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Chemistry: The Molecular Nature of Matter

Neil D. Jespersen, James E. Brady, Alison Hyslop

Chapter 10

Properties of Gases - all with Video Answers

Educators

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Chapter Questions

03:28

Problem 1

If you get jabbed by a pencil, why does it hurt so much more if it's with the sharp point rather than the eraser? Explain in terms of the concepts of force and pressure.

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
05:13

Problem 2

Write expressions that could be used to form conversion factors to convert between: (a) kilopascal and atm,
(b) torr and $\mathrm{mm} \mathrm{Hg}$,
(c) bar and pascal,
(d) torr and
atm,
(e) torr and pascal, (f) bar and atm.

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
01:36

Problem 3

At $20^{\circ} \mathrm{C}$ the density of mercury is $13.6 \mathrm{~g} \mathrm{~mL}^{-1}$ and that of water is $1.00 \mathrm{~g} \mathrm{~mL}^{-1}$. At $20^{\circ} \mathrm{C}$, the vapor pressure of mercury is 0.0012 torr and that of water is 18 torr. Give and explain two reasons why water would be an inconvenient fluid to use in a Torricelli barometer.

Crystal Wang
Crystal Wang
Numerade Educator
02:23

Problem 4

What is the advantage of using a closed-end manometer, rather than an open-end one, when measuring the pressure of a trapped gas? What is the disadvantage?

Crystal Wang
Crystal Wang
Numerade Educator
03:11

Problem 5

Express the following gas laws in equation form: (a) temperature-volume law (Charles' law), (b) temperaturepressure law (Gay-Lussac's law), (c) pressure-volume law (Boyle's law),
(d) combined gas law.

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
02:35

Problem 6

Which of the four important variables in the study of the physical properties of gases are assumed to be held constant in each of the following laws? (a) Boyle's law, (b) Charles' law, (c) Gay-Lussac's law, (d) combined gas law.

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
03:26

Problem 7

Determine how to plot the two properties of gases listed with each of the following gas laws so that the graph will be a straight line: (a) temperature-volume law (Charles" law), (b) temperature-pressure law (Gay-Lussac's law),
(c) pressure-volume law (Boyle's law).

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
04:43

Problem 8

What is meant by an ideal gas? Under what conditions does a real gas behave most like an ideal gas?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
02:31

Problem 9

Explain Avogadro's principle in your own words. Explain why the volumes need to be measured at a constant temperature and pressure.

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
03:07

Problem 10

Explain why two liters of hydrogen gas and one liter of oxygen gas react to form two liters of water, when the pressures and temperatures are held constant.

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
02:14

Problem 11

State the ideal gas law in the form of an equation. What is the value of the gas constant in units of $\mathrm{L}$ atm $\mathrm{mol}^{-1} \mathrm{~K}^{-1} ?$

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
02:58

Problem 12

Using the ideal gas law, show that at STP, the molar volume of an ideal gas is $22.4 \mathrm{~L}$.

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
04:03

Problem 13

The molar mass of a gas can be determined from its mass, volume, pressure, and temperature. Derive the equation from the ideal gas law and the definition of molar mass.

Daniel Kyinakwa
Daniel Kyinakwa
Numerade Educator
03:31

Problem 14

The density of a gas can vary with pressure, volume, and temperature. Develop an equation for density from the ideal gas law.

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
01:06

Problem 15

What is partial pressure?

Madeline Currie
Madeline Currie
Numerade Educator
01:27

Problem 16

State Dalton's law of partial pressures in the form of an equation.

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
01:35

Problem 17

Define mole fraction. How is the partial pressure of a gas related to its mole fraction and the total pressure?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
04:19

Problem 18

Consider the diagrams below that illustrate three mixtures of gases $A$ and $B$. If the total pressure of the mixture is $1.00 \mathrm{~atm},$ which of the drawings corresponds to a mixture in which the partial pressure of $A$ equals 0.600 atm? What are the partial pressures of $A$ in the other mixtures? What are the partial pressures of $B$ ?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
04:12

Problem 19

Explain how a gas is collected over water. Why does the temperature of the gas need to be known to determine the pressure of the gas collected over water?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
04:08

Problem 20

What is the difference between diffusion and effusion? State Graham's law in the form of an equation.

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
01:27

Problem 21

Why does the rate of effusion scale with the square root of the density or the molecular mass of the gas?

Crystal Wang
Crystal Wang
Numerade Educator
02:22

Problem 22

Describe the model of a gas proposed by the kinetic theory of gases.

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
03:40

Problem 23

Use the kinetic molecular theory of gases to explain (a) Charles' law and (b) Boyle's law.

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
01:36

Problem 24

If the molecules of a gas at constant volume are somehow given a lower average kinetic energy, what two measurable properties of the gas will change and in what direction?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
01:22

Problem 25

Explain how raising the temperature of a gas causes it to expand at constant pressure. (Hint: Describe how the model of an ideal gas connects the increase in temperature to the gas expansion.)

Crystal Wang
Crystal Wang
Numerade Educator
02:23

Problem 26

Explain in terms of the kinetic theory how raising the temperature of a confined gas makes its pressure increase.

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
02:37

Problem 27

How does the kinetic theory explain the existence of an absolute zero, $0 \mathrm{~K}$ ?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
02:59

Problem 28

Which of the following gases has the largest value of $v_{\text {rms }}$ $25^{\circ} \mathrm{C}: \mathrm{N}_{2}, \mathrm{CO}_{2}, \mathrm{NH}_{3},$ or $\mathrm{HBr} ?$

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
02:47

Problem 29

How would you expect the rate of effusion of a gas to depend on (a) the pressure of the gas, and
(b) the temperature of the gas?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
03:14

Problem 30

Which postulates of the kinetic theory are not strictly true, and why?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
01:34

Problem 31

What does a small value for the van der Waals constant $a$ suggest about the molecules of the gas?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
01:33

Problem 32

Which of the molecules below has the larger value of the van der Waals constant $b$ ? Explain your choice.

