashshir Ansari

Numerade Educator

Problem 89

Oxygen gas dissolves in water to a small extent according to the equilibrium:
$$
\mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons \mathrm{O}_{2}(\mathrm{aq})
$$
Fish extract the dissolved $\mathrm{O}_{2}$. Without the oxygen in the water, the fish will die. The heating of water in lakes and reservoirs has led to massive fish kills caused by suffocation. Without doing actual calculations, from these facts, determine the sign of $\Delta H$ for the equilibrium as written above.

Nicole Smina

Numerade Educator

Problem 90

In the gas phase, acetic acid forms an equilibrium between the monomer and the dimer:
The equilibrium constant for the equation as written is $3.2 \times 10^{4}$ at $25^{\circ} \mathrm{C}$. Is the monomer or dimer favored at equilibrium?

Nicole Smina

Numerade Educator

Problem 91

Describe, in general terms, each of the following reactions and also characterize each as product- or reactant-favored.
(a) $\mathrm{CO}(\mathrm{g})+\frac{1}{2} \mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons \mathrm{CO}_{2}(\mathrm{~g})$
$K_{\mathrm{p}}=1.2 \times 10^{+5}$
(b) $\mathrm{H}_{2} \mathrm{O}(\mathrm{g}) \rightleftharpoons \mathrm{H}_{2}(\mathrm{~g})+\frac{1}{2} \mathrm{O}_{2}(\mathrm{~g})$
$K_{\mathrm{P}}=9.1 \times 10^{-41}$
(c) $\mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{O}(\mathrm{g})$
$K_{\mathrm{P}}=1.2 \times 10^{-10}$

Ronald Prasad

Numerade Educator

Problem 92

At $700 .{ }^{\circ} \mathrm{C}, K_{\mathrm{P}}$ is $1.50$ for the reaction
$$
\mathrm{C}(\mathrm{s})+\mathrm{CO}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{CO}(\mathrm{g})
$$
Suppose the total gas pressure at equilibrium is $1.00 \mathrm{~atm}$. What are the partial pressures of $\mathrm{CO}$ and $\mathrm{CO}_{2} ?$

Mubashshir Ansari

Mubashshir Ansari

Numerade Educator

Problem 93

At $-10 .{ }^{\circ} \mathrm{C}$, the solid compound $\mathrm{Cl}_{2}\left(\mathrm{H}_{2} \mathrm{O}\right)_{8}$ is in equilibrium with gaseous chlorine, water vapor, and ice. The partial pressures of the two gases in equilibrium with a mixture of $\mathrm{Cl}_{2}\left(\mathrm{H}_{2} \mathrm{O}\right)_{8}$ and ice are $0.20$ atm for $\mathrm{Cl}_{2}$ and $0.00262$ atm for water vapor. Find the equilibrium constant $K_{\mathrm{P}}$ for each of these reactions.
(a) $\mathrm{Cl}_{2}\left(\mathrm{H}_{2} \mathrm{O}\right)_{8}(\mathrm{~s}) \rightleftharpoons \mathrm{Cl}_{2}(\mathrm{~g})+8 \mathrm{H}_{2} \mathrm{O}(\mathrm{g})$
(b) $\mathrm{Cl}_{2}\left(\mathrm{H}_{2} \mathrm{O}\right)_{8}(\mathrm{~s}) \rightleftharpoons \mathrm{Cl}_{2}(\mathrm{~g})+8 \mathrm{H}_{2} \mathrm{O}(\mathrm{s})$
Why are your two answers so different?

Mubashshir Ansari

Mubashshir Ansari

Numerade Educator

Problem 94

A flask contains $\mathrm{NH}_{4} \mathrm{Cl}(\mathrm{s})$ in equilibrium with its decomposition products
$$
\mathrm{NH}_{4} \mathrm{Cl}(\mathrm{s}) \rightleftharpoons \mathrm{NH}_{3}(\mathrm{~g})+\mathrm{HCl}(\mathrm{g})
$$
For this reaction, $\Delta H=176 \mathrm{~kJ} / \mathrm{mol}$. How is the mass of $\mathrm{NH}_{3}$ in the flask affected by each of the following disturbances? (a) The temperature is decreased. (b) $\mathrm{NH}_{3}$ is added.
(c) HCl is added. (d) $\mathrm{NH}_{4} \mathrm{Cl}$ is added, with no appreciable change in the gas volume. (e) A large amount of $\mathrm{NH}_{4} \mathrm{Cl}$ is added, decreasing the volume available to the gases.