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
01:38

Problem 33

Under the same conditions of $T$ and $V$, why is the pressure of a real gas less than the pressure the gas would exert if it were ideal? At a given $T$ and $P$, why is the volume of a real gas larger than it would be if the gas were ideal?

Crystal Wang
Crystal Wang
Numerade Educator
02:14

Problem 34

Suppose we have a mixture of helium and argon. On average, which atoms are moving faster at $25^{\circ} \mathrm{C},$ and why?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
03:51

Problem 35

Carry out the following unit conversions: (a) 1.26 atm to
torr,
(b) 740 torr to atm,
(c) 738 torr to $\mathrm{mm} \mathrm{Hg}$,
(d) $1.45 \times 10^{3} \mathrm{~Pa}$ to torr.

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
04:32

Problem 36

Carry out the following unit conversions: (a) 0.625 atm
to torr,
(b) 825 torr to atm,
(c) $62 \mathrm{~mm} \mathrm{Hg}$ to torr,
(d) $1.22 \mathrm{kPa}$ to bar.

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
02:05

Problem 37

What is the pressure in torr of the following?
(a) 0.329 atm (summit of $M \mathrm{t}$. Everest, the world's highest mountain)
(b) 0.460 atm (summit of Mt. Denali, the highest mountain in the United States)

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
02:40

Problem 38

What is the pressure in atm of each of the following? (These are the values of the pressures exerted individually by $\mathrm{N}_{2}, \mathrm{O}_{2},$ and $\mathrm{CO}_{2},$ respectively, in typical inhaled air.)
(a) 595 torr,
(b) 160 torr
(c) 0.300 torr

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
03:29

Problem 39

An open-end manometer containing mercury was connected to a vessel holding a gas at a pressure of 720 torr. The atmospheric pressure was 765 torr. Sketch a diagram of the apparatus showing the relative heights of the mercury in the two arms of the manometer. What is the difference in the heights of the mercury expressed in centimeters?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
04:14

Problem 40

An open-end manometer containing mercury was connected to a vessel holding a gas at a pressure of 820 torr. The atmospheric pressure was 750 torr. Sketch a diagram of the apparatus showing the relative heights of the mercury in the two arms of the manometer. What is the difference in the heights of the mercury expressed in centimeters?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
05:01

Problem 41

An open-end mercury manometer was connected to a flask containing a gas at an unknown pressure. The mercury in the arm open to the atmosphere was $65 \mathrm{~mm}$ higher than the mercury in the arm connected to the flask. The atmospheric pressure was 748 torr. What was the pressure of the gas in the flask (in torr)?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
04:09

Problem 42

An open-end mercury manometer was connected to a flask containing a gas at an unknown pressure. The mercury in the arm open to the atmosphere was $65 \mathrm{~mm}$ higher than the mercury in the arm connected to the flask. The atmospheric pressure was 748 torr. What was the pressure of the gas in the flask (in torr)?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
02:26

Problem 43

Suppose that in a closed-end manometer the mercury in the closed arm was $12.5 \mathrm{~cm}$ higher than the mercury in the arm connected to a vessel containing a gas. What is the pressure of the gas expressed in torr?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
03:44

Problem 44

Suppose a gas is in a vessel connected to both an open-end and a closed-end manometer. The difference in heights of the mercury in the closed-end manometer was $236 \mathrm{~mm}$, while in the open-end manometer the mercury level in the arm open to the atmosphere was $512 \mathrm{~mm}$ below the level in the arm connected to the vessel. Calculate the atmospheric pressure. (It may help to sketch the apparatus.)

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
02:53

Problem 45

A sample of nitrogen has a volume of $880 \mathrm{~mL}$ and a pressure of 740 torr. What pressure will change the volume to $550 \mathrm{~mL}$ at the same temperature?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
02:57

Problem 46

A gas has a volume of $255 \mathrm{~mL}$ at 725 torr. What volume will the gas occupy at 365 torr if the temperature of the gas doesn't change?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
03:05

Problem 47

A balloon has a volume of $2.50 \mathrm{~L}$ indoors at $22^{\circ} \mathrm{C}$. If the balloon is taken outdoors on a cold day when the air temperature is $-15^{\circ} \mathrm{C}\left(5^{\circ} \mathrm{F}\right),$ what will its volume be in liters? Assume constant air pressure within the balloon.

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
02:38

Problem 48

A gas has a volume of $3.86 \mathrm{~L}$ at $45^{\circ} \mathrm{C}$. What will the volume of the gas be if its temperature is raised to $87^{\circ} \mathrm{C}$ while its pressure is kept constant?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
04:03

Problem 49

A sample of a gas has a pressure of 854 torr at $285^{\circ} \mathrm{C}$. To what Celsius temperature must the gas be heated to double its pressure if there is no change in the volume of the gas?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
02:53

Problem 50

Before taking a trip, you check the air in a tire of your automobile and find it has a pressure of $45 \mathrm{lb}$ in. $^{-2}$ on a day when the air temperature is $12^{\circ} \mathrm{C}\left(54^{\circ} \mathrm{F}\right)$. After traveling some distance, you find that the temperature of the air in the tire has risen to $43^{\circ} \mathrm{C}$ (approximately $109{ }^{\circ} \mathrm{F}$ ). What is the air pressure in the tire at this higher temperature, expressed in units of lb in. $^{-2}$ ?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
03:36

Problem 51

A sample of helium at a pressure of 745 torr and in a volume of $2.58 \mathrm{~L}$ was heated from 24.0 to $75.0^{\circ} \mathrm{C}$. The volume of the container expanded to $2.81 \mathrm{~L}$. What was the final pressure (in torr) of the helium?

Susan Hallstrom
Susan Hallstrom
Numerade Educator
04:14

Problem 52

When a sample of neon with a volume of $648 \mathrm{~mL}$ and a pressure of 0.985 atm was heated from 16.0 to $63.0^{\circ} \mathrm{C}$, its volume became $689 \mathrm{~mL}$. What was its final pressure (in atm)?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
03:12

Problem 53

What must be the new volume of a sample of nitrogen (in
L) if $2.68 \mathrm{~L}$ at 745 torr and $24.0{ }^{\circ} \mathrm{C}$ is heated to $375.0^{\circ} \mathrm{C}$ under conditions that let the pressure change to 765 torr?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
03:35

Problem 54

When $286 \mathrm{~mL}$ of oxygen at 741 torr and $18.0{ }^{\circ} \mathrm{C}$ was warmed to $33.0^{\circ} \mathrm{C}$, the pressure became 765 torr. What was the final volume (in $\mathrm{mL}$ )?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
04:28

Problem 55

A sample of argon with a volume of $6.18 \mathrm{~L}$, a pressure of 761 torr, and a temperature of $20.0^{\circ} \mathrm{C}$ expanded to a volume of $9.45 \mathrm{~L}$ and a pressure of 373 torr. What was its final temperature in ${ }^{\circ} \mathrm{C}$ ?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
04:18

Problem 56

A sample of a refrigeration gas in a volume of $455 \mathrm{~mL},$ at a pressure of 1.51 atm and at a temperature of $25.0^{\circ} \mathrm{C}$, was compressed into a volume of $222 \mathrm{~mL}$ with a pressure of $2.00 \mathrm{~atm}$. To what temperature (in ${ }^{\circ} \mathrm{C}$ ) did it have to change?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
02:05

Problem 57

How many milliliters of $\mathrm{O}_{2}$ are consumed in the complete combustion of a sample of hexane, $\mathrm{C}_{6} \mathrm{H}_{14}$, if the reaction produces $855 \mathrm{~mL}$ of $\mathrm{CO}_{2}$ ? Assume all gas volumes are measured at the same temperature and pressure. The reaction is
$$
2 \mathrm{C}_{6} \mathrm{H}_{14}(g)+19 \mathrm{O}_{2}(g) \longrightarrow 12 \mathrm{CO}_{2}(g)+14 \mathrm{H}_{2} \mathrm{O}(g)
$$

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
02:12

Problem 58

How many milliliters of oxygen are required to react completely with $175 \mathrm{~mL}$ of $\mathrm{C}_{4} \mathrm{H}_{10}$ if the volumes of both gases are measured at the same temperature and pressure? The reaction is
$$
2 \mathrm{C}_{4} \mathrm{H}_{10}(g)+13 \mathrm{O}_{2}(g) \longrightarrow 8 \mathrm{CO}_{2}(g)+10 \mathrm{H}_{2} \mathrm{O}(g)
$$

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
03:40

Problem 59

How many milliliters of $\mathrm{O}_{2}$ measured at $27{ }^{\circ} \mathrm{C}$ and 654 torr are needed to react completely with $16.8 \mathrm{~mL}$ of $\mathrm{CH}_{4}$ measured at $35^{\circ} \mathrm{C}$ and 725 torr?

David Collins
David Collins
Numerade Educator
05:19

Problem 60

How many milliliters of $\mathrm{H}_{2} \mathrm{O}$ vapor, measured at $318^{\circ} \mathrm{C}$ and 735 torr, are formed when $33.6 \mathrm{~mL}$ of $\mathrm{NH}_{3}$ at 825 torr and $127^{\circ} \mathrm{C}$ react with oxygen according to the following equation?
$$
4 \mathrm{NH}_{3}(g)+3 \mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{~N}_{2}(g)+6 \mathrm{H}_{2} \mathrm{O}(g)
$$

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
09:12

Problem 61

Calculate the maximum number of milliliters of $\mathrm{CO}_{2}$ at 745 torr and $27^{\circ} \mathrm{C},$ that could be formed in the combustion of carbon monoxide if $0.300 \mathrm{~L}$ of $\mathrm{CO}$ at 683 torr and $25^{\circ} \mathrm{C}$ is mixed with $155 \mathrm{~mL}$ of $\mathrm{O}_{2}$ at 715 torr and $125^{\circ} \mathrm{C}$.

Daniel Kyinakwa
Daniel Kyinakwa
Numerade Educator
01:24

Problem 62

A mixture of ammonia and oxygen is prepared by combining $0.300 \mathrm{~L}$ of $\mathrm{NH}_{3}$ (measured at $0.750 \mathrm{~atm}$ and $\left.28{ }^{\circ} \mathrm{C}\right)$ with $0.220 \mathrm{~L}$ of $\mathrm{O}_{2}$ (measured at $0.780 \mathrm{~atm}$ and $\left.50{ }^{\circ} \mathrm{C}\right)$. How many milliliters of $\mathrm{N}_{2}$ (measured at $0.740 \mathrm{~atm}$ and $\left.100.0^{\circ} \mathrm{C}\right)$ could be formed if the following reaction occurs?
$$
4 \mathrm{NH}_{3}(g)+3 \mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{~N}_{2}(g)+6 \mathrm{H}_{2} \mathrm{O}(g)
$$

Crystal Wang
Crystal Wang
Numerade Educator
03:09

Problem 63

What would be the value of the gas constant $R$ in units of $\mathrm{mL}$ torr $\mathrm{mol}^{-1} \mathrm{~K}^{-1}$ ?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
04:08

Problem 64

The SI generally uses its base units to compute constants involving derived units. The SI unit for volume, for example, is the cubic meter, called the stere, because the meter is the base unit of length. We learned about the SI unit of pressure, the pascal, in this chapter. The temperature unit is the kelvin. Calculate the value of the gas constant in the SI units, $\mathrm{m}^{3} \mathrm{~Pa} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}$.