Manik Pulyani

Numerade Educator

Problem 95

The equilibrium constant for the reaction
$$
\mathrm{H}_{2}(\mathrm{~g})+\mathrm{Br}_{2}(\ell) \rightleftharpoons 2 \mathrm{HBr}(\mathrm{g})
$$
is $K_{\mathrm{P}}=4.5 \times 10^{18}$ at $25^{\circ} \mathrm{C}$. The vapor pressure of liquid $\mathrm{Br}_{2}$ at this temperature is $0.28 \mathrm{~atm}$.
(a) Find $K_{\mathrm{p}}$ at $25^{\circ} \mathrm{C}$ for the reaction
$$
\mathrm{H}_{2}(\mathrm{~g})+\mathrm{Br}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{HBr}(\mathrm{g})
$$
(b) How will the equilibrium in part (a) be shifted by an increase in the volume of the container if (1) liquid $\mathrm{Br}_{2}$ is absent; (2) liquid $\mathrm{Br}_{2}$ is present? Explain why the effect is different in these two cases.

Ronald Prasad

Numerade Educator

Problem 96

Given that $K_{\mathrm{p}}$ is $4.6 \times 10^{-1+}$ at $25^{\circ} \mathrm{C}$ for the reaction
$2 \mathrm{Cl}_{2}(\mathrm{~g})+2 \mathrm{H}_{2} \mathrm{O}(\mathrm{g}) \rightleftharpoons 4 \mathrm{HCl}(\mathrm{g})+\mathrm{O}_{2}(\mathrm{~g})$
$\Delta H^{0}=+115 \mathrm{~kJ} / \mathrm{mol}$
Calculate $K_{\mathrm{p}}$ and $K_{c}$ for the reaction at $400 .{ }^{\circ} \mathrm{C}$ and at $800{ }^{\circ} \mathrm{C}$.

Manik Pulyani

Numerade Educator

Problem 97

$K_{\mathrm{c}}=19.9$ for the reaction
$$
\mathrm{Cl}_{2}(\mathrm{~g})+\mathrm{F}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{ClF}(\mathrm{g})
$$
What will happen in a reaction mixture originally containing $\left[\mathrm{Cl}_{2}\right]=0.200 \mathrm{~mol} / \mathrm{L},\left[\mathrm{F}_{2}\right]=0.300 \mathrm{~mol} / \mathrm{L}$, and $[\mathrm{CIF}]=$
$0.950 \mathrm{~mol} / \mathrm{L} ?$

Ronald Prasad

Numerade Educator

Problem 98

A mixture of $\mathrm{CO}, \mathrm{H}_{2}, \mathrm{CH}_{4}$, and $\mathrm{H}_{2} \mathrm{O}$ is kept at $1133 \mathrm{~K}$ until the reaction
$$
\mathrm{CO}(\mathrm{g})+3 \mathrm{H}_{2}(\mathrm{~g}) \rightleftharpoons \mathrm{CH}_{+}(\mathrm{g})+\mathrm{H}_{2} \mathrm{O}(\mathrm{g})
$$
has come to equilibrium. The volume of the container is $0.100 \mathrm{~L} .$ The equilibrium mixture contains $1.21 \times 10^{-4} \mathrm{~mol}$ $\mathrm{CO}, 2.47 \times 10^{-4} \mathrm{~mol} \mathrm{H}_{2}, 1.21 \times 10^{-4} \mathrm{~mol} \mathrm{CH}_{4}$, and $5.63 \times$
$10^{-8} \mathrm{~mol} \mathrm{H}_{2} \mathrm{O} .$ Calculate $K_{\mathrm{e}}$ for this reaction at $1133 \mathrm{~K}$.

Manik Pulyani

Numerade Educator

Problem 99

What would the pressure of hydrogen be at equilibrium when $P_{\mathrm{WCL}}=0.012 \mathrm{~atm}$ and $\dot{P}_{\mathrm{HO}}=0.10 \mathrm{~atm} ? \mathrm{~K}_{\mathrm{p}}=1.37 \times$
$10^{21}$ at $900 . \mathrm{K}$.
$$
\mathrm{WCl}_{6}(\mathrm{~g})+3 \mathrm{H}_{2}(\mathrm{~g}) \rightleftharpoons \mathrm{W}(\mathrm{s})+6 \mathrm{HCl}(\mathrm{g})
$$

Ronald Prasad

Numerade Educator

Problem 100

When the beam of the triple beam balance stops swinging, has the balance reached a dynamic or a static equilibrium? Explain.

Nicole Smina

Numerade Educator

Problem 101

Theoretically, in closed systems all chemical reactions are reversible and can be characterized with equilibrium constants. Students attempting to correlate the information from all the chapters of a chemistry text may wonder if the reactions described in the chemical equilibrium chapters are somehow different from those used in connection with stoichiometry, gas laws, and so on. Speculate about the selection of reactions that the authors have used as illustrations in the various sections of this text.

David Collins

Numerade Educator

Problem 102

What is the relationship between the forward and reverse reactions in an equilibrium?

Manik Pulyani

Numerade Educator

Problem 103

The term "equilibrium" brings to mind the word "equal." What is the relationship between the two terms?

Nicole Smina

Numerade Educator

Problem 104

The masses of participants in a chemical equilibrium are not the same on both sides of the reaction. Does the equilibrium concept violate the Law of Conservation of Matter? Explain.