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
04:35

Problem 65

What volume in liters does $0.136 \mathrm{~g}$ of $\mathrm{O}_{2}$ occupy at $20.0^{\circ} \mathrm{C}$ and 748 torr?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
04:15

Problem 66

What volume in liters does $1.67 \mathrm{~g}$ of $\mathrm{N}_{2}$ occupy at $22.0^{\circ} \mathrm{C}$ and 756 torr?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
04:40

Problem 67

What pressure (in torr) is exerted by $10.0 \mathrm{~g}$ of $\mathrm{O}_{2}$ in a $2.50 \mathrm{~L}$ container at a temperature of $27^{\circ} \mathrm{C} ?$

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
05:04

Problem 68

If $12.0 \mathrm{~g}$ of water is converted to steam in a $3.60 \mathrm{~L}$ pressure cooker held at a temperature of $108{ }^{\circ} \mathrm{C},$ what pressure will be produced?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
05:44

Problem 69

A sample of carbon dioxide has a volume of $26.5 \mathrm{~mL}$ at $20.0^{\circ} \mathrm{C}$ and 624 torr. How many grams of $\mathrm{CO}_{2}$ are in the sample?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
05:17

Problem 70

Methane is formed in landfills by the action of certain bacteria on buried organic matter. If a sample of methane collected from a landfill has a volume of $255 \mathrm{~mL}$ at 758 torr and $27^{\circ} \mathrm{C}$, how many grams of methane are in the sample?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
05:03

Problem 71

A chemist isolated a gas in a glass bulb with a volume of $255 \mathrm{~mL}$ at a temperature of $25.0{ }^{\circ} \mathrm{C}$ and a pressure (in the bulb) of 10.0 torr. The gas weighed $12.1 \mathrm{mg}$. What is the molar mass of this gas?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
05:05

Problem 72

At $22.0^{\circ} \mathrm{C}$ and a pressure of 755 torr, a gas was found to have a density of $1.13 \mathrm{~g} \mathrm{~L}^{-1}$. Calculate its molar mass.

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
05:15

Problem 73

To three significant figures, calculate the density in $\mathrm{g} \mathrm{L}^{-1}$ of the following gases at STP: (a) $\mathrm{C}_{2} \mathrm{H}_{6}$ (ethane), (b) $\mathrm{N}_{2}$,
(c) $\mathrm{Cl}_{2}$
(d) Ar.

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
05:39

Problem 74

To three significant figures, calculate the density in $\mathrm{g} \mathrm{L}^{-1}$ of the following gases at $S T P$ :
(a) $\mathrm{Ne}$,
(b) $\mathrm{O}_{2},$
(c) $\mathrm{CH}_{4}$
(methane), (d) CF $_{4}$.

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
02:55

Problem 75

What density (in $\mathrm{g} \mathrm{L}^{-1}$ ) does oxygen have at $24.0^{\circ} \mathrm{C}$ and 742 torr?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
02:59

Problem 76

At 748.0 torr and $20.65^{\circ} \mathrm{C}$, what is the density of argon $\left(\right.$ in $\left.g \mathrm{~L}^{-1}\right) ?$

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
05:04

Problem 77

The explosive PETN, pentaerythritol tetranitrate, is one of the most powerful explosives known. It reacts with the following balanced equation
$$
\begin{aligned}
\mathrm{C}\left(\mathrm{CH}_{2} \mathrm{ONO}_{2}\right)_{4}(s) \longrightarrow 2 \mathrm{CO}(g) &+4 \mathrm{H}_{2} \mathrm{O}(g) \\
&+3 \mathrm{CO}_{2}(g)+2 \mathrm{~N}_{2}(g)
\end{aligned}
$$
How many grams of PETN will react to fill a $30.0 \mathrm{~L}$ sphere to a pressure of 720 torr at a temperature of $25^{\circ} \mathrm{C}$ ?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
05:24

Problem 78

TNT, trinitrotoluene, is an explosive that can react with the following balanced equation: $$
2 \mathrm{C}_{7} \mathrm{H}_{5} \mathrm{~N}_{3} \mathrm{O}_{6}(s) \longrightarrow 3 \mathrm{~N}_{2}(g)+5 \mathrm{H}_{2} \mathrm{O}(g)+7 \mathrm{CO}(g)+7 \mathrm{C}(s)
$$
What is the total volume of the products at 760 torr and $25^{\circ} \mathrm{C}$ if $50 \mathrm{~g}$ of TNT did explode?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
04:17

Problem 79

Propylene, $\mathrm{C}_{3} \mathrm{H}_{6},$ reacts with hydrogen under pressure to give propane, $\mathrm{C}_{3} \mathrm{H}_{8}$ :
$$
\mathrm{C}_{3} \mathrm{H}_{6}(g)+\mathrm{H}_{2}(g) \longrightarrow \mathrm{C}_{3} \mathrm{H}_{8}(g)
$$
How many liters of hydrogen (at 740 torr and $24^{\circ} \mathrm{C}$ ) react with $18.0 \mathrm{~g}$ of propylene?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
06:05

Problem 80

Nitric acid is formed when $\mathrm{NO}_{2}$ is dissolved in water.
$$
3 \mathrm{NO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow 2 \mathrm{HNO}_{3}(a q)+\mathrm{NO}(g)
$$
How many milliliters of $\mathrm{NO}_{2}$ at $25^{\circ} \mathrm{C}$ and 752 torr are needed to form $12.0 \mathrm{~g}$ of $\mathrm{HNO}_{3} ?$

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
02:36

Problem 81

A mixture of gases contains 315 torr $\mathrm{N}_{2}, 275$ torr $\mathrm{O}_{2}$, and 285 torr Ar. What is the total pressure of the mixture? What is the mole fraction of $\mathrm{O}_{2}$ in this mixture?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
02:23

Problem 82

A certain biological incubator gas mixture contains 29 torr $\mathrm{CO}_{2}, 313$ torr $\mathrm{H}_{2}, 383$ torr $\mathrm{N}_{2}$. What is the total pressure of the mixture? What is the mole fraction of $\mathrm{H}_{2}$ in this mixture?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
03:39