Mubashshir Ansari

Mubashshir Ansari

Numerade Educator

Problem 105

A sample of benzoic acid, a solid carbon-containing acid, is in equilibrium with an aqueous solution of benzoic acid. A tiny quantity of $\mathrm{D}_{2} \mathrm{O}$, water containing the isotope ${ }^{2} \mathrm{H}$, deuterium, is added to the solution. The solution is allowed to stand at constant temperature for several hours, after which some of the solid benzoic acid is removed and analyzed. The benzoic acid is found to contain a tiny quantity of deuterium, D, and the formula of the deuterium containing molecules is $\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{COOD}$. Explain how this can happen. (Hint: Look at the ECP plot.)

Ronald Prasad

Numerade Educator

Problem 106

Imagine yourself the size of atoms and molecules inside a beaker containing the following equilibrium mixture with a $K$ greater than 1 .
Write a brief description of what you observe around you before and after additional water is added to the mixture.

Manik Pulyani

Numerade Educator

Problem 107

Hemoglobin, Hb, has four Fe atoms per molecule that, on the average, pick up roughly three molecules of $\mathrm{O}_{2}$.
$$
\mathrm{Hb}(\mathrm{aq})+3 \mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons \mathrm{Hb}\left(\mathrm{O}_{2}\right)_{3}(\mathrm{aq})
$$
Discuss mountain (high altitude) or space sickness in terms of this equilibrium.

Mubashshir Ansari

Mubashshir Ansari

Numerade Educator

Problem 108

At room temperature, the equilibrium constant for the reaction
$$
2 \mathrm{SO}_{2}+\mathrm{O}_{2} \rightleftharpoons 2 \mathrm{SO}_{3}
$$
is $6.98 \times 10^{24}$. Calculate $\Delta G_{\text {ran }}^{0}$ and $\Delta G_{\mathrm{f}}^{0}\left(\mathrm{SO}_{3}\right)$, given the additional information that $\Delta G_{\mathrm{f}}^{0}\left(\mathrm{SO}_{2}\right)=-300.194 \mathrm{~kJ} / \mathrm{mol}$.
Check your answer by looking up $\Delta G_{\mathrm{f}}^{0}\left(\mathrm{SO}_{3}\right)$ in Appendix $\mathrm{K}$.

Mary Shields

Numerade Educator

Problem 109

At $25^{\circ} \mathrm{C}, 550.0 \mathrm{~g}$ of deuterium oxide, $\mathrm{D}_{2} \mathrm{O}(20.0 \mathrm{~g} / \mathrm{mol}$;
density $1.10 \mathrm{~g} / \mathrm{mL}$ ), and $498.5 \mathrm{~g}$ of $\mathrm{H}_{2} \mathrm{O}(18.0 \mathrm{~g} / \mathrm{mol}$; den-
sity $0.997 \mathrm{~g} / \mathrm{mL}$ ) are mixed. The volumes are additive. $47.0 \%$ of the $\mathrm{H}_{2} \mathrm{O}$ reacts to form HDO. Calculate $K_{\mathrm{c}}$ at $25^{\circ} \mathrm{C}$ for the reaction
$$
\mathrm{H}_{2} \mathrm{O}+\mathrm{D}_{2} \mathrm{O} \rightleftharpoons 2 \mathrm{HDO}
$$

Ronald Prasad

Numerade Educator

Problem 110

At its normal boiling point of $100 .{ }^{\circ} \mathrm{C}$, the heat of vaporization of water is $40.66 \mathrm{~kJ} / \mathrm{mol}$. What is the equilibrium vapor pressure of water at $75^{\circ} \mathrm{C}$ ?

Manik Pulyani

Numerade Educator

Problem 111

Use the data in the preceding exercise to calculate the temperature at which the vapor pressure of water is $1.20 \mathrm{~atm}$.

Ronald Prasad

Numerade Educator

Problem 112

Use an Internet search engine (such as http://www.google .com) to locate information on a mission to Mars and equilibrium. (a) What chemical equilibrium is associated with the Mars mission? (b) What factors influence the equilibrium in part (a)?

Ronald Prasad

Numerade Educator

Problem 113

Use an Internet search engine (such as http://www.google .com) to locate information on Max Bodenstein. What equilibrium constant or reaction did he study? What year did he publish his results?

Ronald Prasad

Numerade Educator

Problem 114

Use an Internet search engine (such as http://www.google .com) to locate information on LeChatelier. State his principle in simple terms. Give an example of LeChatelier's Principle being applied to a non-chemical equilibrium.

Ronald Prasad

Numerade Educator

Problem 115

Use an Internet search engine (such as http://www.google $.$ com to locate information on Karst formations. Describe the reaction that creates a Karst formation. Does that reaction ever establish an equilibrium?

Ronald Prasad

Numerade Educator