Problem 83

A $1.00 \mathrm{~L}$ container was filled by pumping into it $1.00 \mathrm{~L}$ of $\mathrm{N}_{2}$ at $20.0 \mathrm{~cm} \mathrm{Hg}, 1.00 \mathrm{~L}$ of $\mathrm{O}_{2}$ at 155 torr, and 1.00
$L$ of $H e$ at 0.450 atm. All volumes and pressures were measured at the same temperature. What was the total pressure inside the container after the mixture was made?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
04:24

Problem 84

A special gas mixture, BAR 97 High without $\mathrm{NO},$ is used in engine emission testing and contains $16.3 \mathrm{~atm} \mathrm{CO}_{2}$, 8270 torr $\mathrm{CO},$ and $331 \mathrm{~mm} \mathrm{Hg}$ propane with the 108 atm nitrogen. What was the total pressure in the gas cylinder?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
01:43

Problem 85

What are the mole fraction and the mole percent of oxygen in exhaled air if $P_{\mathrm{O}_{2}}$ is 116 torr and $P_{\text {total }}$ is 788 torr?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
02:06

Problem 86

A mixture of 26,000 torr $\mathrm{CO}_{2}$ and 104,000 torr $\mathrm{N}_{2}$ is sold for packaging food. What are the mole fraction and mole percent of $\mathrm{CO}_{2}$ in this mixture?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
09:31

Problem 87

A $22.4 \mathrm{~L}$ container at $0{ }^{\circ} \mathrm{C}$ contains $0.300 \mathrm{~mol} \mathrm{~N}_{2}$, $0.200 \mathrm{~mol} \mathrm{O}_{2}, 0.400 \mathrm{~mol} \mathrm{He},$ and $0.10 \mathrm{~mol} \mathrm{CO}_{2} .$ What
are the partial pressures of each of the gases in torr, atm, and bar?

Daniel Kyinakwa
Daniel Kyinakwa
Numerade Educator
04:09

Problem 88

A mixture of $\mathrm{N}_{2}, \mathrm{O}_{2},$ and $\mathrm{CO}_{2}$ has a total pressure of 740 torr. In this mixture the partial pressure of $\mathrm{N}_{2}$ is $12.0 \mathrm{~cm}$ $\mathrm{Hg}$ and the partial pressure of $\mathrm{O}_{2}$ is $4.00 \mathrm{dm} \mathrm{Hg}$. What is the partial pressure of the $\mathrm{CO}_{2} ?$

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
00:55

Problem 89

A $0.200 \mathrm{~mol}$ sample of a mixture of $\mathrm{N}_{2}$ and $\mathrm{CO}_{2}$ with a total pressure of 845 torr was exposed to an excess of solid $\mathrm{CaO},$ which reacts with $\mathrm{CO}_{2}$ according to the equation
$$
\mathrm{CaO}(s)+\mathrm{CO}_{2}(g) \longrightarrow \mathrm{CaCO}_{3}(s)
$$
After the reaction was complete, the pressure of the gas had dropped to 322 torr. How many moles of $\mathrm{CO}_{2}$ were in the original mixture? (Assume no change in volume or temperature.)

Crystal Wang
Crystal Wang
Numerade Educator
01:24

Problem 90

A sample of carbon monoxide was prepared and collected over water at a temperature of $22^{\circ} \mathrm{C}$ and a total pressure of 754 torr. It occupied a volume of $268 \mathrm{~mL}$. Calculate the partial pressure of the CO in torr as well as its dry volume (in mL) under a pressure of 1.00 atm and $25^{\circ} \mathrm{C}$

Crystal Wang
Crystal Wang
Numerade Educator
01:16

Problem 91

The methane from the landfills, Problem 10.70 , is saturated with water. What volume of "wet" methane would you have to collect at $20.0^{\circ} \mathrm{C}$ and 742 torr to be sure that the sample contains $244 \mathrm{~mL}$ of dry methane (also at 742 torr $) ?$

Crystal Wang
Crystal Wang
Numerade Educator
03:33

Problem 93

Under conditions in which the density of $\mathrm{CO}_{2}$ is $1.96 \mathrm{~g} \mathrm{~L}^{-1}$ and that of $\mathrm{N}_{2}$ is $1.25 \mathrm{~g} \mathrm{~L}^{-1}$, which gas will effuse more rapidly? What will be the ratio of the rates of effusion of $\mathrm{N}_{2}$ to $\mathrm{CO}_{2}$ ?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
01:31

Problem 94

A mixture of He and Ne needs to be separated. What will be the ratio of the rates of effusion of He and Ne?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
02:29

Problem 95

Arrange the following gases in order of increasing rate of diffusion at $25^{\circ} \mathrm{C}: \mathrm{Cl}_{2}, \mathrm{C}_{2} \mathrm{H}_{4}, \mathrm{SO}_{2}$

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
02:03

Problem 96

For the gases $\mathrm{CO}, \mathrm{CO}_{2}, \mathrm{NO},$ and $\mathrm{NO}_{2},$ which gas will effuse the fastest? Which gas the slowest? Which gases will be the most difficult to separate by effusion?

Anand Jangid
Anand Jangid
Numerade Educator
03:23

Problem 97

An unknown gas $X$ effuses 1.65 times faster than $\mathrm{C}_{3} \mathrm{H}_{8}$. What is the molecular mass of gas $X ?$

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
01:10

Problem 98

To determine the molecular mass of an unknown gas, it was determined that it effuses 1.58 times slower than argon. What is the molecular mass of the gas, and what could the gas be?
of a uniform column of water $33.9 \mathrm{ft}$ high having an area of 1.00 in. $^{2}$ at its base. (Use the following data: density of mercury $=13.6 \mathrm{~g} \mathrm{~mL}^{-1} ;$ density of water $=1.00 \mathrm{~g} \mathrm{~mL}^{-1}$; $\left.1 \mathrm{~mL}=1 \mathrm{~cm}^{3} ; 1 \mathrm{lb}=454 \mathrm{~g} ; 1 \mathrm{in.}=2.54 \mathrm{~cm} .\right)$

Crystal Wang
Crystal Wang
Numerade Educator
01:02

Problem 99

Uranium hexafluoride is a white solid that readily passes directly into the vapor state. (Its vapor pressure at $20.0{ }^{\circ} \mathrm{C}$ is 120 torr. $)$ A trace of the uranium in this compound - about $0.7 \%-$ is uranium- 235 , which can be used in a nuclear power plant. The rest of the uranium is essentially uranium- 238 , and its presence interferes with these applications for uranium-235. Gas effusion of $\mathrm{UF}_{6}$ can be used to separate the fluoride made from uranium- 235 and the fluoride made from uranium- 238 . Which hexafluoride effuses more rapidly? By how much? (You can check your answer by reading Chemistry and Current Affairs 10.1 in Section $10.6 .)$

Crystal Wang
Crystal Wang
Numerade Educator
01:38

Problem 100

A bicycle pump has a barrel that is $75.0 \mathrm{~cm}$ long (about 30 in.). If air is drawn into the pump at a pressure of 1.00 atm during the upstroke, how long must the downstroke be, in centimeters, to raise the pressure of the air to 5.50 atm (approximately the pressure in the tire of a 10 -speed bike)? Assume no change in the temperature of the air.

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
02:47

Problem 101

One of the oldest units for atmospheric pressure is $\mathrm{lb}$ in. $^{-2}$ (pounds per square inch, or psi). Calculate the numerical value of the standard atmosphere in these units to three significant figures. Calculate the mass in pounds of a uniform column of water $33.9 \mathrm{ft}$ high having an area of $1.00 \mathrm{in} .{ }^{2}$ at its base. (Use the following data: density of mercury $=13.6 \mathrm{~g} \mathrm{~mL}^{-1} ;$ density of water $=1.00 \mathrm{~g} \mathrm{~mL}^{-1}$; $1 \mathrm{~mL}=1 \mathrm{~cm}^{3} ; 1 \mathrm{lb}=454 \mathrm{~g}$
$$
\text { in. }=2.54 \mathrm{~cm} .)
$$

Crystal Wang
Crystal Wang
Numerade Educator
02:24

Problem 102

A typical automobile has a weight of approximately 3500 Ib. If the vehicle is to be equipped with tires, each of which will contact the pavement with a "footprint" that is 6.0 in. wide by 3.2 in. long, what must the gauge pressure of the air be in each tire? (Gauge pressure is the amount that the gas pressure exceeds atmospheric pressure. Assume that atmospheric pressure is $14.7 \mathrm{lb}$ in. $^{-2}$.)

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
05:11

Problem 103

Suppose you were planning to move a house by transporting it on a large trailer. The house has an estimated weight of 45.6 tons $(1$ ton $=2000 \mathrm{lb})$. The trailer is expected to weigh 8.3 tons. Each wheel of the trailer will have tires inflated to a gauge pressure of 85 psi (which is actually 85 psi above atmospheric pressure). If the area of contact between a tire and the pavement can be no larger than $100.0 \mathrm{in}^{2}(10.0$ in. $\times 10.0$ in. $),$ what is the minimum number of wheels the trailer must have? (Remember, tires are mounted in multiples of two on a trailer. Assume that atmospheric pressure is 14.7 psi.)

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
01:29

Problem 104

The motion picture Titanic described the tragedy of the collision of the ocean liner of the same name with an iceberg in the North Atlantic. The ship sank soon after the collision on April $14,1912,$ and now rests on the sea floor at a depth of $12,468 \mathrm{ft}$. Recently, the wreck was explored by the research vessel Nautile, which has successfully recovered a variety of items from the debris field surrounding the sunken ship. Calculate the pressure in atmospheres and pounds per square inch exerted on the hull of the Nautile as it explores the sea bed surrounding the Titanic. (Hint:
The height of a column of liquid required to exert a given pressure is inversely proportional to the liquid's density. Seawater has a density of approximately $1.025 \mathrm{~g} \mathrm{~mL}^{-1}$; mercury has a density of $13.6 \mathrm{~g} \mathrm{~mL}^{-1}$
$1 \mathrm{~atm}=14.7 \mathrm{lb} \mathrm{in} .^{-2} .$

Crystal Wang
Crystal Wang
Numerade Educator
03:06

Problem 105

Two flasks (which we will refer to as flask 1 and flask 2$)$ are connected to each other by a U-shaped tube filled with an oil having a density of $0.826 \mathrm{~g} \mathrm{~mL}^{-1}$. The oil level in the arm connected to flask 2 is $16.24 \mathrm{~cm}$ higher than in the arm connected to flask 1 . Flask 1 is also connected to an open-end mercury manometer. The mercury level in the arm open to the atmosphere is $12.26 \mathrm{~cm}$ higher than the level in the arm connected to flask 1 . The atmospheric pressure is $0.827 \mathrm{~atm}$. What is the pressure of the gas in flask 2 expressed in torr? (See the hint given in Problem $10.104 .$ )

A. Elizabeth Hildreth
A. Elizabeth Hildreth
Numerade Educator
02:17

Problem 106

A bubble of air escaping from a diver's mask rises from a depth of $100 \mathrm{ft}$ to the surface where the pressure is $1.00 \mathrm{~atm} .$ Initially, the bubble has a volume of $10.0 \mathrm{~mL}$. Assuming none of the air dissolves in the water, how many times larger is the bubble just as it reaches the surface? Use your answer to explain why scuba divers constantly exhale as they slowly rise from a deep dive. (The density of seawater is approximately $1.025 \mathrm{~g} \mathrm{~mL}^{-1}$; the density of mercury is $13.6 \mathrm{~g} \mathrm{~mL}^{-1}$.)

Crystal Wang
Crystal Wang
Numerade Educator
01:53

Problem 107

In a diesel engine, the fuel is ignited when it is injected into hot compressed air, heated by the compression itself. In a typical high-speed diesel engine, the chamber in the cylinder has a diameter of $10.7 \mathrm{~cm}$ and a length of $13.4 \mathrm{~cm} .$ On compression, the length of the chamber is shortened by $12.7 \mathrm{~cm}$ (a " 5 -inch stroke"). The compression of the air changes its pressure from 1.00 to $34.0 \mathrm{~atm} .$ The temperature of the air before compression is $364 \mathrm{~K}$. As a result of the compression, what will be the final air temperature (in $\mathrm{K}$ and ${ }^{\circ} \mathrm{C}$ ) just before the fuel injection?

Crystal Wang
Crystal Wang
Numerade Educator
01:15

Problem 108

Early one cool $\left(60.0^{\circ} \mathrm{F}\right)$ morning you start on a bike ride with the atmospheric pressure at $14.7 \mathrm{lb}$ in. $^{-2}$ and the tire gauge pressure at $50.0 \mathrm{lb}$ in. $^{-2}$. (Gauge pressure is the amount that the pressure exceeds atmospheric pressure.) By late afternoon, the air had warmed up considerably, and this plus the heat generated by tire friction sent the temperature inside the tire to $104^{\circ} \mathrm{F}$. What will the tire gauge now read, assuming that the volume of the air in the tire and the atmospheric pressure have not changed?

Crystal Wang
Crystal Wang
Numerade Educator
01:03

Problem 109

The range of temperatures over which an automobile tire must be able to withstand pressure changes is roughly -50 to $120^{\circ} \mathrm{F}$. If a tire is filled to $35 \mathrm{lb}$ in. $^{-2}$ at $-35^{\circ} \mathrm{F}$ (on a cold day in Alaska, for example), what will be the pressure in the tire (in the same pressure units) on a hot day in Death Valley when the temperature is $115^{\circ} \mathrm{F}$ ? (Assume that the volume of the tire does not change.)

Crystal Wang
Crystal Wang
Numerade Educator
02:50

Problem 110

A mixture was prepared in a $0.500 \mathrm{~L}$ reaction vessel from $0.300 \mathrm{~L}$ of $\mathrm{O}_{2}$ (measured at $25^{\circ} \mathrm{C}$ and $74.0 \mathrm{~cm}$ $\mathrm{Hg}$ ) and $0.400 \mathrm{~L}$ of $\mathrm{H}_{2}$ (measured at $45^{\circ} \mathrm{C}$ and 1250 torr). The mixture was ignited and the $\mathrm{H}_{2}$ and $\mathrm{O}_{2}$ reacted to form water. What was the final pressure inside the reaction vessel after the reaction was over if the temperature was held at $122^{\circ} \mathrm{C}$ ?

Crystal Wang
Crystal Wang
Numerade Educator
01:37

Problem 111

A student collected $18.45 \mathrm{~mL}$ of $\mathrm{H}_{2}$ over water at $24^{\circ} \mathrm{C}$. The water level inside the collection apparatus was 8.5 $\mathrm{cm}$ higher than the water level outside. The barometric pressure was 746 torr. How many grams of zinc had to react with $\mathrm{HCl}(a q)$ to produce the $\mathrm{H}_{2}$ that was collected?

Crystal Wang
Crystal Wang
Numerade Educator
01:49

Problem 112

A mixture of gases is prepared from $87.5 \mathrm{~g}$ of $\mathrm{O}_{2}$ and $12.7 \mathrm{~g}$ of $\mathrm{H}_{2} .$ After the reaction of $\mathrm{O}_{2}$ and $\mathrm{H}_{2}$ is complete, what is the total pressure of the mixture if its temperature is $162^{\circ} \mathrm{C}$ and its volume is $12.0 \mathrm{~L}$ ? What are the partial pressures of the gases remaining in the mixture?

Crystal Wang
Crystal Wang
Numerade Educator
03:58

Problem 113

A gas was found to have a density of $0.08747 \mathrm{mg} \mathrm{mL}^{-1}$ at $17.0^{\circ} \mathrm{C}$ and a pressure of $1.00 \mathrm{~atm} .$ What is its molecular mass? Can you tell what the gas most likely is?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
03:48

Problem 114

In one analytical procedure for determining the percentage of nitrogen in unknown compounds, weighed samples are made to decompose to $\mathrm{N}_{2}$, which is collected over water at known temperatures and pressures. The volumes of $\mathrm{N}_{2}$ are then translated into grams and then into percentages.
(a) Show that the following equation can be used to calculate the percentage of nitrogen in a sample having a mass of $W$ grams when the $\mathrm{N}_{2}$ has a volume of $V$ in $\mathrm{mL}$ and is collected over water at $t_{\mathrm{C}}$ in ${ }^{\circ} \mathrm{C}$ at a total pressure of $P$ in torr. The vapor pressure of water occurs in the equation as $P_{\mathrm{H}_{2} \mathrm{O}}^{\mathrm{o}}$
Percentage $\mathrm{N}=0.04489 \times \frac{V\left(P-P_{\mathrm{H}_{2} \mathrm{O}}^{\circ}\right)}{W\left(273+t_{\mathrm{C}}\right)}$
(b) Use this equation to calculate the percentage of nitrogen in the sample described in Problem 10.117

Crystal Wang
Crystal Wang
Numerade Educator
07:01

Problem 115

A common laboratory preparation of hydrogen on a small scale uses the reaction of zinc with hydrochloric acid. Zinc chloride is the other product.
(a) If $12.0 \mathrm{~L}$ of $\mathrm{H}_{2}$ at 765 torr and $20.0{ }^{\circ} \mathrm{C}$ is wanted, how many grams of zinc are needed, in theory?
(b) If the acid is available as $8.00 \mathrm{M} \mathrm{HCl}$, what is the minimum volume of this solution (in milliliters) required to produce the amount of $\mathrm{H}_{2}$ described in part (a)??

Daniel Kyinakwa
Daniel Kyinakwa
Numerade Educator
06:18

Problem 116

A sample of an unknown gas with a mass of $3.620 \mathrm{~g}$ was made to decompose into $2.172 \mathrm{~g}$ of $\mathrm{O}_{2}$ and $1.448 \mathrm{~g}$ of $\mathrm{S}$. Before the decomposition, this sample occupied a volume of $1120 \mathrm{~mL}$ at $75.0 \mathrm{~cm} \mathrm{Hg}$ and $25.0^{\circ} \mathrm{C}$. What is the molecular formula of this gas?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
02:49

Problem 117

A sample of a new anti-malarial drug with a mass of $0.2394 \mathrm{~g}$ was made to undergo a series of reactions that changed all of the nitrogen in the compound into $\mathrm{N}_{2}$. This gas had a volume of $18.90 \mathrm{~mL}$ when collected over water at $23.80^{\circ} \mathrm{C}$ and a pressure of 746.0 torr. At $23.80^{\circ} \mathrm{C}$, the vapor pressure of water is 22.110 torr. When $6.478 \mathrm{mg}$ of the compound was burned in pure oxygen, $17.57 \mathrm{mg}$ of $\mathrm{CO}_{2}$ and $4.319 \mathrm{mg}$ of $\mathrm{H}_{2} \mathrm{O}$ were obtained. What are the percentages of $\mathrm{C}$ and $\mathrm{H}$ in this compound?
(a) Assuming that any undetermined element is oxygen, write an empirical formula for the compound.
(b) The molecular mass of the compound was found to be 324 . What is its molecular formula?

Crystal Wang
Crystal Wang
Numerade Educator
02:22

Problem 118

The odor of a rotten egg is caused by hydrogen sulfide, $\mathrm{H}_{2} \mathrm{~S} .$ Most people can detect it at a concentration of 0.15 ppb (parts per billion), meaning $0.15 \mathrm{~L}$ of $\mathrm{H}_{2} \mathrm{~S}$ in $10^{9} \mathrm{~L}$ of space. A typical student lab is $42 \times 24 \times 8.6 \mathrm{ft}$ (a) At STP, how many liters of $\mathrm{H}_{2} \mathrm{~S}$ could be present in a typical lab to have a concentration of 0.15 ppb?
(b) How many milliliters of $0.100 \mathrm{M} \mathrm{Na}_{2} \mathrm{~S}$ would be needed to generate the amount of $\mathrm{H}_{2} \mathrm{~S}$ in part (a) by the reaction of hydrochloric acid with sodium sulfide? (Assume that all of the $\mathrm{H}_{2} \mathrm{~S}$ generated enters the atmosphere.)

Crystal Wang
Crystal Wang
Numerade Educator
04:04

Problem 119

Chlorine reacts with sulfite ion to give sulfate ion and chloride ion. How many milliliters of $\mathrm{Cl}_{2}$ gas measured at $25^{\circ} \mathrm{C}$ and 734 torr are required to react with all the $\mathrm{SO}_{3}^{2-}$ in $50.0 \mathrm{~mL}$ of $0.200 \mathrm{M} \mathrm{Na}_{2} \mathrm{SO}_{3}$ solution?

Daniel Kyinakwa
Daniel Kyinakwa
Numerade Educator
01:58

Problem 120

In an experiment designed to prepare a small amount of hydrogen by the method described in Problem 10.115 , a student was limited to using a gas-collecting bottle with a maximum capacity of $335 \mathrm{~mL}$. The method involved collecting the hydrogen over water. What are the minimum number of grams of $\mathrm{Zn}$ and the minimum number of milliliters of $6.00 M \mathrm{HCl}$ needed to produce the wet hydrogen that can exactly fit this collecting bottle at $0.932 \mathrm{~atm}$ and $25.0^{\circ} \mathrm{C} ?$

Crystal Wang
Crystal Wang
Numerade Educator
06:05

Problem 121

Carbon dioxide can be made in the lab by the reaction of hydrochloric acid with calcium carbonate. How many milliliters of $\mathrm{dry} \mathrm{CO}_{2}$ at $20.0^{\circ} \mathrm{C}$ and 745 torr can be prepared from a mixture of $12.3 \mathrm{~g}$ of $\mathrm{CaCO}_{3}$ and $185 \mathrm{~mL}$ of $0.250 \mathrm{MHCl} ?$

Daniel Kyinakwa
Daniel Kyinakwa
Numerade Educator
04:27

Problem 122

Boron forms a variety of unusual compounds with hydrogen. A chemist isolated $6.3 \mathrm{mg}$ of one of the boron hydrides in a glass bulb with a volume of $385 \mathrm{~mL}$ at $25.0{ }^{\circ} \mathrm{C}$ and a bulb pressure of 11 torr. Which of the following is likely to be its molecular formula: $\mathrm{BH}_{3}$ $\mathrm{B}_{2} \mathrm{H}_{6},$ or $\mathrm{B}_{4} \mathrm{H}_{10} ?$

Daniel Kyinakwa
Daniel Kyinakwa
Numerade Educator
01:04

Problem 123

Firefighters advise that you get out of a burning building by keeping close to the floor. We learned that carbon dioxide and most other hazardous compounds are more dense than air and they should settle to the floor. What other facts do we know that make the firefighter's advice correct?

Crystal Wang
Crystal Wang
Numerade Educator
03:22

Problem 124

Carbon dioxide is implicated in global warming. Propose ways to control or perhaps decrease the carbon dioxide content in our air. Rank each proposal based on its feasibility

Crystal Wang
Crystal Wang
Numerade Educator
00:41

Problem 125

Methane is another gas implicated in the global warming problem. It has been proposed that much of the methane in the atmosphere is from ruminating cows. Evaluate that suggestion and come up with other possible sources of methane.

Crystal Wang
Crystal Wang
Numerade Educator
06:01

Problem 126

One of the CFCs that is implicated in decreasing the ozone layer and formation of the ozone hole over Antarctica is Freon-12 or $\mathrm{CCl}_{2} \mathrm{~F}_{2} .$ Calculate the density of Freon-12 at STP and compare it to the average density of air. Suggest how Freon-12 can get into the stratosphere to threaten the ozone layer.

Daniel Kyinakwa
Daniel Kyinakwa
Numerade Educator